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GC/OC > GC - Ch 4 > Flashcards

GC - Ch 4 Flashcards

1
Q

2H2(g) + O2(g) -> 2H2O(g). This is an example of a combination reaction. describe what a combination reaction is.

A

This is an example of 2 or more molecules reacting to create a single molecule which are combination reactions.

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2
Q

What are the expected results of a decomposition reaction?

A

Decomposition reactions are chemical reactions in which a single molecule breaks down to create 2/more products. Decomposition reactions tend to be seen with the use of high frequency radiation OR electrophoresis

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3
Q

Contrast combustion reactions from decomposition reactions.

A

Decomposition reactions are reactions in which a molecule breaks down to create multiple products.
Combustion reactions are those in which oxygen is used to make oxides. These types of reactions are usually seen with the use of a hydrogen carbon fuel along with oxygen. Products typically formed always include H2O and CO2

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4
Q 
The chemical reaction that typically requires O2
A. Incorporation reaction 
B. Combination reaction 
C. Decomposition Reaction 
D. Combination Reaction
A

D. O2 + HC fuels can also be sulfur or sugar based (because these have HC in them!)

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5
Q

Assess this chemical reaction: Cu(s) + Ah(NO3)2(aq) -> Aq(s) + CuNO3. defend what generic type of reaction this is in terms of atomic reaction

A

A single displacement reaction. You can see that Cu has replaced Ag in its bond to NO3.
Note: these reactions do tend to be further classified as redox reactions as these tend to demonstrate electron movement.

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6
Q

What is a metathesis reaction? describe the physical states of the products in this type of reaction?

A

This is a double replacement reaction where 2 compounds swap places and bind to the other’s previous molecules
Products tend to be removed from solution as a precipitate or gas. these products can also remain as electrolytes (aqueous) in solution as well

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7
Q

Contrast neutralization reactions from metathesis reactions.

A

Neutralization reactions are a special type of metathesis reactions. These types of reactions are those that specifically involve an acid or base! Where in the reaction, both cancel one another out in acidity/basicity and create a more neutral solution. Products of these types of reactions tend to be a salt and water.

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8
Q

Unlike the typical products from double replacement, how are products of neutralization different

A

Double replacement products - precipitate or leave the system as a gas.
Neutralization produces salt and water. This change is not often visible and requires an indicator!!

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9
Q

Describe in words what occurs when Zn(NO3)2 is dissolved in (NH4)2S

A

The likely product of this reaction is a double replacement where Zn-S and NH4NO3

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10
Q

In the reaction of Zn + AgCl, what are the products, conditions, and reaction type

A

Appears to be a single replacement. More specifically a prod: ZnCl + Ag (aq)

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11
Q

Contrast the different ways how compounds can be represented in general chemistry, organic, and inorganic chemistry

A

General chemistry - VESPR and Lewis Dot structure
Organic chemistry - Structural formulas - these are skeletal representation
Inorganic chemistry - Constituent atoms with NO bonds Ex: C6H12O6

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12
Q 
Pure samples of a given compound will contain the same elements in a given identical mass ratio
A. Percent composition 
B. Law of constant composition
C. Law of conservation 
D. Law of conservation of mass
A

B. This law is defined by the question stem. Ex: Every sample of water has 2 atoms of every O atom. Therefore for every H gram of H, there are 8 grams of O. This is because H molar mass is 1g/mol. There are 2 atoms therefore there is 2 g/mol of H for every mole of O (16g/mol) therefore the ratio of H:O => 2:16

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13
Q

T/F - based on the law of constant composition, pure samples of a given compound will contain the same elements in an identical density ratio anywhere else in the universe

A

False. Law of constant composition defines the mass ratio is conserved, not that density ratios are conserved. Density is affected by gravity and therefore changes with different locations

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14
Q

Compare and contrast empirical and molecular formulas of compounds

A

Sometimes both can be one and the same for a molecule. But both are ways to represent the formula of compound. Ex: H2O
Empirical formula - this is the simplest whole-number ratio of the elements in the compound Ex: Benzene CH
Molecular formula - this is the formula which represents all of the atoms in the compound. this should be the multiple of the molecule’s empirical formula. Benzene: C6H6

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15
Q

The empirical formula is indicative of CH2O

A

A monosaccharide!

there are many monosaccharides and many of them have this empirical formula as well! Fructose, glucose, and galactose

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16
Q

What is the percent composition?

A

This quantity looks at what percent of our compound is made up of a certain element
therefore this is a mass evaluation
% = (mass in element in formula/molar mass) 100%

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17
Q

T/F - Percent composition can only be found based off the molecular formula and not empirical

A

false! Both can be used to find the percent composition as both demonstrate ratios of different elements (this is percent composition)

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18
Q

What is the empirical and molecular formula of a compound that contains 40.9% C, 4.58% H, and 54.52% O and has a molar mass of 264 g/mol

A

Just as you are able to find % composition from an empirical or molecular formula, you can use these %s to find the molecular and empirical formula too!!
S1: Find the moles each element has out of _ grams. this _ tends to be 100 as this is the easiest to work with. This step uses their % and molar mass on PT to dtm moles
C moles: 40.9g/12g/mol = 3.4 mole
H moles = 0.05g/1g/mol = 4.6 mole
O moles = 54.52g/16g/mol = 3.4 mole

S2: Using the smallest moles to divide all the other moles, this creates whole number ratios that we can all work with
C = 3.4/3.4 = 1
H = 4.6/3/4 = 1.33
O = 3.4/3.4 = 1

S3: Create an empirical formula:
C1H1.33O1 (3) => C3H4O3

S4: Find the molecular formula: Molar mass/empirical formula mass => (264g/mol)/88g = 3. Use this value to multiply this to your empirical formula to get your molecular formula. C3H4O3(3) => C9H12O9

OR

S1: multiple molar mass to the % then the divid the value by molar mass - this gives you the moles of each in the molecular formula and then simplify this molecular formula until you reach the empirical formula.
C moles = [(0.409)(2644g)] / 12g/mol = 9mol
H moles = (0.0458)(264g)/ 19mol = 12mol
etc..

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19
Q

Find the percent composition (by mass) of Na, Cr, and O in Sodium Carbonate (Na2CO3)

A

Na = 14g(2) = 28g
C = 12g
O = 16g(3) = 48g
Total 88g

Na% = 28/88 = 0.318 
C% = 12/88 = 0.136
O% = 48/88 = 0.545
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20
Q

Experimental data from the combustion of an unknown compound indicates that it is 28.5% iron, 24.0% sulfur, and 49.7% oxygen by mass. What is its empirical formula?

A

Assume that there are 100g of sample, and each %composition represents a percentage of the 100g. Fe = 28.5g, S = 24g, and O = 49.7g

Next divide each number of grams by the atomic weight to determine the number of moles
Fe = 28.5g / (55.8g/mol) = 0.5/0.5 = 1
S = 24g/(32g/mol) = 0.7/0.5 = 1.5
O = 48.6g/(16g/mol) = 3/0.5 = 6
=> Fe1S1.5O6 (2) = Fe2S3O12
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21
Q

What is the definition of compounds?

A

This is defined as pure substance composed of 2/more elements in a fixed proportion.
Compounds can be broke down by chemical means to produce their constituent elements or other compounds

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22
Q

Contrast atomic weight from molecular weight

A

Atomic weight - this is a misnomer because it is actually a weighted average of the masses of the naturally occurring isotopes of an element.
Molecular weight - is simply the sum of the atomic weights of all the atoms in a molecule, and its units are atomic mass units (amu) per molecule

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23
Q

Why is it hard to define ionic compounds as true molecules? Use NaCl in your explanation

A

These are hard to define because of the oppositely charged ions arrange themselves in solid states.
For instance, NaCl are coordinated in lattices where Cl- ions surround the Na+ ions. This makes it rather difficult to clearly define NaCl - this is why we use formula units

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24
Q

What are formula units? Why are they used?

A

These represent the empirical formula of the compound. The use of this quantity is because ionic compounds are hard to define as a molecules (combination of 2/more atoms held together by COVALENT bonds)

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25
Q

What is the purpose of formula weight?

A

This is the sum of atomic weights of all atoms appearing in a given chemical formula. This formula weight is important for substances that do not consist of indv molecules (Ex: Ionic compound NaCl)
To calculate:
1. multiply the atomic weight of each element in a formula by the number of atoms of that element present in the formula
3. and then add all these products together

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26
Q

How many moles are in 9.53g MgCl2?

A

Molar mass: Mg = 24g/mol, Cl = 35x2 = 70g/mol. Total molar mass = 94g/mol
9.53g MgCl2 (mole/94g) = 0.101 mole

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27
Q

What is the molecular weight of SOCl2?

A 
Molecular weight = sum of molar mass 
S = 32g/mol
O = 16g/mol
Cl = 35 x 2 = 70g/mol 
= 118g/mol
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28
Q

What is the gram equivalent (GEW) of sulfuric acid?

A 
S1: Molar mass of H2SO4 
S = 32g/mol
H = 1x2 = 2g/mol
O = 16x4 = 64g/mol 
Molar mass = 98g/mol

S2: Id the equivalents (n) - this is the particles of interest produced or consumed per molecule. In this case, equivalents are H+ and this value = 2

S3: Calculate the gram equivalent weight = molar mass/n
98/2 = 49g/mol of H+

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29
Q

What is the normality of 2M Mg(OH)2 in solution?

A

Again normality, like gram equivalent weight is the focus of the equivalent of the compound. In this case there are 2 equivalents (OH) per molecule

Normality = molarity x n = 2M (2) = 4N Mg(OH)2

30
Q

Calculate the molar masses of NaBr

A

Na = 23g/mol
Br = 80g/mol
103g/mol

31
Q

Calculate the number of moles in 100g of SrCl2

A

Molar mass:
Sr = 88g/mol
Cl = 35x2 = 70g/mol
158g/mol

100g(mol/158g) = 0.633 mol

32
Q

How do the number of molecules in 18g of H2O compare to the number of formula units in 58.5g of NaCl?

A

18g of H2O = the total molar mass of H2O
and 58.5g of NaCl = the molar mass of NaCl

Both values equal one mole of the given substance. The number of entities in a mole is always the same (Avogadro’s number, 6 x10^23/mol)

33
Q

In the reaction of H2 + O2 -> _. What are the conditions, products and reaction type?

A

This is a combustion (due to the use of O2)
this requires heat and some sort of CH or S based fuels
Products: 2H2O

34
Q

In the reaction of AL(OH)3 + H3PO4, what are the conditions, products, and reaction types

A

Appears to be a double replacement, and more specifically a neutralization because of OH and H
Products: 3H2O and salt (AlPO4)

35
Q

In the reaction of 2H2O with electricity, what are the products and the reaction types

A

The use of electricity tends to be seen with electrophoresis. Remember that electrophoresis tends top be used in the decomposition reactions
Products: H2 and O2

36
Q

In the reaction of NaNO3 + CuOH, what are the products and reaction type

A

Products: NaOH and a salt (CuNO3)

this tends to dissociate fast because this is a strong base

37
Q

Compare and contrast the differences of rate constants and equilibrium constants

A 
Rate constants (k) this is constant is used to determine how fast a reaction will proceed. This constant is based on the concentrations of the reactants only. This constant is dependent on temperature and Ea this can be explained by its use in the rate law = k[A]^x[B]^y (note: the effect of concentration is already taken into account by the other [ ]. Reaction rate can be determined theoretically at the beginning.
Equilibrium constant (keq) is a constant used to determine where the equilibrium lies. This constant is based on the concentrations of aqueous reactants and products. This constant is use in measurement of equilibrium which tends to be measured at the end of a reaction
38
Q

What is the relationship of the equilibrium constant to the rate constant.

A

Rate constants (k) this is constant is used to determine how fast a reaction will proceed. Equilibrium constant (keq) is a constant used to determine where the equilibrium lies.You can demonstrate the relationship of one another through keq - this is the ratio of the rate constant of the forward rcn (k) divided by the rate constant of reverse. Therefore keq = k/k-1

39
Q

The units of the rate constants change based on the reaction order. Say that this is your rate law, what are the units of your rate constant
Rate law = k[CO2][H2O]

A

Rate law has to equal M/s overall for each rate law.
Our reaction is to the order of 2, this means that the units now are M^2
Therefore our unit of the rate constant: 1/(Ms)

40
Q

The units of the rate constants change based on the reaction order. Say that this is your rate law, what are the units of your rate constant
Rate law = k[CO2]

A

Rate law has to equal M/s overall for each rate law.
Our reaction is to the order of 2, this means that the units now are M
Therefore our unit of the rate constant: 1/s

41
Q

The units of the rate constants change based on the reaction order. Say that this is your rate law, what are the units of your rate constant
Rate law = k[A]^0

A

Rate law has to equal M/s overall for each rate law.
Our reaction is to the order of 2, this means that the units now are nothing!
To make up the difference, the units of our rate law has to be M/s

42
Q 
All are terms of rate constant except: 
A. Reaction rate coefficient
B. k
C. Reaction order 
D. Equilibrium constant
A

D. This term is used to define the constant used to find the equilibrium constant of a reaction and is based on differents molarities.
Note: Often times you’ll hear particular rate constants be termed order rather than rate constant. Reaction order is defined as the power of dependence of rate on the concentration of all reactants

43
Q

The concentration of all reactants in a zero-order reaction are increased two fold. What is the new rate of the reaction?
A. It is unchanged
B. It is decreased by a factor of 2.
C. It is increased by a factor of 2.
D. It cannot be determined from the information given.

A

A. The change of concentration of reactants will not affect a chemical reaction of 0th order.

44
Q 
If the rate law for a reaction is: 
rate = k[A]0[B]2[C]1
What is the overall order of the reaction?
A. 0
B. 2
C. 3
D. 4
A

The overall order of the reaction is the sum of the exponents. Therefore 2 + 1 = 3, C.

45
Q

Apply first order reactions to nuclear decay. What assumptions from the first order reactions are held in radioactive decay

A 
This is assumed that the reaction proceeds where there is no interaction of the decaying atom with any other molecule (also assumed in first order reaction) 
Nuclear decay = [A]t = [A]oe-kt 
[A]0 = [ ] @ initial 
[A]t = [ ] of A @ time t
k = rate constant (M/s) 
t = time
46
Q

On a rate vs concentration graph, depict how first order reactions are different from 0th order reactions.

A

0th order reactions are not affected by concentration changes, and therefore its curve will be a horizontal line at a constant rate (y axis)
1st order reaction are affected by changes in concentration proportionally. This means that increase in concentration will increase the rate at a steady rate. Therefore the curve will be linear line.

47
Q

A reactant in a second-order at a certain temperature is increased by a factor of 4. By how much is the rate of the reaction altered?
A. It is unchanged
B. It is increased by a factor of 4
C. It is increased by a factor of 16
D. It cannot be determined from the information given
`

A

General second order rcn: rate = k[A]2 or rate k[A][B]
Read the question carefully! A reactant is increased by a factor of 4. Change of 4 for each equation will yield a different result. Because we do not know which rate law this chemical reaction is, the change resulting reaction rate will not be determined

48
Q

A reactant in a second-order at a certain temperature is increased by a factor of 4. By how much is the rate of the reaction altered?
A. It is unchanged
B. It is increased by a factor of 4
C. It is increased by a factor of 16
D. It cannot be determined from the information given

A

General second order rcn: rate = k[A]2 or rate k[A][B]
Read the question carefully! A reactant is increased by a factor of 4. Change of 4 for each equation will yield a different result. Because we do not know which rate law this chemical reaction is, the change resulting reaction rate will not be determined

49
Q

Describe the curve of a second order reaction on a rate vs concentration graph

A

Second order reactions will demonstrate an exponential curve! This is because the second order equation is Rate law = k[A]2

50
Q

What are the assumptions in molecular interactions in regards to second order reactions

A

This means for rate = k[A]2, 2 A molecules MUST collide for reaction to occur
Or with rate = k[A][B], A and B molecules MUST collide

51
Q 
In a third-order reaction involving 2 reactants and 2 products, doubling the concentration of the first reactant causes the rate to increase by a factor of 2. What will happen to the rate of this reaction if the concentration of the second reactant is cut in half? 
A. It will increase by a factor of 2
B. It will increase by a factor of 4
C. It will decrease by a factor of 2
D. It will decrease by a factor of 4
A

General Rate Law for 3rd order Reaction with 2 reactants: Rate = k[A]2[B]
↑2x Reactant 1 => Rate Rcn 2x ↑ MUST be B, because this will increase Rate proportionally
Therefore when ↓1/2 Reactant => [½]2 => ¼ rate of reaction.
Based on this, we say this is a decrease by a factor of 4 AKA D.

52
Q

Which of the following experimental methods should NEVER affect the rate of a reaction?
A. Placing an exothermic reaction in an ice bath.
B. Increasing the pressure of a reactant in a closed container
C. Putting the reactants into an aqueous solution.
D. Removing the product of an irreversible reaction

A

D. Removing the product of an irreversible reaction will not change the rate of reaction. Irreversible reactions will continue until the reactants are completely converted and removing the products will not change the reaction rate. Note: If this was a zero order reaction, partial pressure of gas will affect the rate.
All other factors affect reaction rates. Partial pressure usually affects the reactions. Medium/solvents will affect how solvents interact and therefore has a role on reaction rates. Exothermic AKA heat will affect the rate of a reaction as this changes the temperature and therefore the kinetic energy.

53
Q

What does it mean for a step in a mechanism to be the rate-determining step?

A

This is the slowest step in the mechanism . This step determines the kinetics of the whole reaction because the reaction can only proceed as fast as the rate @ which this step occurs.

54
Q 
The following system obeys second-order kinetics
2NO2 -> NO3 +NO 	(slow) 
NO3 +CO -> NO2 + CO2 (fast)
What is the rate law for this reaction?
A. rate = k[NO2][CO]
B. rate = k[NO2]2[CO]
C. rate = k[NO2][NO3]
D. rate = k[NO2]2
A

The rate law for a whole mechanism IS the slowest step of the reaction as this is step is the step that sets the rate. Therefore the answer is D as contains ONLY the rate determining step AND is a second order reaction

55
Q

Describe what collision theory is

A

Collision theory of chemical kinetics - this is the theory that states the rate of a reaction is proportional to the number of collisions/second between reacting molecules. One caveat to note is that not all collisions are effective in creating a reaction. A proper orientation must exist in order to break old bonds and in order to form new bonds

56
Q

Mathematically describe the collision theory of chemical kinetics

A

The rate of reaction = (the total number of collisions/second)(the fraction of effective collisions)

57
Q

What is activation energy?

A

Ea is the ∆G of the peak of transition state to ∆G of reactant. This ∆G must be overcome in order for reaction to proceed its rcn coordinate

58
Q

How does the transition state theory compare with the collision theory of chemical kinetics?

A

Transition state theory states that the collision of 2 molecules causes both 2 enter into an intermediate molecule. This molecule can either enter into products or revert into reactants. It posits that this can only occur once the collusion occurs with enough energy (which is further elaborated by the collision theory)
Collision theory, unlike transition theory, focuses on energy and orientation of reactants and considers each potential reaction to be all or nothing.

59
Q

On a reaction coordinate diagram, how would the kinetic pathway appear as compared to the thermodynamic pathway?

A

Kinetic pathway - require less ∆G to transition states, but formed products are higher in energy compared to thermodynamic pathway.
Therefore is also a smaller different in ∆G between transition state and products

60
Q

What conditions favor the formation of a kinetic product? A thermodynamic product?

A

A kinetic product - this requires low heat transfer (decrease T) and decrease G to reach transition state.
Thermodynamic product: Increase temp/Increase G to reach transition state. This product requires high heat transfer

61
Q

Which of the following best describes a catalyst?
A. Catalysts are used up in the reaction, increasing reaction efficiency.
B. Catalysts increase the rate of the reaction by lowering the activation energy
C. Catalysts alter the thermodynamics of the reaction to facilitate the formation of products or reactants.
D. Catalysts stabilize the transition state by bringing the it to a higher energy.

A

B. Enzymes increase the rate of reaction by lowering the activation energy. In this process, it does stabilize the transition state, but it does raise the energy therefore this cannot be D.
Enzymes - do not change the thermodynamics of reactions and are not consumed in reactions

62
Q 
In a certain equilibrium process, the activation energy of the forward reaction ∆G‡f is greater than the activation energy of the reverse reaction ∆G‡r. This reaction is:
A. Endothermic 
B. Exothermic 
C. Spontaneous 
D. Nonspontaneous
A

If you draw out a free energy diagram, 2 key features should pop out from this: (1) Ea forward should be large in energy (2) Ea reverse should be smaller. This means that the energy of the products compared to the reactants is much higher in energy. This means that in order to form these products, you would require energy to do so and the final products are less stable due to this higher free energy. This would mean that not only is this reaction nonspon, but also endergonic as well AKA consumes energy.
D. Nonspontaneous. This activation barrier is preventing reaction to move forward.
Note: Endothermic and exothermic are associated with enthalpy. Free energy DOES depend on enthalpy AND entropy. BUT, remember that in order to safely conclude endothermic or exothermic, we need to know if it consumes or releases HEAT. But there is not enough information about this

63
Q

What would happen in the reaction of H2SO4(aq) ⇔ H+(aq) + HSO4- (aq), if the pH has been increased?

A

An increase in pH means a decrease in [H+] => right shift in reaction

64
Q

What would happen in the reaction H3PO4(aq) + H2O(l) ⇔ H3O+(aq) + H2PO4-(aq), if water is removed (without changing the temperature)?

A

Decrease in H2O leads to a left shift. All [ ] would increase proportionately; because there are more products than reactants (and the stoichiometric coefficients is 1 for each reactant and product), the value of Q will increase.

65
Q

2(g) + 3H2(g) ⇔ 2NH3(g) Increase in Pressure for this system leads to:

A

Remember that Increase in pressure means there is increase in pressure for the whole system! Therefore both reactants and products can feel this change.
Increase in P, leads to increase in moles in the side of the reaction with less moles. Therefore for this system, there will be an increase in volume for products with an increase in pressure. Therefore there is a decrease in reactants.

66
Q

N2(g) + 3H2(g) ⇔ 2NH3(g) Decrease in pressure for this system leads to:

A

Remember that decrease in pressure means there is a decrease in pressure for the whole system! Therefore both reactants and products can feel this change.
Decrease in P, leads to decrease in moles in the side of the reaction with more moles. Therefore for this system, there will be a decrease in volume for the products, with an decrease in pressure. Therefore there is an increase in reactant

67
Q

What would happen in the reaction of 2C(s) +O2(g) ⇔ 2CO(g), if the P of the reaction vessel is decrease?

A

Increase in P => shifts in reaction to the side with more moles of gas. Therefore right shift to increase products

68
Q

N2O4(g) ⇔ 2NO2(g) Say the reaction is endothermic with an increase in temperature. What do you expect to happen?

A

Reaction should shift right.

69
Q

N2O4(g) ⇔ 2NO2(g) Say this reaction is endothermic. What do you expect to happen if heat was removed?

A

Removal of heat => decrease in temperature. This would cause the reaction to shift left.

70
Q

What would happen in the reaction of CH4(g) + 2O2(g) ⇔ CO2(g) + 2H2O(l) + heat, if the reaction vessel is warmed?

A

Heat is a product in this reaction, and therefore exothermic. Therefore increase in heats shifts the reaction to the left

GC/OC (5 decks)

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