General Inorganic Chemistry and Analytical Chemistry Flashcards
Which of the following is a homogenous mixture?
I. water
II. water and alcohol
III. air
A. I, II and III
B. II and III only
C. I and II only
D. I and III only
B. II and III only
NH3 is
A. trigonal planar
B. tetrahedral
C. trigonal pyramid
D. linear
C. trigonal pyramid
PH3 is
A. trigonal planar
B. tetrahedral
C. trigonal pyramid
D. linear
C. trigonal pyramid
Water is a _____ molecule
A. diatomic
B. triatomic
C. monoatomic
D. tetraatomic
B. triatomic
Transition elements are found in the
A. d and f block
B. p block
C. s block
D. d block
A. d and f block
An atomic bond resulting from the formation of a molecular orbital by the head-on collision of atomic orbitals.
A. sigma bond
B. ionic bond
C. pi bond
D. covalent bond
A. sigma bond
Which does not belong to the group?
A. Cu
B. B
C. Si
D. As
A. Cu
The most abundant element in the solar system is
A. hydrogen
B. nitrogen
C. oxygen
D. helium
A. hydrogen
P1V1/T1=P2V2/T2 is
A. Charles law
B. Ideal gas law
C. Combined Boyle’s & Charles law
D. Amagat’s law
C. Combined Boyle’s & Charles law
H+ is a an _____.
A. proton
B. electron
C. element
D. neutron
A. proton
In which of the following is the size of particles increasing?
A. colloids, solution, suspension
B. colloids, suspension, solution
C. solution, suspension, colloids
D. suspension, solution, colloids
A. colloids, solution, suspension
Which of the following is the most polar bond?
A. N - O
B. C - C
C. C -H
D. H - F
D. H - F
The pair of electrons which do not participate in the bonding is called
A. ione pair of non-bonding electrons
B. ionic bond
C. covalent bond
D. bonding electrons
A. ione pair of non-bonding electrons
A chemical reaction which requires heat to produce products.
A. reversible reaction
B. irreversible reaction
C. exothermic reaction
D. endothermic reaction
D. endothermic reaction
It is define as the tendency of an atom to attract electrons.
A. ionization energy
B. electronegativity
C. exothermic reaction
D. activation energy
B. electronegativity
Dispersion of solid or liquid particles of microscopic size in a gas media such as smoke is
A. a soot
B. a vapor
C. a mist
D. an aerosol
D. an aerosol
It is a proton donor.
A. Arrhenius acid
B. Lewis acid
C. Bronsted acid
D. Acetic acid
C. Bronsted acid
Which of the following has the greatest affinity to electrons?
A.Na
B. Br
C. Cl
D. K
C. Cl
Elements in a given period have the same
A. atomic weight
B. maximum principal quantum number
C. maximum azimuthal quantum number
D. valence electron structure
B. maximum principal quantum number
Electron affinity is defined as
A. the change in energy when a gaseous atom in its ground state gains an electron
B. the pull an atom has on the electrons in chemical bond
C. the energy required to remove a valence electron from a neutral gaseous atom in its ground state
D. the energy difference between an electron in its ground and exited states
A. the change in energy when a gaseous atom in its ground state gains an electron
A triple bond consist of
A. 3 sigma bonds
B. 1 pi & 2 sigma bonds
C. 1 sigma & 2 pi bonds
D. 3 pi bonds
C. 1 sigma & 2 pi bonds
Colligative properties depend on
A. number of solute particles
B. temperature of solution
C. nature of solute
D. nature of solvent
A. number of solute particles
It is the Greek word for “salt forming”
A. actinides
B. lanthanides
C. halogen
D. transition
C. halogen
Who discovered radium?
A. Marie Curie
B. John Priestly
C. Ernest Rutherford
D. John Dalton
A. Marie Curie
Aqua regia is a mixture of
A. hydrochloric & perchloric acid
B. hydrochloric, nitric & perchloric acid
C. nitric & perchloric acid
D. nitric & hydrochloric acid
D. nitric & hydrochloric acid
Mayonnaise and milk are examples of
A. emusion
B. suspension
C. colloid
D. mixture
A. emusion
Colloidal dispersion has ______ phase while a suspension has ______ phases.
A. 1 and 2
B. 1 and 1
C. 2 and 1
D. 2 and 2
A. 1 and 2
Which of the following has no definite stricture?
A. crystalline
B. amorphous
C. amphoteric
D. allotroph
B. amorphous
Who discovered positron?
A. Rutherford
B. Chadwick
C. Goldstein
D. Anderson
D. Anderson
How many halogens are there in period three?
A. 6
B. 5
C. 4
D. 1
D. 1
It is a substance that yields hydronium ions in aqueous solution.
A. Arrhenius acid
B. Lewis acid
C. Bronsted acid
D. Lewis acid
C. Bronsted acid
What expressions of concentration are independent of temperature?
A. molality and mole fraction
B. molarity and normality
C. molarity and mole fraction
D. molarity and J molarity
A. molality and mole fraction
A yellowish gas.
A. chlorine
B. carbon dioxide
C. nitrogen
D. hydrogen
A. chlorine
Which of the following is the lightest?
A. alpha particle
B. proton
C. beta particle
D. hydrogen
C. beta particle
Group 1R elements are also known as
A. alkaline earth metals
B. Halogen
C. alkali metals
D. chalcogen
C. alkali metals
Which of the following statement is/are correct?
I. Liquid water is denser than ice.
II. Ice is denser than liquid water.
III. Ice and liquid water have equal densities.
IV. Ice has a more open structure than liquid water due to the allignment of hydrogen molecules.
V. The molecules of liquid water are farther apart than the molecules of ice
A. III and IV only
B. II and IV only
C. I, IV and V only
D. I and IV only
C. I, IV and V only
Atomic number is equal to the
A. mass number
B. number of protons
C. number of electrons
D. number of neutrons
B. number of protons
One atomic mass unit is equivalent to _____ of the atomic weight of carbon.
A. 12 times
B. 1/12
C. 1/3
D.1/4
B. 1/12
The energy needed to remove the most loosely bonded electron of an atom is the
A. ionization energy
B. electron affnity
C. electronegavity
D. kinetic energy
A. ionization energy
Who stated that the properties of elements are periodic functions of their atomic weights not atomic number?
A. Ernest Rutherford
B. Henry Moseley
C. Dmitri Mendeleev
D. Neils Bohr
C. Dmitri Mendeleev
Calcuim carbonate is also known as
A. chalk
B. feldspar
C. charcoal
D. silica
A. chalk
Which of the following has the least strength?
A. covalent bond
B. electrovalent bond
C. van der waals bond
D. ionic bond
C. van der waals bond
How many neutrons are there in platinum atom?
A. 78
B. 117
C. 195
D. 273
B. 117
Two major types of chemical bonds are observed in chemical bonding: ionic covalent. Which of the following has the bond that is least ionic in character?
A. NaCl
B. H2O
C. CH4
D. H2
D. H2
The most abundant element in the solar system is
A. hydrogen
B. Oxygen
C. nitrogen
D. argon
A. hydrogen
The number of electrons in an atom of an element is equal to
A. atomic weight
B. atomic number
C. equivalent weight
D. electron affinity
B. atomic number
According to Lewis definition, a base is that which
A. gives hydronium ions
B. accepts an electron pair
C. donates an electron
D. is protogenic
B. accepts an electron pair
The composition of the nucleus of deuterium is
A. one electron, one proton
B. one protons, one neutron
C. one neutron, one electron
D. two protons, one electron
B. one protons, one neutron
Which of the following is the most electronegative?
A. fluorine
B. bromine
C. chlorine
D. iodine
A. fluorine
What is the molecular weight of ammonium perchlorate?
A. 116.45 g/mol
B. 97.55 g/mol
C. 122.20 g/mol
D. 86.21 g/mol
A. 116.45 g/mol
An uneven sharing of electrons between two atoms indicate
A. bonding
B. electronegativity
C. coupling
D. polarity
D. polarity
All of the following are colligative properties, except
A. solubility
B. vapor pressure lowering
C. freezing point depression
D. boiling point elevation
A. solubility
The number that expresses the oxidation state of an atom of an element or group is called the
A. indicator
B. displacement factor
C. valence
D. electrolyte
C. valence
A solution used principally to control the pH value of a solution to a point where selective precipitation can be made.
A. acid solution
B. basic solution
C. neutral solution
D. buffer solution
D. buffer solution
Hydrogen is common to all
A. acids
B. oxides
C. salts
D. metals
A. acids
Defines an acid as a compound that dissolves in water to produce hydronium ions.
A. Arrhenius
B. Bronsted-Lowry
C. Lewis
D. Rutherford
A. Arrhenius
One gram mole of a spacie is weight of the spacie equivalent to its
A. molecular weight
B. atomic number
C. number of nuetrons
D. atomic mass
A. molecular weight
Along a row in the periodic table of elements have the same
A. energy level
B. configuration
C. electronegativity
D. size
A. energy level
The electrons of metals are free to move in solids. This explains why
A. metals are unstable
B. metals have high reflectivity
C. metals can be easily molded
D. metals have high conductivity
D. metals have high conductivity
How many pi bonds are there in a double bond?
A. 0
B. 2
C. 1
D. 3
B. 2
All isotopes of a given element have
A. equal number of protons and neutrons
B. the same number of atomic mass unit
C. the same number of protons
D. the same number of neurons
C. the same number of protons
Used to express the ethanol concentration in beverages.
A. % ethanol
B. years
C. proof
D. kara
C. proof
The universal blood type donor is
A. type A
B. type AB
C. type B
D. type O
D. type O
Which will dissolve fastest in coffee?
A. lump sugar in hot coffee
B. granular sugar in hot coffee
C. granular sugar in cold coffee
D. lump sugar in cold coffee
B. granular sugar in hot coffee
As water boils at 1atm, the temperature
A. increases
B. decreases
C. remains constant at 100°C until all is changed to vapor
D. varies
C. remains constant at 100°C until all is changed to vapor
Saltwater at 1 atm boils at
A. slightly higher than 100°C
B. 100°C
C. less than 100°C
D. 98°C
A. slightly higher than 100°C
The method of measuring the specific heat of liquids and solid is
A. entropy
B. enthalpy
C. thermometry
D. calorimetry
D. calorimetry
Which has the greatest rest mass?
A. alpha particle
B. neuron
C. proton
D. electron
A. alpha particle
Which noble gas is 1% by volume in air
A. argon
B. xenon
C. krypton
D. radon
A. argon
Which of the following is also known as soda lye or caustic soda which is use in manufacture of soap?
A. sodium chloride
B. sodium hydroxide
C. sodium carbonate
D. ammonia
B. sodium hydroxide
A complete fertilizer contains
A. N, P and K
B. N, P and C
C. Na, P and K
D. N, P and S
A. N, P and K
Prussic acid has a formula
A. HNO3
B. HCN
C. C5H5OH
D. H2SO4
B. HCN
An azeotropic mixture is
A. liquid mixture of two or more substances in which the vapor has the same composition as the liquid
B. a solution of two or more substances that cannot be made
C. a mixture of two or more substances where the boiling point cannot be determined
D. solution of two or more substances present in the same amounts in the liquid phase
C. a mixture of two or more substances where the boiling point cannot be determined
Which of the following grades has the highest purity?
A. technical grade
B. reagent grade
C. primary standard
D. USP grade
C. primary standard
The temperature at which a polymer changes from hard and brittle to rubbery and tough is called
A. boiling point
B. glass transition temperature
C. thermosetting temperature
D. melting point
C. thermosetting temperature
Consider the following reaction
KMnO4 + KCI + H2SO4 → MnSO4 + H2O + Cl2
What is the reducing agent?
A. KMnO4
B. Mn
C. KCI
D. CaCl2
A. KMnO4
In HAsO3 of the following is covalently bonded?
A. -5
B. -2
C. +6
D. +3
D. +3
Which of the following is covalently bonded?
A. MgO
B. NaCl
C. KCI
D. CaCl2
A. MgO
Discovered water by exploding hydrogen and oxygen.
A. Lewis
B. Cavendish
C. Lavoiser
D. Huey
B. Cavendish
Buffer solution resists changes in acidity. If an acid is added to a buffer solution, the ______ remains the same
A. pH
B. molality
C. concentration
D. mole fraction
A. pH
Jellies and paints are examples of
A. gen
B. emuision
C. sol
D. aerosol
A. gen
Which of the following is a heavy ductile metal?
A. Mn
B. Ni
C. Mg
D. Al
B. Ni
Optical pyrometer is used to
A. determine the voltage at the junction of dissimilar metal
B. measure temperature of solid objects at temperature above 700°C
C. determine the density of an ideal gas
D. measure turbidity of wastewater
D. measure turbidity of wastewater
Teratogens can cause
A. cancer
B. nervous system breakdown
C. child birth defects
D. skin allergies
B. nervous system breakdown
Which of the following has the least polar bonding?
A. carbon dioxide
B. oxygen
C. nitrogen dioxide
D. sulfur dioxide
B. oxygen
The type of intermolecular bond present in water is
A. extended covalent
B. ionic bond
C. polar bond
D. hydrogen bond
D. hydrogen bond
Which of the following is another allotropic form of graphite?
A. gold
B. silver
C. diamond
D. bronze
C. diamond
All are isoelectronic, expect
A. Mg2+
B. Na+
C. F
D. Ne
C. F
Which of the following does not belong to the group?
A. energy
B. force
C. work
D. heat
B. force
The poorest source of hydrogen is
A. protein, fat and carbohydrate
B. atmosphere
C. fossil fuel
D. water
B. atmosphere
When atoms collide, they do not lose energy. This is because
A. collision are elastic
B. collisions are adiabatic
C. collisions are elastic
D. Collisions are frictionless
C. collisions are elastic
Which is not common property to both hydrogen, oxy gen and nitrogen?
A. their densities are lighter than air
B. weak intermolecular forces
C. tasteless, odorless and colorless gas
D. slightly soluble in water
A hydrocarbon has an empirical formula of CH3. If the molecular weight of the hydrocarbon is 30 g/mol, what is the hydrocarbon?
A. C2H6
B. C2H2
C. C4H10
D. C6H12
A. C2H6
The state at which the rate of forward reaction is equal to the rate of backward reaction.
A. eutectic acid
B. equilibrium state
C. reversible state
D. ideal state
B. equilibrium state
It is a substance that yields hydronium ions in aqueous solution.
A. Arrhenius acid
B. Lewis acid
C. Bronsted acid
D. amphoteric
A. Arrhenius acid
Two bodies are of temperature of 70°F and 200°F respectively. Calculate the difference in temperature in degrees Kelvin.
A. 72.22
B. 65.90
C. 60.25
D. 75.12
A. 72.22
All these about redox are correct except
A. the total number of the electrons lost by the element reduces is equal to the total number of electrons gained by the element oxidized
B. the reducing agent oxidized
C. reduction is loss in positive valence
D. oxidation is loss of electrons
A. the total number of the electrons lost by the element reduces is equal to the total number of electrons
What is the color of commercially available nickel chloride?
A. white
B. yellow
C. red
D. green
D. green
Defines a base as a compound that dissolves in water to produce hydroxide ions
A. another electrons goes from a low energy state to a high one
A. another electrons goes from a low energy state to a high one
When an electron goes from a high energy state to a low one, what occur?
A. another electron goes from a low energy state to a high one
B. the atom moves faster
C. light is given off
D. this process is not possible
C. light is given off
Calculate percent oxygen in Fe2(SO4)3.
A. 37%
B. 44%
C. 40%
D. 48%
D. 48%
A 0.5 M solution of a solute (MW = 57 g/mol) has a density of 2.5 g/mol. Calculate the percent by mass of the solute.
A. 0.75%
B. 2.80%
C. 1.14%
D. 0.42%
C. 1.14%
A 0.5 M solution of a solute (MW = 57 g/mol) has a density of 2.5 g/mol. Calculate the percent by mole of the solute.
A. 0.18%
B. 0.36%
C. 0.25%
D. o.42%
B. 0.36%
A 0.5 M solution of a solute (MW = 57 g/mol) has a density of 2.5 g/mol. Calculate the molality of the solution.
A. 0.20
B. 0.30
C. 0.25
D. 0.40
A. 0.20
A compound has a molecular formula of X4O10. If 1 g of X reacts with oxygen to yield 2.24 g of X4O10, find the element X.
A. S
B. Mg
C. Ca
D. P
A. S
A 1.038 M sucrose solution has a density of 1.1 g/ml. Calculate the molarity of the solution.
A. 12.4 M
B. 9.7 M
C. 10.87 M
D. 9.0 M
A. 12.4 M
A 1.038 M sucrose solution has a density of 1.1 g/ml. Calculate the percent by mass sucrose (C12 H22O11).
A. 30.82%
B. 32.27%
C. 31.15%
D. 34.50%
B. 32.27%
A 1.038 M sucrose solution has a density of 1.1 g/ml. Calculate the percent by mole sucrose (C12 H22O11).
A. 2.45%
B. 2.72%
C. 2.60%
D. 2.84%
A. 2.45%
A 1.038 M sucrose solution has a density of 1.1 g/ml. Calculate the molality of the solution.
A. 1.39 m
B. 2.15 m
C. 1.89 m
D. 2.30 m
A. 1.39 m
How many electrons are removed from an atom that changes its oxidation number from -3 to +5?
A. 2
B. 6
C. 8
D. 4
C. 8
Calculate the molarity of NaOH solution if 5 ml of NaOH is titrated with 25 ml of 0.26 M HCI.
A. 1.0 M
B. 1.5 M
C. 1.3 M
D. 1.7 M
C. 1.3 M
The pH of an aqueous solution which has an analytical concentration of 1E-7 M of hydronium ion is
A. 6.0
B.6.79
C. 7.0
D. 6.69
What reacts with AgNO3 to form a silver mirror?
A. aldehydes
B. Acids
C. ketones
D. esters
A. aldehydes
18.7 g unknown acid is reacted with zinc to produce 800 cc of hydrogen gas at STP. What is the equivalent weight of the acid?
A. 624
B. 173
C. 262
D. 131
What weight of AgNO3 is required to precipitate the chlorides in a 750 mg solution of 14% BaCl2?
A. 256 mg
B. 80 mg
C. 342 mg
D. 171 mg
D. 171 mg
Calculate the pH of a solution prepared by mixing 10 ml of 0.1 N NaOH and 25 ml of 0.1 N HAc.
A. 2.46
B. 12.96
C. 4.57
D. 8.72
C. 4.57
Calculate the pH of a solution prepared by mixing 25 ml of 0.1 N NaOH and 25 ml of 0.1 N HAc.
A. 2.46
B. 12.96
C. 4.57
D. 8.72
D. 8.72
Calculate the pH of a solution prepared by mixing 30 ml of 0.1 N NaOH and 25 ml of 0.1 N HAc.
A. 2.46
B. 12.96
C. 4.57
D. 8.72
B. 12.96
hat is the pH of natural water?
A. 5.6 - 6.2
B. 7.0 - 8.3
C. 4.2 - 4.4
D. 2.2 - 2.4
A. 5.6 - 6.2
Asorbic acid (vitamin C ) contains 40.92 percent C, 4.58 percent H, and O by mass.
A. C3H4O3
B. C3H3O3
C. C3H5O3
D. C6H6O3
A. C3H4O3
How many grams of water are produced in the combustion of 1 g of glucose, C6H12O6 :
C6H12O6(S) + 6O2 (g) → 6CO2 (g) + 6H2O (I)
A. 0.5
B. 0.6
C. 0.7
D. 0.8
B. 0.6
One commercial method used to peel potatoes is to soak them in a solution of NaOH for a short time, remove them from the NaOH, and spray off the peel. The concertration of NaOH is normally in the rangeof 3 to 6M. The NaOH is analyzed periodically. In one such analysis, 45.7 ml of 9.5 M H2SO4 is required to neutralize a 20 ml sample of NaOH solution. What is the contration of the NaOH solution?
A. 1.52 M
B. 1.75 M
C. 2.05 M
D. 2.28 M
D. 2.28 M
A series of measurements are made in order to determine the molar mass of an unknown gas. First, a large flask is evacuated and found to weight 134.567 g. It is then filled with the gas to a pressure of 735 torr at 310°C and reweighed; its mass is now 137.456 g. Finally, the flask filled with water at 31° and found to weigh 1067.9 g. (The density of the water at this temperature is 0.977g/mL). Assuming that the ideal gas equation applies, calculated the molar mass of the unknown gas.
A. 65.2 g/mol
B. 70.8 g/mol
C. 74.2 g/mol
D. 79.7 g/mol
D. 79.7 g/mol
A gaseous mixture containing 50% mol H2 and 50% mol acetaldehyde is initially contained in a rigid vessel at 1 atm. The formation of ethanol occurs, after a time it was noted that the pressure drop 700 mmHg. Calculate the degree of completion of the reaction.
A. 15.8%
B. 17.2%
C. 7.8%
D. 9.2%
C. 7.8%
2320 g of tetra-methanol cyclopentane is denoted in the absence of air in a 1000 L closed bomb.
C9H12N4O18 → 4CO2 + 5CO + 5H2O + H2 +2N2
The temperature in the bomb if the pressure rises to 300kPa is
A .425 K
B. 365 K
C. 285 K
D.345 K
A .425 K
If 1.588 g of nitrogen tetroxide (N2O4) gives a total pressure of 1.0133 bar when partially dissociated in a 500-cm3 glass vessel at 25°C, what is the extent of the reaction?
A. 18.42%
B. 27.81%
C. 38.91%
D. 47.65%
B. 27.81%
A solid metallic element burns in oxygen to produce an oxide which dissolves in water to give the hydroxide of the metal. The hydroxide obtained from 1 gram of metal neutralizes 111.2 ml of normal hydrochloric acid. The specific heat of the metal is 0.228 cal/g °C. What is the valency of the metal?
A. 1
B. 2
C. 3
D. 4
C. 3
A solid metallic element burns in oxygen to produce an oxide which dissolves in water to give the hydroxide of the metal. The hydroxide obtained from 1 gram of metal neutralizes 111.2 ml of normal hydrochloric acid. The specific heat of the metal is 0.228 cal/g °C. What is the equivalent weight of the metal?
A. 9.33
B. 8.992
C. 9.002
D. 9.005
B. 8.992
A 6.30-mg sample of a newly discovered isotope was analyzed and found to contain only 4.75 mg after a period of 27.2 hours. What is the half-life (in hours) of the isotope?
A. 27.2
B. 8.13
C. 92.3
D. 66.7
D. 66.7
Consider the following reaction at equilibrium: N2O4(g)==2NO2(g). If a 5 L reaction vessel, held at constant temperature, is initially filled with 10 mol pure N2O4(g), and if 3.5 mol NO2(g) are found in the vessel once equilibrium has been established, what is the value of the equilibrium constant, Kc, for this reaction (at the temperature of the experiment)?
A. 0.297 M
B. 1.48M
C. 0.424 M
D. 0.0594 M
B. 1.48M
The reaction of Br2(g) and Cl2(g) to form BrCl(g) has an equilibrium constant of 15 at a certain temperature. If 10 grams of BrCl is present in a 15-L reaction vessel, initially, what will be the constant of BrCl at equilibrium?
A. 3.8E-3 mol/L
B. 5.77 E-3 mol/L
C. 1.97 E-3 mol/L
D. 9.9 E-4 mol/L
D. 9.9 E-4 mol/L
Carbom dioxide decomposes at elevated temperature to carbon monoxide and oxygen:
2CO2(g) ↔ 2CO(g) + O2(g)
At 3000 K, 2 mol of CO2 is placed in a 1 L container and allowed to equilibrate. At equilibrium, 0.90 mol CO2 remains. What is the value for Kc at this temperature?
A. 0.82
B. 1.88
C. 2.44
D. 3.12
A. 0.82
If 1 mol of PCl3 and 1 mol of Cl2 are placed in a 5-L container, the following equilibrium is reached. PCl3(g) + Cl2(g) → PCl5(g) Kc= 10 at the t4emperature maintained. What is the equilibrium molar concentration of PCl3?
A. 0.13
B. 0.11
C. 0.14
D. 0.10
B. 0.11
Consider the reaction: H2(g) + I2(g) → 2HI(g) Keq=25. Determine the number of moles of H2 remaining when 1 mole of both H2 and I2 are equilibrated in a liter box.
A. 1/8 mole
B. 2/7 mole
C. 5/7 mole
D. 5/6 mole
B. 2/7 mole
Given the reaction: A + B → 2C; K=50. Determine the final concentration of C when 1 mole of both A and B are added to a 1 liter container containing 0.1 mole of C.
A. 0.78 mole
B. 0.88 mole
C. 1.66 mole
D. 1.85 mole
C. 1.66 mole
For the reaction 2NO2(g) → N2O4(g). At a certain temperature one mole of NO2 is placed in a 1 liter container. After equilibrium is established, there are 0.20 mole of N2O4 present. Calculate the equilibrium constant at this temperature.
A. 55.6 mol/L
B. 5.56 mol/L
C. 5.56 L/mol
D. 55.6 L/mol
B. 5.56 mol/L
For the reaction 2A(g) + B(g) ↔ 3C(g) + D(g). the concentration at equilibrium are 0.30 M of A, 0.60 M of B, 0.20 M of C and 0.50 M of D. Find the equilibrium constant.
A. 0.074
B. 0.047
C. 0.74
D. 0.47
A. 0.074
