UNIT#08 THERMOCHEMSITRY AND ENERGETICS OF CHEMICAL REACTIONS Flashcards
Thermodynamics does NOT deal with:
➡Heat of Reaction❌
➡Rate of Reaction✅
➡Spontaneity of Reaction❌
➡Entropy of Reaction❌
If an endothermic reaction is allowed to take place very rapidly in air, the temperature of the surrounding air will:
Decrease
The exothermic process is;
Respiration
A process, which takes place on its own without any outside assistance, is termed as:
Spontaneous
The work done by expansion of gas against constant pressure is:
-PΔV
(Work done by the system is considered negative)
A state function which describes together the internal energy and product of pressure and volume is called:
Enthalpy
The enthalpy of formation of a compound is:
Either positive or negative
Enthalpy is an expression for the:
Heat Energy
Which one of the following has a standard enthalpy of formation that is zero?
Cu (s)
➡Standard Enthalpy of an element in its standard state is zero
Which of the following statement is correct:
➡ΔH is positive for exothermic reaction❌
➡ΔH is negative for endothermic reaction❌
➡The heat of neutralization of strong acid with a strong base is always the same✅
➡The enthalpy of fusion is negative❌
What is not correct about ΔHf :
➡Its value gives an idea about the relative stability of reactants and the products❌
➡It is always negative❌
➡Value depends upon the nature of bonds✅
➡ITs value may be negative or positive❌
Which of the following has a positive value of enthalpy:
Atomization
NaOH + HCl ➡ NaCl + H2O
Enthalpy change in the above reaction is called:
Enthalpy of neutralization
Enthalpy o neutralization per mole of H2SO4/Ba(OH)2 is:
-54.7 kJmol-1
Which of the following processes has always ΔH= -ve
Combustion
Heat absorbed or evolved during the chemical reaction at constant pressure is:
ΔH
The change in enthalpy of a system when one mole of the substance is completely burnt in air or oxygen is called:
Heat of combustion
Which of the following enthalpy change may be positive or negative value:
➡ΔHc
➡ΔHsolution
Neutralization of acid-base is:
➡Spontaneous
➡Exothermic
ΔH represent the enthalpy change at;
25°C and 1 atm pressure
The enthalpy changes ΔH of a process are given by the relation:
ΔE = ΔH + PΔV
A system absorbs 100kJ heat and performs 50kJ work on the surroundings. The change in internal energy of the system is:
50kJ
Which equation represents the atomization of iodine:
1/2 I2(s) ➡ I(l)
The ΔH of a reaction is recorded at:
298K
Which of the following enthalpies is always negative;
Enthalpy of neutralization
Which of the following enthalpies is always positive:
Enthalpy of sublimation
Enthalpy of reaction can be measured in;
Glass calorimeter
How much heat is evolved by 100g of water when its temperature decreases from 25°C to 5°C?
-84,00J
(q = msΔT)
➡Specific Heat o water is 4.2 J/gK
Enthalpy of combustion of food, fuel and other compounds can be measured accurately by
Bomb Calorimeter
Which enthalpy of reaction can not be determined by glass calorimeter
Enthalpy of combustion
Total Heat energy (q) can be calculated in a bomb calorimeter by using the following:
c x ΔT
(q = c x ΔT)
Which one of the following is applied to calculate lattice energy indirectly?
Born-Haber cycle
In order to determine ΔHlattice of ionic compound which is the correct relationship?
ΔHlattice = ΔHf - ΔHx
Which equation shows the lattice energy of an ionic compound?
ΔH (lattice) = Hf - Hx
With the increase in charge to size ratio of ions, the lattice energy:
Increases
(ΔHlattice ∝ Charge/Size of an atom)
Hess’s law is analogous to;
Law of heat summation
Which of the following enthalpies of formation cannot be measured directly?
➡ΔH lattice for the ionic compound
➡ΔH for CO
➡ΔH for B2O3
The standard enthalpy changes of formation of carbon dioxide and water are -394kJmol-1 and -286kJmol-1 respectively, if the standard enthalpy change of combustion of propyne, C3H4 is -1932kJmol-1. What is the standard enthalpy change of formation?
-184 kJmol-1
The heat of combustion o ethane (C2H6) is -337.0 kcal at 25°C. The heat reaction when 3g of ethane is burnt completely is:
-33.7 kcal
Hess’s law is known as:
Law of heat summation
Relation between qp and qv:
qp > qv
The formation of SO3 from SO2 is ___ reaction.
Endothermic
For strong acid and strong base neutralization energy:
Constant
Unit of energy:
➡Joule
➡Kilojoule
➡Calorie
The unavailability of methods to find out the heat of reactions accurately makes thermochemistry
A limited field of study
Which one of the following is not an example of a state function?
Heat (q)
Temperature and volume in an experiment are part of :
State of a system
In endothermic reaction heat is absorbed from:
Surrounding
ΔH for the exothermic reaction is:
Negative
Which of the following condition is constant in the bomb calorimeter;
Volume
Heat exchanged between the system and surrounding at constant volume is shown by the relation
ΔH = qv + w
At constant volume, the heat supplied is equal to:
Internal energy change
Work done on the system is:
Positive
Which one is not a state function:
Work
Heat supplied at constant pressure equals:
Enthalpy
Enthalpy is the sum of the internal energy and:
Work done
Heat o a solution for the substance whose solubility decreases with an increase in temperature is:
Negative
Enthalpy change of solution of Na2CO2 is a ____ reaction
Exothermic reaction
An enthalpy cycle used to calculate the lattice energy is;
Born Haber cycle
Energy for the endothermic reaction is given a ___ value:
Positive
Which is correct for 1st law of thermodynamics?
ΔE = q +W
The energy of products is greater in:
Endothermic Reaction
Amount of heat absorbed by 2kg of water when temperature changes by 10°C are:
84,000
(q = msΔT)
When a bond is formed, energy is;
Released
Which one is the state function?
PTVUHSG
What is the value of one calorie in Joule?
4.18J
The formation of carbon dioxide hinders calculating the heat of formation of;
CO
Decomposition of water into hydrogen and oxygen is a:
Endothermic Reaction
The heat of the formation of CO
-110 kJ/mol
When 40J heat is provided and 20J work is done, if the initial energy is 10J then the final internal energy is;
30J
In glass calorimeter, which is constant
Pressure
A spontaneous process is;
➡Unidirectional and Irreversible
➡Unidirectional and Real
➡Irreversible and Real
ΔH will be given a negative sign in:
Exothermic Reaction
Reactants have high energy than products;
Exothermic Reaction
The reaction of water with quick lime results in a rise in the temperature of the system. Using the concentration change, indicate the nature of reaction.
Exothermic Reaction
Which of the following enthalpy change is always exothermic?
Enthalpy of Combustion
The heat of formation of MgO is given below.
Mg + 1/2 O2 ➡MgO ΔH=-692 kJ/mol. This equation shows that:
The product is very stable
When one mole of gaseous hydrogen ions are dissolved in water to form an infinitely dilute solution, the amount of heat liberated is;
-1075 kJ/mol
In standard enthalpy of atomization heat of surrounding:
Decreases
The heat of formation (ΔH) for CO2 is;
-394 kJ/mol
2H2 + O2 ➡2H2O ΔH=205.5 kJ/mol
What will be the enthalpy change in the above reaction:
-205.5 kJ/mol
1/2 H2(g) ➡ H(g) ΔH=218 kJ/mol
In this reaction ΔH will be called:
Enthalpy of atomization
Determine the value of enthalpy of formation of NH4Cl:
-692 kJmol-1
Enthalpy is measured at:
298K and 1 atm
When two moles of H2 and one mole of O2 react to form H2O 484 KJ heat is evolved what is ΔHf for one mole of H2O
-242 KJmol-1
The lattice energy of an ionic crystal is the enthalpy of
Formation
The thermal energy at constant pressure is called:
Enthalpy
The born-Haber cycle is used to determine the lattice energies of;
Ionic Solids
One calorie is equal to;
4.18J
The net change in energy in a chemical reaction is the same whether it takes place directly or indirectly. It is called:
Hess’s Law
The enthalpy of formation of an ionic compound is -392kJ/mol. Total energy changes (ΔHx) involved in the formation of gaseous ions from normal physical state is 280kJ/mol. The enthalpy of lattice is:
-672 kJ/mol
Enthalpy of neutralization of strong acids and bases is same because:
H+ and OH- combine to form H2O
Unit of heat is SI system is:
J
If there is the interconversion of solid and liquid states then:
➡ΔV = 0
➡ΔH = ΔE
First law of thermodynamics relates:
➡Internal Energy
➡Heat
➡Work
An exothermic process is:
O (g) + 1e- ➡O-1
If an endothermic reaction is allowed to take place very rapidly in air the temperature of the surrounding air:
Decreases
Which of the following sets constitutes of all the state functions of system:
➡Enthalpy
➡Entropy
➡Internal Energy
___ is not a state function.
Heat
Which of the following enthalpy change (ΔH) is always endothermic
ΔH (atomization)
Incorrect statement about endothermic reaction is;
➡Evaporation is an endothermic process❌
➡Products are more stable than reactants✅
➡ΔH is positive❌
➡Reaction mixture becomes stable❌
Among the following changes, which is exothermic?
➡Freezing
➡Condensation
➡Combustion
Which of the following process will be spontaneous and endothermic:
➡Melting of ice
➡Evaporation of water
➡Dissolution of NH4Cl
When water is added to quicklime, the reaction is:
Explosive
Which is non-spontaneous reaction?
N2 + O2 ➡2NO
The sum of all the energies of atoms, molecules or ions within a system is called:
Internal Energy
Which statement is true when liquid is converted into vapors?
Heat is absorbed
When ΔE of a system increases, then which of the following possibilities is correct?
➡Temperature of the system can increase
➡Phase change may take place
➡Chemical reaction can occur
ΔH = ΔE for which of the following reaction
K + H2O ➡ KOH + H2
According to the first law of thermodynamics, energy from the system to the surrounding can be transferred in the form of:
Heat and Work
Change in enthalpy of ΔH of a gaseous system can be calculated by following relationship:
ΔH = ΔE + PΔV
The amount of heat evolved when one mole of CH3COOH reacts with one mole of NaOH is:
< 57.4 kJ
Standard enthalpies of formation of O3, CO2, NH3 and HI are 142.2, -33.3, -46.2 and +25.9 kJ/mol respectively. The order o their increasing stabilities will be:
O3, HI, NH3, CO2
The enthalpy change for the reaction C(s) + O2(g) ➡ CO2 is called:
➡Enthalpy of formation
➡Enthalpy of combustions
➡Enthalpy of reaction
Which of the following processes has always ΔH = -ve
Combustion
Which one of the following reactions represents both standard enthalpy of combustion as well as standard enthalpy of formation
C (s) + O2 ➡ CO2(g)
The enthalpy of atomization of H2 is 218kJ/mole, the enthalpy of formation of H2 from gaseous atoms:
-218 kJ/mole
Which reaction shows enthalpy of formation:
C + O2 ➡CO2
The enthalpy of formation of an ionic compound is -392 kJ/mol. Total energy changes involved in the formation of gaseous ions form normal physical state is 280 kJ/mol. The enthalpy of lattice is:
-672 kJ/mol
Which of the following change in enthalpy in Born-Haber cycle may be negative
H (E.A)
Hess Law follows:
➡First law of thermodynamics
➡Law of conservation of energy
The net heat change in a chemical reaction is the same whether it is brought about in two or more different ways in one or several steps. It is known as:
Hess’s Law
Standard heat of formation of Al2O3 cannot be determined directly because:
Protective layer of Al2O3 form
One joule is equivalent to:
1/4.184 Cal
The enthalpies of all elements in their standard states are;
Zero
____ is not a state function.
Heat
No work is done at constant:
V
For an endothermic reaction, enthalpy of reactants:
Is smaller than that of the products
Most of the reactions which give stable products are;
Exothermic
Decomposition of H2O is;
Endothermic reaction
What type of reaction constitutes a limiting case between spontaneous and non-spontaneous reactions:
Reversible Reaction
In an endothermic reaction:
Er < Ep
In an exothermic reaction the heat energy is ______ while in an endothermic reaction it is;
➡Released
➡Absorbed
Whenever a reaction is endothermic, then it means that:
Heat is transferred from the surroundings to the system
Enthalpy of neutralization of strong acids and strong bases have the same values because;
The net change involves the combination of H+ and OH- ions to form water
The measurement of enthalpy change at standard conditions means that we should manage the measurement at:
25°C at 1 atm
The enthalpy change for the reaction C2H2 + 5/2 O2 ➡2CO2 + H2O is known as enthalpy of:
Enthalpy of Combustion
BaCl2 + H2SO4 ➡ BaSO4 + HCl, an exothermic reaction, the heat change represented by the above equation is called;
Heat of Reaction
The enthalpy of atomization of H2 is 218 kJ/mol and the enthalpy of formation of H2 from gaseous atoms
-436 kJ/mol
An enthalpy change which is always exothermic:
ΔHn
(Enthalpy of Neutralization)
The enthalpy change for the reaction, C2H5OH + 3O2 ➡ 2CO2 + 3H2O is known as enthalpy of;
Combustion of C2H5Oh
Which of the following gases have the highest heat of combustion
Acetylene
Which one of the following pairs has a maximum enthalpy of neutralization;
HCl + NaOH
ΔH of a system can be calculated by which of the following relationship
q = m x s x ΔT
Bomb calorimeter is used to determine the;
ΔHc
What is the unit of molar heat capacity?
J/mol¹K¹
This is true about the lattice energy of an ionic compound
➡Cannpt be determined directly
➡Can be obtained by means of the Born Haber cycle
The enthalpy of formation of an ionic compound is -392 kJ/mol. Total energy changes (ΔHx) involved in the formation of gaseous ions from a normal physical state is 280 kJ/mol. The enthalpy of the lattice is;
-672 kJ/mol
Choose from the following the correct statement about the Born Haber cycle
The lattice energy of crystalline substances can be calculated easily
Standard heat of formation of Al2O3 cannot be determined directly because:
A protective layer of Al2O3
The heat of combustion of graphite at 25°C is -393.51 kJ/ mol and that of a diamond is -395.41 kJ/mol. What is the enthalpy for the conversion of graphite into diamond at the same temperature?
+1.9 kJ/mol
By applying Hess’s Law, we can calculate:
ΔH
Enthalpy of neutralization of strong acids and strong bases have the same values because:
The net change involves the combination of H+ and OH- ions to form water.
For an endothermic reaction, enthalpy of reactants
Is smaller than that of the products
Which of the following has a positive value of enthalpy
Atomization
The net heat change in a chemical reaction is the same whether it is brought about in two or more different ways in one or several steps. It is known as;
Hess’s Law
Hess’s Law is analogous to;
Law of Heat summation
NaOH + HCl ➡NaCl + H2O. Enthalpy change in the above reaction is called;
ΔH = ΔE
A calorie is equivalent to:
4.184 J
The values of ΔH for the process I + e ➡ I-1 are;
< O
The enthalpy of formation of a compound is;
Either Positive or Negative
What is correct about the heat of combustion:
It is always negative
What is not correct about ΔHf:
It is always negative
If an endothermic reaction is allowed to take place very rapidly in air, the temperature of the surrounding air will;
Decrease
One Joule is equivalent to:
1/4.184 cal
The heat of reaction depends upon:
➡Temperature of the Reaction
➡Physical states of the reactants and the products
The exothermic process is;
Respiration
During an exothermic or endothermic reaction, one of the following formulas is used to calculate the amount of heat evolved or absorbed:
q = m x s x ΔT
Most of the reactions which give stable products are;
Exothermic
The measurement of enthalpy change at standard conditions means that we should manage the measurement at:
25°C at 1 atm
The total heat content of a system is called:
Enthalpy
The enthalpies of all elements in their standard states are;
Zero
A state function which describes together the internal energy and product of pressure and volume is called
Enthalpy
The enthalpy change for the reaction C2H2 + 5/2 O2 ➡ 2CO2 + H2O is known as enthalpy of;
Combustion of C2H2
The value of ΔV is very small. The term PΔV can be neglected for processes involving:
➡Liquid
➡Solid
The lattice energy of NaCl is;
-787 kJ/mol
Decomposition of H2O is :
Endothermic Reaction
According to Hess’s Law, the enthalpy change for a reaction:
independent of the path
Enthalpy of formation of one mole of ionic compound form gaseous ion under standard condition is called;
Lattice Energy
Change in enthalpy (ΔH) of a system can be calculated as;
ΔH = ΔE + PΔV
If the internal energy of the system is increased:
➡Change in the state of the system may occur
➡Temperature of the system may rise
➡Chemical reaction may take place
Enthalpy of a reaction can be measured by:
Glass calorimeter
In order to determine ΔH of ionic compound which is the correct relationship:
ΔH (Lattice) = ΔHf - ΔHx
Enthalpy of neutralization per mole of H2SO4/ Ba(OH)2 is;
-57.4 kJ/mol
Whenever a reaction is endothermic, then it means that ;
Heat is transferred from the surroundings to the system
How much heat is absorbed by 100g of water when its temperature decreases from 25°C to 5°C
(Heat capacity is 4.2 k/gK)
-84,00 J
One of the best applications of Hess’s law to calculate the lattice energy of ionic compound is;
Born-Haber Cycle
ΔH of a system can be calculated by which of the following relationships:
q = m x s x ΔT
Which of the following processes has always ΔH= -ve
Dissolution of an ionic compound
ΔH = ΔE is true for which of the following reaction?
▶K + H2O ➡ KOH + H2❌
▶N2 + 3H2 ➡ 2NH3❌
▶AlCl3 + 3NaOH ➡ Al(OH)3 + 3NaCl✅
▶ 4Na + O2 ➡ 2Na2O❌
BaCl + H2SO4 ➡ BaSO4 + HCl ΔH =-22.4 kJ/mol, the heat change represented by the above equation is called;
The heat of the reaction of BaSO4
When water is added to quick lime, the reaction is:
Exothermic
What type of reaction constitutes a limiting case between spontaneous and non-spontaneous reactions;
Reversible Reaction
Thermodynamics does NOT deal with
Rate of Reaction
____ is not a state function.
Heat
The enthalpy of atomization of H2 is 218 kJ/mole and the enthalpy of formation of H2 from gaseous atoms:
-436 kJ/mol
The enthalpy change for the reaction C + O2 ➡ CO2 is called:
➡Enthalpy of formation
➡Enthalpy of reaction
➡Enthalpy of combustion
Which equation shows lattice energy for the ionic compound?
Na+ + Cl- ➡NaCl
A process which is spontaneous and endothermic;
H2O(l) ➡ H2O(g)
An enthalpy change which is always exothermic
ΔHn
All of the following are exothermic processes except:
Evaporation
Enthalpy of combustion of food, fuel and other compounds can be measured accurately by:
Bomb Calorimeter
The enthalpy of formation of an ionic compound is -392 kJ/mol. Total energy changes (ΔH) involved in the formation of gaseous ions from the normal physical state is 280 kJ/mol. The enthalpy of the lattice is;
-672 kJ/mol
Which of the following enthalpies of formation cannot be measured directly:
➡ΔH(lattice) of an ionic compound
➡ΔHf for CO
➡ΔHf for B2O3
All are slow processes except:
The reaction of AgNO3 with NaCl
Heat absorbed or evolved during the chemical reaction at constant pressure is;
ΔH
A bomb calorimeter is used to determine the:
ΔHc
Which enthalpy of reaction can not be determined by glass calorimeter
Enthalpy of combustion
Which is not related to state function:
➡It deals with atomic level✅
➡It is a macroscopic property❌
➡It depends upon initial and final values❌
➡It is independent on apth❌
In an endothermic reaction:
Er < Ep
Standard heat of formation of Al2O3 cannot be determined directly because:
Protective Layer of Al2O3
In an exothermic reaction, the heat energy is ___ while in an endothermic reaction it is___
➡Released
➡Absorbed
Which one is the endothermic and spontaneous process
Melting of Ice
One kilo calorie is equal to;
4184 J
By convention, the standard heat of formation of all elements is assumed to be:
Zero
The change in enthalpy of a system when one mole of the substance is completely burnt in excess of air or oxygen is called:
Heat of combustion
Which of the following enthalpy change always have a negative value:
ΔHc
The change in enthalpy when one mole of a substance is dissolved in a specified quantity of solvent at a given temperature is called:
Heat of Solvation
Neutralization of acid-base is;
➡Spontaneous
➡Non-Spontaneous
The born-Haber cycle is an application of;
Hess’s law
ΔH represent the enthalpy change at;
25°C and 1 atm pressure
The enthalpy change ΔH of a process is given by the relation:
ΔH = ΔE + PΔV
A system absorbs 100 kJ heat and performs 50kJ work on the surroundings. the increase in internal energy of the system is:
50K
Which equation represents the atomization of iodine ;
1/2 I2 (s) ➡I (g)
The heat of combustion of ethane is -337.0 kcal at 25°C. The heat of the reaction when 3g of ethane is burnt completely is;
-33.7 kcal
The heat of combustion of graphite at 25°C is 393.51 kJ/mol ad that of a diamond is 395.41 kJ/mol. What is the enthalpy for the conversion of graphite into diamond at the same temperature?
+1.9 kJ/mol
The standard enthalpy changes of the formation of carbon dioxide and water are -394kJ/mol and -286 kJ/mol respectively, if the standard enthalpy change of combustion of propyne, C3H4 is -1938 kJ/mol. What is its standard enthalpy change of formation?
-184 kJ/mol
Total heat energy (q) can be calculated in a bomb calorimeter by using the following formula:
c x ΔT
Enthalpy of neutralization of strong acids and strong bases have same values of because:
The net change involves the combination of H+ and OH- ions to form water
For endothermic reaction, enthalpy of reactions:
Is smaller than that of the products
Which of the following has positive value of enthalpy:
Atomization
The net heat change in a chemical reaction is the same whether it is brought about in two or more different ways in one or several steps. It is known as:
Hess’s Law
Hess’s law is analogus to:
Law of heat summation
NaOH + HCl ➡NaCl + H2O.
Enthalpy change in the above reaction is called
Enthalpy of neutralization
If a reaction involves only solids and liquids, which of the following is true?
ΔH = ΔE
Calorie is equivalent to:
4.184 J
The values of ΔH or the process I(g) + e- ➡I-1 is :
<0
The enthalpy of formation of a compound is:
Either positive or negative
What is correct about heat of combustion:
It is always negative
What is not correct about ΔH:
➡ It is always negative✅
➡ Its value is gives an idea about the realtive stability of reactants and products❌
➡ Value depends upon nature of bonds❌
➡ Its value can be greater or less than zero❌
If an endothermic reaction is allowed to take place very rapidly in air, the temperature of the surrounding air will:
Decrease
One Joule is equivalent to:
1/4.184 cal
The heat of reaction depends upon
➡Temperature of the reactants
➡Physical States of the reactants and the products
The exothermic process is:
Respiration
During an exothermic process or endothermic reaction one of the following formulas is used to calculate the amount of heat evolved or absorbed:
q = m x s x ΔT
Most of the reactions which give stable products are
Exothermic
The measurement of enthalpy change at standard conditions means that we should manage the measurement at;
25°C at 1 atm
Total heat content of a system is called:
Enthalpy
The enthalpies of all elements in their standard states are:
Zero
A state function which describees together the internal energy and product of pressure and volume is called;
Enthalpy
The enthalpy change for the reaction C2H2 + 5/2 O2 ➡2CO2 +H2O. is known as the enthalpy of:
COmbustion of C2H2
The value of ΔV being very small. The term PΔV can be neglected for process involving:
➡Liquid
➡Solid
The lattice energy of NaCl is:
-787 kJ/mole
Decomposition of H2O is :
Endothermic reaction
According to Hess’s law ,the enthalpy change for a reaction:
Independent of the path
Enthalpyof formaton of one mole of ionic compound form gaseous ion under standard condition is called:
Bond Energy
Choose from the followings the correct statements about Born Haber cycle:
The energy changes in a cyclic process is not zero
Change in enthalpy (ΔH) of a system can be calculated by:
ΔH = ΔE + PΔV
If internal energy of the system is increased:
➡Change in state of the system may occur
➡Temperature of the system may rise
➡Chemical reaction may take place
Enthalpy of a reaction can be measured by:
Glass Calorimeter
To determine ΔH of ionic compound which is the correct relationship
ΔH (lattice) = Hf - Hx
Enthalpy of neutralization per mole of H2SO4/ Ba(OH)2 is:
-57.4 kJ/mole
Whenever a reaction is endothermic , then it means that:
Heat is transferred from the surroundings to the system
How much heat is abosrbed by 100g of water when ts temperature decreases from 25°C to 5°C?
(Heat capacity of H2O=4.2 J/gK)
-84,00J
One of the best applications of Hess’s law to calculate the lattice energy of ionic compound is:
Born Haber Cycle
ΔH of a system can be calculated by which of the following relationship:
q = m x s x ΔT
Which of the following processes has always ΔH=-ve
Dissolution of ionic compound
ΔH=ΔE is true for which of the following reaction:
AlCl3 + 3NaOH ➡Al(OH)3 + 3NaCl
When water is added to quicklime, the reaction is;
Exothermic
ΔH = ΔE for which of the folowing reaction:
AlCl3 + 3NaOH ➡Al(OH)3 + 3NaCl
What type of reaction constitute a limiting case between spontaneous and non-spontaneous reaction:
Reversible Reaction
Thermodynamics does NOT deal with:
Rate of reaction
____ is not a state function:
Heat
The enthalpy of atomization of H2 is 218 kJ/mole, the enthalpy of formation of H2 from gaseous atoms
-436 kJ/mole
The enthalpy of change for the reaction C + O2 ➡CO2 is called:
➡Enthalpy of formation
➡Enthalpy of reaction
➡Enthalpy of combustion
Which equation shows lattice energy of ionic compound:
Na+(g) + Cl-(g) ➡NaCl
A process which is spontaneous and endothermic:
H2O (l) ➡H2O(g)
An enthalpy change which is always exothermic:
ΔH n
All of the following are exothermic process except:
➡Freezing of water❌
➡Evaporation✅
➡Condensation❌
➡Combustion❌
Enthalpy of combustion of food, fuel and other compounds can be measured accurately by:
Bomb calorimeter
The enthalpy of formation of ionic compound is -392 kJ/mol. Total energy changes (ΔHx) involved in the formaton of gaseous ions from normal physical state is 280 kJ/mol. The enthalpy of lattice (ΔHlattice) is:
-672 kJ/mole
Which of the following enthalpies of formation cannot be calculated directly:
➡ΔH(lattice) for ionic compounds
➡ΔHf for CO
➡ΔHf for B2O3
All are slow procecsses except:
Reacton of AgNO3 with NaCl
Heat absorbed or evolved during the chemical reaction at constant pressure is:
ΔH
A bomb calorimeter is used to determine the:
ΔHc
Which enthalpy of reaction cannot be determined by glass calorimeter:
Enthalpy of combustion
Which is not related to state function:
It deals with atomic level
In an endothermic reaction :
Er < Ep
Standard heat of formation of Al2O3 cannot be determined directly because:
Protective layer of Al2O3
In an exothermic reaction, the heat energy is __- while in endothermic reaction it is;
Released, Abosrboed
Which one is endothmeric and spontaneous process:
Melting of ice
One kilo calorie is equal to
4184 J
By convention, the standard heat of formation of all elements is assumed to be:
Zero
The change in enthalpy of a system when one mole of the substance is compeltely burnt in excess of air or oxygen is called:
Heat of combustion
Which of the following enthalpy change always have a negative value:
ΔHc
The change in enthalpy when one mole of a substance is dissovled in a specified quantity of solvent at a given a temperature is called:
Heat of solvation
Neutralization of acid-base is;
➡Spontaneous
➡Exothermic
Born Haber cycel is an applicaton of;
Hess’s Law
ΔH represent the enthalpy change at;
25°C and 1 atm pressure
The enthalpy change of ΔH of a process is given by the realtion:
ΔH = ΔE + PΔV
A system absrobs 100 kJ heat and perorms 50KJ work on the surroundngs. The increase in internal energy of the system is:
50kJ
Which equaton represents the atomization of iodine:
1/2 I2 (s) ➡I(s)
The heat of combustion of ethane (C2H6) is -337.0 kcal at 25°C. The heat of the reaction when 3g of ethane is burnt completely is:
-33.7 kcal
Heat of combustion of graphite at 25°C is -393.51 Kj/mol and that of diamond is -395.41 kJ/mol. What is the enthalpy for the conversion of graphite into diamond at same temperature.
+1.9 kJ/mol
The standard enthalpy changes of formation of carbon dioxide and water are -394 kJ/mol and -286 kJ/mole respectively, if the standard enthalpy change of combustion of propyne, C3H4 is -138 kJ/mole. What is its standard enthalpy change of formaton?
-184 kJ/mole
Total energy (q) can be calcualted in a bomb calorimeter by using following ormula:
c x ΔT
One calorie is equal to:
4.184 J
Which of the following change in enthalpy in Born-Haber cycle may be negative:
ΔH (E.A)
Which of the following is incorrect about enthalpy of neutralization?
➡Its maximum value is 57.5 kJ/mol❌
➡It is equal to enthalpy of formation of water from ions❌
➡It is less than 57.5 kJ/mol when one o the acid or base is weaker❌
➡Energy is abosrbed in this process✅
Standard enthalpy of Al2O3 cannot be measured because:
Protective layer of oxide covers the surface
The dissolution of ammonium chloride in water is a/an:
➡Endothermic process
➡Spontaneous process
For an endothermic reaction the value of ΔH is denoted by:
Positive sign
Which is used to measure enthalpy of combustion:
Bomb calorimeter
For a given process, the heat change at constant pressure (qp) and constant volume (qv) are related to each other as:
qp > qv
The amount o heat required to convert one mole of a solid directly into its vapour state at STP is called as
Standard heat of sublimation
Enthalpy of neutralization of all the strong acids and strong bases has the same value because:
The net chemical change involves the combination o H+ and OH- ions to form water
In endothermic reactions, the heat contents of the:
Product is more than that of reactant
Work may be defined in terms of pressure-volumes s:
1 atm 298K
Which of the following molecule show only translational motion?
He
(Mono-atomic)
The study of heat changes accompanied by a chemical reaction is called as:
Thermochemistry
The system becomes more stable if it:
Loses energy
According to the first law of thermodynamics energy from the system to the surroundings can be transferred in the form of:
Heat and Work
The sum of all the energies of atoms, molecules, or ions within a system s called:
Internal Energy
Evaporation of water is ___ change.
Endothermic
The expresson ΔE=q + w is:
First law of thermodynamics
An enthalpy change which is always endothermic
ΔH (atomization)
The enthalpy change in a cyclic process is:
Zero
The net heat change in a chmical reaction is same whether it is brought in two or more diferent ways n one or several steps. it is known as:
Hess’s law
Which of the following is correct relation at constant pressure
ΔH = qp
Which of the following is the correct representation for the calculation of lattice energy
ΔHf = ΔHx + ΔHl
The enthalpy of neutralization for given reaction
H2SO4 + Ba(OH)2 ➡BaSO4 + 2H2O
-57.4 kJ/mol
The change in enthalpy of a system when one mole of the substance is completely burnt in excess of air or oxygen is called:
Enthalpy of combustion
ΔH represent the enthalpy change at:
➡25°
➡1 atm pressure
A system absorbs 100 kJ heat and performs 50 kJ work. The increase in internal energy of the system is:
50 kJ
Which of the followig enthalpy is always proceeding through evolution of heat?
Enthalpy of combustion
In order to determine ΔH (lattice) of ionic compound which is correct relatonship:
ΔH (lattice) = ΔHf - ΔHx
With decrease in charge to size ratio of ions, the lattice energy:
Decrease
Hess’s law is analogus to:
Law of constant heat summation
The heat of combustion o ethane (C2H6) is -337.0 kJ at 25°C. The heat of the reaction when 3g of ethane is burnt completely is:
-33.7 kJ
Born Haver cycle is an application of:
Hess’s Law
Which of the following enthalpy of formation cannot be measured directly?
➡ΔH (lattice) for ionic compound
➡ΔHf of CO
➡ΔHf of B2O3
Enthalpy of combustion of food, fuel and other compounds can be measrued accurately by:
Bomb calorimeter
Which equation shows lattice energy for ionic compound
Na+(g) + Cl-(g) ➡NaCl (s)
A process which is spontaneous and endothermic
H2O (l) ➡ H2O (g)
The enthalpy change for the reaction C(s) + O2 (g) ➡CO2 (g) is called:
➡Enthalpy of formaton of CO2
➡Enthalpy of combustion of C
➡Enthalpy of reaction
For a given gaseous process, the heat changes at constant pressure (qp) and at constant volume (qv) are related to each other as
qp > qv
The enthalpy of formation of an ionic compound is -390 kJ/mol. Total energy changes (ΔHx) involved in the fomration of gaseous ions from normal physical state is 280 kj/mol. The enthalpy of lattice (ΔH lattic.) s;
-670 kJ/mol
Which one indicates enthalpy of atomization
Na (s) ➡Na (g)
(Physical state to gaseous 1 mole)
The standard enthalpy of ormatio of all the elements in their standard physical state is:
Zero
Does no depend on initial and final state;
Heat
Enthalpy of formation of hydroge molecule is -436 kJ/mol. What will be enthalpy of atomization o fhydrogen.
+218 kJ/mol
(As atomization is for 1 mole)
he enthalpy change for the reaction, C2H2 + 5/2 O2 ➡2CO2 + H2O is known asenthalpy of:
Combustion o C2H2
Which of the following pairs has maximum enthalpy o neutralization?
HCl + NaOH
Amount of energy abosrbed when 1 mole of solid Na Cl is dissociated into its gaseous ions:
+787 kJ/mole
Calorie is equivalent to;
4.184 J
For the reaction NaCl (s) ➡Na+ (aq) + Cl- (aq) the change in enthalpy is called:
heat o solution
Evaporation of water is an exceptional case of:
Spontaneous
Which statement is contrary to the first all of thermodynamics?
Continuous production of mechanical work without supplying an equivalent amount of heat is possible
Born haber’s cycle enables us to calculate:
Lattice Energy
Which statement is not correct about ΔH?
➡ΔH of the reaction depends on temperature❌
➡ΔH of reaction can > or < zero❌
➡ΔH of catalyzed and uncatalyzed reaction is same❌
➡ΔH is always < 0✅
Which of the following processes is always endothermic?
Atomization
Which one of the following statements is correct or the neutralizaton of a strong acid by a strong alkali in aqueous solution at 25°C?
The enthalpy change per mole of H2O formed is independent of the acid or alkali used as they are strong
According to Born Haber cycle, ΔH (lattice) of ionic compound is determined by the formula:
ΔH (lattice) = ΔHf - ΔHx
Lattice energy helps to explain all of the following properties of ionic compounds EXCEPT:
Dipole Moment
In azeotropic mixture showing positive deviation from Raoult’s law, the volume of the mixture is:
Slightly more than the total volume of the components
All of the following reactions are exothermic EXCEPT:
N2(g) + O2(g) ➡2NO (g)
For which one of the following compounds standard enthalpy change (ΔH) can be measured directly by calorimeter?
MgO
All of the following are state functions EXCEPT?
q
All of the following standard enthalpy change (ΔH) have only positive value EXCEPT:
➡ΔHv❌
➡ΔHBDE❌
➡ΔHsol✅
➡ΔHi❌
12.0 g of graphite is burnt in a bomb calorimeter and the temperature is recorded in 5K. Calculate the enthalpy of combustion (ΔH) of graphite if the heat capacity of the calorimeter is 0.0 kJ/mol
-450 kJ/mol
A glass calorimeter is used to determine:
ΔH neutralization
If an endothermic reaction is allowed to take place very rapidly in the air, the temperature of the surrounding air:
Decreases
The nature of an aqueous solution of ammonia (NH3) is:
Basic
Internal energy of a system depends on all the factors EXCEPT
Path
Which of the following is a correct representation of the electron affinity of chlorine:
Cl (g) + 1e ➡Cl -1 (g) ΔH = -349 kJ/mole
Which value of heat of fomration indicates that the product is the least stable?
+ 64.8 kCal
Absorption of heat occurs when:
NH4Cl dissolved in water
Identify the state function among the following:
q + W
For the neutralization of 1 mole o H2SO4 with 2 moles of NaOH in dilute solution, the heat liberated is:
> 57 kJ
The enthalpy change of a reaction does not depend o:
Different intermediate reactions
Which enthalpy change (ΔH) is relevant in the following equation
H2 ➡ H + H ΔH=+436 kJ/mol
Bond Dissociation Energy
Heat of formation of MgO is given below:
Mg + 1/2 O2 ➡MgO ΔH = -692 kJ/mol
This equaton shows that :
The product is ver stable
In exothermic reaction heat transer from:
System to surrounding
Enthalpy change during the formation of one mole fo atoms from its elements is called enthalpy of atomization. The element in this change is n:
➡Solid State
➡Liquid State
➡Gaseosu State
Which of the following formula cannot be used in Hess’s law?
H (lattice) = Hf + Hx
Standard enthalpy of combustion of carbon (ΔHc ) is
-393.7 kJ/mol
Correct decreasing order of energy is
1 Cal > 1 Joule > 1 erg
Lesser the energy of a system
Greater is its stability
For the melting of ice H is
Positive
When an exothermic reaction is reversed it
Becomes an endothermic reaction
All types of energies of aprticels forming a system is called:
internal Energy
Spontenous reacton aer:
Uni-Directional
Spontaneous processes:
Move from non-equilibirum to equilibirum state
Spontaneous processes:
Move from non-equilibirum to equilibirum state
In order to predict whether reaction s spontaneous or non-spontaneous we should study:
Free energy chagne of the system
Which one of the following is incorrect to the first law of thermodynamics?
Energy of the universe tends to be either maxmum or minimum
We can keep the volume of a system constant, consisting o agas enclosng ia cylinder fitted with piston, by:
Fixing the postion of piston
Born Haber’s Cylce is applicable to;
ionic compounds
The highest energy releasing step in Born Haber’s cycle is;
Lattice Energy
The value of ΔV being very small, the term Δ(PV) can be neglected, for processes involving:
Solids and Liquids
The total heat contents of the system is called;
Enthalpy
The enthalpy of ionic compounds i calculated best with;
Born Haber Cycle
The enthapy change when one mole of compound is formed its elements at standard state is called:
Enthalpy of formation
Heat evolved or absorbed during reaction can be measured by using which formula:
q = mcΔT
Bomb calorimeter is used to determine the accurate enthalpy of:
Combustion
Energetically a chemica reation is independent of its path according to ___ law of thermochemistry
Second
For the reaction NH4Cl + aq ➡NH4Cl the enthalpy change is called:
Heat of solution
Enthalpy o neutralization is represented as:
ΔHn
Hes’s law of constant summation is for each step mechanims:
Dependent
Which statement about internal energy is incorrect?
➡It is equal to sum of K.E. and P.E.❌
➡At constant volume ΔE=qv❌
➡It is expressed in Newton or Dynes✅
➡With the increase in internal energy the temperature of the system also increases❌
or the reaction CH3COOH ➡CH3COO- + H+ the change in enthalpy is called:
ENthalpy of ionization
It is common observation that asa result of chemical reaction, the energy is either evolved or absorbed in the fomr of:
Heat
During a chemical process which one is valid:
Total energy of the products is never equal to that of reactants
During an endothermic reacton:
Temperature of the surrounding will decrease and energy of the system will increase
The energy units in which heat chagnes are expressed in SI system are:
Joule
Thermochemsitry gives us information about:
➡Energy of heat contents of the compund
➡Energy involved n chemical bonding
➡Energy chagnes occurring n chemical equilibirum
Which is the Non-Spontaneous process?
Reaction of N2 and O2
To predict the spontaneity of reaction. It is necessary to study:
Free energy of the system
Ionic charge has ___ relationship with alttice energy.
Exponentially Direct
The potential energy of a system include:
➡All the types of bonds
➡Van der Waals forces present the particles
Which is the symbol of standard heat of formation?
ΔH
Which one of the following equations correctly defines the enthalpy change of formation of carbon monoxide?
C(s) + 1/2 O2 (g) ➡CO (g)
The value of the enthalpy change or the process represented by the equation Na (s) ➡Na+ (g) + e- is equal to;
The sum of the enthalpy change of atoizaton and the first ionization energy of sodium
Which one of the followng processes is endothermic?
The electrolysis of water
Which value would be requred to estimate the lattice nergy for the hypothetical ionic compound MgH2?
the standard enthalpy chage of formation of MgH2
Which equation represents the change corresponding to the enthalpy change of atomization of iodine?
1/2 I2 (s) ➡I (g)
From which of the following reactions can the bond energy of the C-F bonds be determined by usng only the standard enthalpy change of the reaction
C4 (g) ➡C(g) + 4F(g)
Which statement about the standard enthalpy change of ormation of carbon dioxide is correct?
It is equal to the standard enthalpy change of combustion of carbon
the following questons each represent a step in the Born-haber cycle for the enthalpy change of formation of sodium choride. Which changes have a negatvie ΔH value?
Cl (g) + e- ➡Cl- (g)
