Accounting
Anthropology
Archaeology
Art History
Banking
Biology & Life Science
Business
Business Communication
Business Development
Business Ethics
Business Law
Chemistry
Communication
Computer Science
Counseling
Criminal Law
Curriculum & Instruction
Design
Earth Science
Economic
Education
Engineering
Finance
History & Theory
Humanities
Human Resource
International Business
Investments & Securities
Journalism
Law
Management
Marketing
Medicine
Medicine & Health Science
Nursing
Philosophy
Physic
Psychology
Real Estate
Science
Social Science
Sociology
Special Education
Speech
Visual Arts
Science
Q:
Iron oxide ores are reduced to iron metal by exothermic reaction with carbon monoxide:FeO(s) + CO(g) Fe(s) + CO2(g)Which of the following changes in condition will cause the equilibrium to shift to the right?A) add FeOB) add COC) add CO2D) raise the temperature
Q:
The pink and blue species below form a violet colored mixture at equilibrium:[Co(H2O)6]2+ (aq) + 4 Cl- (aq) [CoCl4]2- (aq) + 6 H2O (l)(pink) (blue)If the concentration of [Co(H2O)6]2+ is increased, what happens to the solution?A) The concentration of [CoCl4]2- increases.B) The concentration of [CoCl4]2- decreases.C) The solution becomes colorless.D) No color change is observed.
Q:
For a homogeneous equilibrium of gases, which of the following changes in reaction conditions will not alter the equilibrium concentrations?
A) addition of an inert gas to the reaction mixture
B) addition of reactants or products
C) decreasing the pressure or volume
D) increasing the temperature
Q:
Which of the following changes in reaction conditions will alter the composition of an equilibrium mixture of gases for a reaction having unequal moles of gaseous products and gaseous reactants?
A) addition of reactants or products
B) decreasing the pressure or volume
C) increasing the temperature
D) All of these will alter the equilibrium concentrations.
Q:
"If a stress is applied to a reaction mixture at equilibrium, the reaction occurs in the direction that will relieve the stress." This statement is called
A) the First Law of Thermodynamics.
B) the Law of Combining Volumes.
C) the Law of Mass Action.
D) Le Chtelier's principle.
Q:
Salt solubilities can be compared by the concentration of cation formed when the salt dissolves in the general reaction: MaXb(s) a Mb+(aq) + b Xa-(aq). Given the following salts and their equilibrium constants for the reaction above at 25C, which salt is the least soluble?A) AgCl, Kc = 1.8 10-10B) Ag2SO4, Kc = 1.2 10-5C) CaCO3, Kc = 2.6 10-9D) CaF2, Kc = 1.5 10"10
Q:
The solubility of 1:1 salts is measured by the equilibrium constant for the general reaction: MX(s) = Mn+(aq) + Xn-(aq). Given the following salts and their equilibrium constants for the reaction above at 25C, which salt is the least soluble?
A) MgCO3, Kc = 6.8 10-6
B) CaCO3, Kc = 5.0 10-9
C) SrCO3, Kc = 5.6 10-10
D) BaCO3, Kc = 2.6 10-9
Q:
The equilibrium constant Kc for the reaction HF(aq) + H2O(l) H3O+(aq) +F-(aq) is 3.5 10-4. What is the equilibrium concentration of H3O+ if the initial concentration of HF is 1.0 M?A) 1.0 MB) 3.5 10-2 MC) 1.9 10-2 MD) 1.9 10-4 M
Q:
For acid solutions of the same molarity acid strength is proportional to the equilibrium concentration of H3O+. For equimolar solutions of acids, which equilibrium expression below corresponds to the strongest acid?A) Kc = = 3.5 10-4B) Kc = = 3.5 10-8C) Kc = = 4.5 10-4D) Kc = = 4.9 10-10
Q:
Acids donate protons to water according to the general equation:HA(aq) + H2O(l) H3O+(aq) + A-(aq)Consider the following acids and their equilibrium constants for reaction with water at 25C. If all the acids have the same initial concentration, which is the strongest acid (i.e. which donates the most protons to water)?A) HBrO, Kc = 2.0 10-9B) HNO2, Kc = 4.5 10-4C) HF, Kc = 3.5 10-4D) HIO3, Kc = 1.7 10-1
Q:
Oxalic acid can donate two protons to water in successive reactions:(1) H2C2O4(aq) + H2O(l) H3O+(aq) + HC2O4-(aq)(2) HC2O4-(aq) + H2O(l) H3O+(aq) + C2O42-(aq)If Kc1 = 5.9 10-2 and Kc2 = 6.4 10-5 at 25C, what is the value of Kc for reaction (3)?(3) H2C2O4(aq) + 2 H2O(l) 2 H3O+(aq) + C2O42-(aq)A) 3.8 10-6B) 1.1 10-3C) 5.9 10-2D) 9.2 102
Q:
HNO2(aq) + OH-(aq) NO2-(aq) + H2O(l)If K1 = 4.50 10-4, and K2 = 1.00 1014, find the equilibrium constant, K3.A) 4.50 10-18B) 4.50 1010C) 1.00 1014D) 2.22 1017
Q:
When reaction (1) and (2) below are added together, the result is reaction (3).
Q:
Gaseous hydrogen bromide decomposes at elevated temperatures according to the following equation:2 HBr(g) H2(g) + Br2(g).At a certain temperature a 2.00 L flask is initially filled only with 0.600 mol of HBr. What is the value of Kc at that temperature if the flask contains 0.104 mol of H2 at equilibrium?A) 7.04 10-2B) 4.40 10-2C) 3.00 10-2D) 2.10 10-1
Q:
Ammonium carbamate can dissociate into gases at 25C according to the reaction:NH2COONH4(s) 2 NH3(g) + CO2(g)If sufficient ammonium carbamate is sealed in a flask, the total pressure will be 0.117 atm at equilibrium. What is the value of Kp at 25C?A) 2.37 10-4B) 2.00 10-4C) 1.60 10-3D) 3.42 10-1
Q:
When baking soda is heated it decomposes according to the following reaction:2 NaHCO3(s) Na2CO3(s) + H2O(g) + CO2(g)If sufficient baking soda is placed in a container and heated to 90C, the total pressure of the gases is 0.5451 atm. What is the value of Kp at that temperature?A) 0.07428B) 0.2973C) 0.4228D) 1.091
Q:
Kp is equal to 48.70 at 731 K for the reaction: H2(g) + I2(g) 2 HI(g). Initially the mixture contains 0.08592 atm each of H2 and I2 and 1.0000 atm of HI. What is the pressure of HI at equilibrium?A) 0.7955 atmB) 0.9108 atmC) 0.9140 atmD) 0.9498 atm
Q:
The esterification of acetic acid and ethanol is given by the reaction below:C2H5OH(aq) + CH3COOH(aq) CH3COOC2H5(aq) + H2O(l)When 1.00 mol of ethanol was mixed with 2.00 mol of acid in a 1.00 L flask, 0.86 mol of ester was formed at room temperature. What is the value of the equilibrium constant, Kc?A) 0.43B) 2.3C) 4.6D) 5.4
Q:
Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the reaction:PCl5(g) PCl3(g) + Cl2(g)At 250C, 0.250 M PCl5 is added to a flask. If Kc = 1.80, what are the equilibrium concentrations of each gas?A) [PCl5] = 0.0280 M, [PCl3] = 0.222 M, [Cl2] = 0.222 MB) [PCl5] = 1.25 M, [PCl3] = 0.474 M, [Cl2] = 0.474 MC) [PCl5] = 1.80 M, [PCl3] = 1.80 M, [Cl2] = 1.80 MD) [PCl5] = 2.27 M, [PCl3] = 2.02 M, [Cl2] = 2.02 M
Q:
The equilibrium constant, Kp, equals 3.40 for the isomerization reaction:cis-2-butene trans-2-butene.If a flask initially contains 0.250 atm of cis-2-butene and 0.125 atm of trans-2-butene, what is the equilibrium pressure of each gas?A) P(cis-2-butene) = 0.037 atm, P(trans-2-butene) = 0.125 atmB) P(cis-2-butene) = 0.048 atm, P(trans-2-butene) = 0.165 atmC) P(cis-2-butene) = 0.074 atm, P(trans-2-butene) = 0.250 atmD) P(cis-2-butene) = 0.085 atm, P(trans-2-butene) = 0.290 atm
Q:
At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction:2 ICl(g) I2(g) + Cl2(g).What is the equilibrium concentration of ICl if 0.75 mol of I2 and 0.75 mol of Cl2 are initially mixed in a 2.0-L flask?A) 0.23 MB) 0.28 MC) 0.45 MD) 0.56
Q:
Cyclohexane (C6H12) undergoes a molecular rearrangement in the presence of AlCl3 to form methylcyclopentane (CH3C5H9) according to the equation:C6H12 CH3C5H9If Kc = 0.143 at 25C for this reaction, find the equilibrium concentrations of C6H12 and CH3C5H9 if the initial concentrations are 0.200 M and 0.100 M, respectively.A) [C6H12] = 0.0625 and [CH3C5H9] = 0.062 MB) [C6H12] = 0.138 and [CH3C5H9] = 0.162 MC) [C6H12] = 0.262 M and [CH3C5H9] = 0.038 MD) [C6H12] = 0.282 and [CH3C5H9] = 0.018 M
Q:
The following two isomers of C3H7NO exist in equilibrium with each other in solution: If Kc = 0.57 at 25C and the initial concentration of the reactant is 0.50 M and the product is 0.70 M, what are the concentrations at equilibrium?
A) [reactant] = 0.43 M and [product] = 0.24 M
B) [reactant] = 0.67 M and [product] = 0.38 M
C) [reactant] = 0.76 M and [product] = 0.44 M
D) [reactant] = 0.82 M and [product] = 0.47 M
Q:
For the isomerization reaction:
butane ⇌ isobutane
Kp equals 25 at 500C. If the initial pressures of butane and isobutane are 10. atm and 0.0 atm, respectively, what are the pressures of the two gases at equilibrium?
A) P(butane) = 0.38 atm and P(isobutane) = 9.6 atm
B) P(butane) = 0.40 atm and P(isobutane) = 10. atm
C) P(butane) = 9.6 atm and P(isobutane) = 0.38 atm
D) P(butane) = 10 atm and P(isobutane) = 0.40 atm
Q:
At a certain temperature, Kc equals 1.4 102 for the reaction:2 CO(g) + O2(g) 2 CO2(g).If a 2.50-L flask contains 0.400 mol of CO2 and 0.100 mol of O2 at equilibrium, how many moles of CO are also present in the flask?A) 0.422 molB) 0.169 molC) 0.107 molD) 0.0114 mol
Q:
An equilibrium mixture of CO, O2 and CO2 at a certain temperature contains 0.0010 M CO2 and 0.0015 M O2. At this temperature, Kc, equals 1.4 102 for the reaction:2 CO(g) + O2(g) 2 CO2(g).What is the equilibrium concentration of CO?A) 4.8 10-6 MB) 2.2 10-3 MC) 9.3 10-2 MD) 3.1 10-1 M
Q:
At a certain temperature, bromine and nitric oxide react to form nitrosyl bromide:Br2(g) + 2 NO(g) 2 NOBr(g).When 0.010 mol Br2 is mixed with 0.025 mol NO and 0.015 mol NOBr in a 2.50 L flask, the concentration of NOBr decreases. Which statement below is true?A) Kc < 36B) Kc > 36C) Kc < 90D) Kc > 90
Q:
At a certain temperature, bromine and nitric oxide react to form nitrosyl bromide:Br2(g) + 2 NO(g) 2 NOBr(g).When initial amounts of Br2, NO, and NOBr are mixed, the concentration of NOBr increases. Which statement below is true?A) Kc < QB) Kc > QC) Kc = QD) More information is needed to make a statement about Kc.
Q:
Cyclohexane (C6H12) undergoes a molecular rearrangement in the presence of AlCl3 to form methylcyclopentane (MCP) according to the equation:C6H12 MCPIf Kc = 0.143 at 25C for this reaction, predict the direction the reaction will shift if the initial concentrations of C6H12 and MCP are 0.200 M and 0.100 M, respectively. The systemA) will shift left.B) will shift right.C) is already at equilibrium.D) is not at equilibrium and will remain in an unequilibrated state.
Q:
The equilibrium constant, Kp, equals 3.40 at 25C for the isomerization reaction:cis-2-butene trans-2-butene.If a flask initially contains 1.00 atm of each gas, in what direction will the system shift to reach equilibrium?A) It will shift left.B) It will shift right.C) The system is already at equilibrium.D) The system is not at equilibrium and will remain in an unequilibrated state.
Q:
The equilibrium constant is equal to 5.00 at 1300 K for the reaction:2 SO2(g) + O2(g) 2 SO3(g).If initial concentrations are [SO2] = 1.20 M, [O2] = 0.45 M, and [SO3] = 1.80 M, the system isA) at equilibrium.B) not at equilibrium and will remain in an unequilibrated state.C) not at equilibrium and will shift to the left to achieve an equilibrium state.D) not at equilibrium and will shift to the right to achieve an equilibrium state.
Q:
For the reaction: 4 HCl(g) + O2(g) 2 Cl2(g) + 2 H2O(l), the equilibrium constant is 0.063 at 400 K. If the reaction quotient is 0.100, which of the following statements is not correct?A) [HCl] will increase.B) [O2] will increase.C) [Cl2] will decrease.D) [H2O] will increase.
Q:
Which statement is true for a reaction with Kc equal to 2.43 10-12?
A) Increasing the temperature will not change the value of Kc.
B) There are appreciable concentrations of both reactants and products.
C) The reaction proceeds hardly at all towards completion.
D) The reaction proceeds nearly all the way to completion.
Q:
For the reaction, A(g) + 2 B(g) 2 C(g), Kc = 1 10-10 at 25C. Which of the following statements is true?A) n = +1B) The concentration of the products is greater than the concentration of the reactants.C) The reaction is favored in the reverse direction.D) The value of Kp will be larger than the value for Kc.
Q:
Given the hypothetical reaction: 2 A(s) + x B(g) 3 C(g), Kp = 0.0105 and Kc = 0.45 at 250C. What is the value of the coefficient x?A) 1B) 2C) 3D) 4
Q:
If Kc = 0.900, and Kp = 538 for a hypothetical reaction, which of the equations below could represent the reaction at 25C?A) A(g) + B(s) 3 C(g)B) A(l) + 2 B(g) 2 C(g)C) B(g) C(l) + D(l)D) A(g) 2 C(s) + D(g)
Q:
For which one of the following reactions will Kc = Kp?A) CO(g) + 2 H2(g) CH3OH(g)B) ZnO(s) + CO(g) Zn(s) + CO2(g)C) 2 O3(g) 3 O2(g)D) COCl2(g) CO(g) + Cl2(g)
Q:
What is the equilibrium constant, Kc, for the reaction:2 Hg(l) + O2(g) 2 HgO(s)if the amounts of reactants and products at equilibrium are: 1.00 g of HgO(s), 2.00 mL of Hg(l), and 1.60 M O2(g)? (The molar mass and density of HgO(s) is 217 g/mol, and 1.10 g/cm3. The molar mass and density of Hg(l) is 201 g/mol, and 13.6 g/mL.)A) 6.85 10-4B) 4.66 10-2C) 0.625D) 1.46 103
Q:
What is the value for Kc for the following reaction:PbCl2(s) Pb2+(aq) + 2 Cl-(aq),if PbCl2(s) = 1.50 grams, [Pb2+] = 1.6 10-2 M and [Cl-] = 3.2 10-2 M at equilibrium? (The molar mass of PbCl2(s) is 278 g/mol and its density is 5.85 g/cm3.)A) 7.6 10-7B) 1.6 10-5C) 6.2 104D) 1.3 106
Q:
What is the equilibrium equation for the following reaction?2 H2O (l) H3O+ (aq) + OH- (aq)A) Kc = B) Kc = C) Kc = D) Kc = [H3O+] [OH-]
Q:
What is the equilibrium equation for the following reaction?FeS(s) + 2 H3O+ (aq) Fe2+(aq) + H2S (aq) + 2 H2O (l)A) Kc = B) Kc = C) Kc = D) Kc =
Q:
What is the equilibrium equation for the following reaction?C2H4 (g) + 3 O2 (g) 2 CO2 (g) + 2 H2O (l)A) Kp = B) Kp = C) Kp = D) Kp =
Q:
What is the equilibrium equation for the dissociation of formic acid in water?HCOOH (aq) + H2O (l) H3O+ (aq) + HCOO- (aq)A) Kc = B) Kc = C) Kc = D) Kc =
Q:
Which equilibrium below is homogeneous?A) BaSO4(s) Ba2+(aq) + SO42-(aq)B) 2 H2O2(l) 2 H2O(l) + O2(g)C) NH4NO3(s) N2O(g) + 2 H2O(g)D) 2 CO(g) + O2(g) 2 CO2(g)
Q:
As a rule, which of the following phases are not included in the equilibrium constant expression?
I. pure liquids II. pure solids III. aqueous solutions IV. gases
A) I, II
B) I, IV
C) III, IV
D) II, III
Q:
A 1.50 L vessel contains an equilibrium mixture of 0.100 mol of NO, 0.150 mol of Br2, and0.250 mol of NOBr at 25C. What is the value of Kp for the reaction below?2 NO(g) + Br2(g) 2 NOBr(g)A) 2.56B) 62.5C) 1.28 102D) 1.53 103
Q:
The decomposition of ammonia is: 2 NH3(g) N2(g) + 3 H2(g). If the pressure of ammonia is1.0 10-3 atm, and the pressures of N2 and H2 are each 0.20 atm, what is the value for Kp' at 400C for the reverse reaction?A) -6.2 10-4B) -1.6 103C) 6.2 10-4D) 1.6 103
Q:
The decomposition of ammonia is: 2 NH3(g) N2(g) + 3 H2(g). If the partial pressure of ammonia is 1.6 10-3 atm and the partial pressures of N2 and H2 are each 0.25 atm at equilibrium, what is the value for Kc at 400C for the forward reaction?A) 0.50B) 1.4C) 1.5 103D) 4.6 106
Q:
The decomposition of ammonia is: 2 NH3(g) = N2(g) + 3 H2(g). If Kp is 1.5 103 at 400C, what is the partial pressure of ammonia at equilibrium when N2 is 0. 10 atm and H2 is 0.15 atm?
A) 2.2 10- 7 atm
B) 4.7 10- 4 atm
C) 2.1 103 atm
D) 4.4 106 atm
Q:
Phosphorus pentachloride decomposes to phosphorus trichloride and chlorine gas at elevated temperatures by the following reaction:PCl5(g) PCl3(g) + Cl2(g). If Kc = 1.8 at 250C.What is the value of Kp at the same temperature?A) 4.2 10-2B) 8.8 10-2C) 65D) 77
Q:
If Kc = 2.0 x 1033 at 25C, for the following reaction: H2(g) + Cl2(g) 2 HCl(g), then find Kp at the same temperature.A) 8.2 1031B) 9.7 1032C) 2.0 1033D) 4.9 1034
Q:
Given the reaction at a certain temperature: 2 HI(g) H2(g) + I2(g). At equilibrium, the partial pressure of HI is 1.8 10-3 atm, and the partial pressures for H2 and I2 are 0.10 atm each. Find Kp at that temperature.A) 3.2 10-4B) 5.6 101C) 3.1 103D) 3.1 104
Q:
The oxidation of sulfur dioxide by oxygen to sulfur trioxide has been implicated as an important step in the formation of acid rain: 2 SO2(g) + O2(g) 2 SO3(g). If the equilibrium partial pressures of SO2, O2, and SO3 are 0.564 atm, 0.102 atm, and 0.333 atm respectively at 1000 K, what is Kp at that temperature?A) 0.292B) 3.42C) 5.79D) 8.11
Q:
What is true about the relationship of Kp and Kc for the reaction:2 CH4(g) + 3 O2(g) 2 CO(g) + 4 H2O(g)?A) Kp < KcB) Kp = KcC) Kp > KcD) Kp and Kc are not related.
Q:
Kp = 1.5 103 at 400C for the reaction 2 NH3(g) N2(g) + 3 H2(g). What is the value of Kp for the reaction:2 N2(g) + 6 H2(g) 4 NH3(g)?A) 4.4 10-7B) 3.3 10-4C) 6.7 10-4D) 2.3 106
Q:
Write the equilibrium equation for the reverse reaction:2 CH4(g) + 3 O2(g) 2 CO(g) + 4 H2O(g)A) Kp' = B) Kp' = C) Kp' = D) Kp' =
Q:
Write the equilibrium equation for the forward reaction:2 CH4(g) + 3 O2(g) 2 CO(g) + 4 H2O(g)A) Kp = B) Kp= C) Kp = D) Kp =
Q:
What is the equilibrium equation for the reaction:NH4NO3(s) N2O(g) + 2 H2O(g)?A) Kp = [N2O]B) Kp = [N2O][H2O]C) Kp = [N2O][H2O]2D) Kp =
Q:
Kp is related to Kc by the equation Kp = Kc (RT)n. What is the value of n for the reaction below? NH4NO3(s) N2O(g) + 2 H2O(g)A) -2B) -1C) +1D) +2
Q:
Which one of the following statements about the equilibrium constant, Kp, is false?A) n is equal to the sum of the coefficients of the gaseous products minus the sum of the coefficients of the gaseous reactants.B) The relationship between Kp and Kc is: Kp =Kc (RT)nC) The units for Kp are usually omitted.D) Total pressures are used in the equilibrium equation in place of molar concentrations.
Q:
If Kc equals 0.11 at 25C for the reaction: N2O4(g) 2 NO2(g), what is Kc for the reaction: NO2(g) 1/2 N2O4(g)?A) 0.33B) 3.0C) 4.5D) 9.1
Q:
If Kc = 7.04 10-2 for the reaction: 2 HBr(g) H2(g) + Br2(g), what is the value of Kc for the reaction: 1/2 H2(g) + 1/2 Br2(g) == HBr(g)?A) 3.52 10-2B) 0.265C) 3.77D) 28.4
Q:
For the reaction: N2(g) + 2 O2(g) 2 NO2(g), Kc = 8.3 10-10 at 25C. What is the concentration of N2 gas at equilibrium when the concentration of NO2 is twice the concentration of O2 gas?A) 2.1 10-10 MB) 4.2 10-10 MC) 2.4 109 MD) 4.8 109 M
Q:
Given the reaction: 2 HI H2 + I2. If Kc' for the reverse reaction is 1.85 10-2 at 425C, what is Kc for the forward reaction at the same temperature?A) -1.85 10-2B) 1.85 10-2C) 3.70 10-2D) 54.1
Q:
A mixture of carbon monoxide, hydrogen, and methanol is at equilibrium. The balanced chemical equation is: CO(g) + 2H2(g) CH3OH(g). At 250C, the mixture contains 0.0960 M CO, 0.191 M H2, and 0.150 M CH3OH. What is the value for Kc?A) 2.33 10-2B) 0.244C) 4.09D) 42.8
Q:
Nitric oxide reacts with oxygen to form nitrogen dioxide:2 NO(g) + O2(g) 2 NO2(g)What is Kc' for the reverse reaction if the equilibrium concentration of NO is 0.300 M, O2 is 0.200 M, and NO2 is 0.530 M at 25C?A) 0.0340B) 0.0641C) 0.624D) 15.6
Q:
Nitric oxide reacts with oxygen to form nitrogen dioxide:2 NO(g) + O2(g) 2 NO2(g)What is Kc for the forward reaction if the equilibrium concentration of NO is 0.200 M, O2 is 0.100 M, and NO2 is 0.250 M at 25C?A) 8.00 10-2B) 6.41 10-2C) 12.5D) 15.6
Q:
Write the equilibrium equation for the reverse reaction:
2 CH4 (g) + 3 O2 (g) ⇌ 2 CO (g) + 4 H2O (g)
A) Kc = B) Kc = C) Kc = D) Kc =
Q:
Write the equilibrium equation for the forward reaction:2 CH4 (g) + 3 O2 (g) 2 CO (g) + 4 H2O (g)A) Kc = B) Kc = C) Kc = D) Kc =
Q:
If Kc is the equilibrium constant for a forward reaction, 2 A⇌ B, what is Kc for the reaction 4 A⇌ 2B?
A) Kc
B) Kc
C) 2 Kc
D) (Kc)2
Q:
If Kc is the equilibrium constant for a forward reaction what is Kc for the reverse reaction?
A) - Kc
B) Kc
C) (Kc)-1
D) none of these
Q:
Which statement about the equilibrium constant is true? The value of Kc
A) changes as product concentration changes.
B) changes as reactant concentration changes.
C) changes as temperature changes.
D) never changes.
Q:
Which of the following statements is false regarding the equilibrium constant, Kc?
A) Kc for a reaction at a particular temperature always has the same value.
B) Kc for the reverse reaction is the negative of Kc for the forward reaction.
C) The numerical value of Kc depends on the form of the balanced equation.
D) When quoting Kc it is customary to omit units.
Q:
The equilibrium equation is also known as the law of
A) coefficients.
B) constant concentration.
C) dynamic equilibrium.
D) mass action.
Q:
Which one of the following statements does not describe the equilibrium state?
A) Equilibrium is dynamic and there is no net conversion to reactants and products.
B) The concentration of the reactants is equal to the concentration of the products.
C) The concentration of the reactants and products reach a constant level.
D) The rate of the forward reaction is equal to the rate of the reverse reaction.
Q:
What is the species present at reaction stage 2?
A) an intermediate
B) a product
C) a reactant
D) a transition state
Q:
What is the species present at reaction stage 1?
A) an intermediate
B) a product
C) a reactant
D) a transition state
Q:
Which of the elementary reactions shown above has a molecularity of three?
A) elementary reaction (a)
B) elementary reaction (b)
C) elementary reaction (c)
D) elementary reactions (a), (b), and (c)
Q:
Which of the elementary reactions shown above has a molecularity of two?
A) elementary reaction (a)
B) elementary reaction (b)
C) elementary reaction (c)
D) elementary reactions (a), (b), and (c)
Q:
Which of the elementary reactions shown above has a molecularity of one?
A) elementary reaction (a)
B) elementary reaction (b)
C) elementary reaction (c)
D) elementary reactions (a), (b), and (c)