AP Chemistry Unit 5 Progress Check MCQ Answers
1. The rate of the reaction CH3I+NaOH→CH3OH+NaICH3I+NaOH→CH3OH+NaI is expressed as rate = k[CH3I][NaOH]. What is the order of the reaction concerning CH3I and NaOH?
a) Zero order
b) First order
c) Second order
d) Third order
2. In the reaction CH3I+NaOH→CH3OH+NaICH3I+NaOH→CH3OH+NaI, the rate equation is given as rate = k[CH3I][NaOH]. What is the rate law expression indicating?
a) The reaction rate is independent of the concentration of CH3I.
b) The reaction rate is directly proportional to the concentration of CH3I.
c) The reaction rate is inversely proportional to the concentration of CH3I.
d) The reaction rate is dependent only on the concentration of NaOH.
3. For the reaction CH3I+NaOH→CH3OH+NaICH3I+NaOH→CH3OH+NaI, the rate expression is given as rate = k[CH3I][NaOH]. What is the overall order of the reaction?
a) Zero order
b) First order
c) Second order
d) Third order
4. In the reaction CH3I+NaOH→CH3OH+NaICH3I+NaOH→CH3OH+NaI, the rate equation is expressed as rate = k[CH3I][NaOH]. What does this expression indicate?
a) The rate of the reaction doubles when the concentration of CH3I is doubled.
b) The reaction rate is halved when the concentration of NaOH is halved.
c) The rate of the reaction quadruples when the concentration of CH3I is quadrupled.
d) The reaction rate remains constant regardless of the concentrations of CH3I and NaOH.
5. For the reaction CH3I+NaOH→CH3OH+NaICH3I+NaOH→CH3OH+NaI, the rate expression is given as rate = k[CH3I][NaOH]. What happens to the reaction rate if the concentration of NaOH is tripled while the concentration of CH3I remains unchanged?
a) The rate increases by a factor of 3.
b) The rate decreases by a factor of 3.
c) The rate remains unchanged.
d) The rate increases by a factor of 9.
Unit 7 progress check MCQ
6. For the reaction 2N2O5(g)→4NO2(g)+O2(g), the concentration of N2O5 was measured over time. If the graph of ln[N2O5] vs. time yields a straight line, what is the order of the reaction concerning N2O5?
a) Zero order
b) First order
c) Second order
d) Third order
7. Based on the graphs provided, if the concentration of N2O5 decreases exponentially with time, what is the order of the reaction concerning N2O5?
a) Zero order
b) First order
c) Second order
d) Third order
8. If the concentration of N2O5 decreases linearly with time, what is the order of the reaction concerning N2O5?
a) Zero order
b) First order
c) Second order
d) Cannot be determined from the given information
9. In the given reaction 2N2O5(g)→4NO2(g)+O2(g), if the rate of reaction is directly proportional to the concentration of N2O5, what is the order of the response concerning N2O5?
a) First order
b) Second order
c) Third order
d) Cannot be determined from the given information
10. If the reaction rate is independent of the initial concentration of N2O5, what is the order of the reaction with respect to N2O5?
a) Zero order
b) First order
c) Second order
d) Third order
11. For the radioactive decay process described by the equation Bi83214→Po84214+e−Bi83214→Po84214+e−, which of the following quantities plotted versus time will produce a straight line?
a) The concentration of Polonium-214
b) The concentration of Bismuth-214
c) The ratio of Polonium-214 to Bismuth-214
d) The natural logarithm of the concentration of Bismuth-214
12. In the radioactive decay of Bismuth-214 to Polonium-214 via beta decay, if the half-life of Bismuth-214 is known, which of the following can be determined?
a) The rate constant (k) of the decay reaction
b) The rate of decay of Polonium-214
c) The rate of decay of Bismuth-214
d) The activation energy of the decay reaction
13. Based on the radioactive decay equation provided, if a plot of ln[Bismuth-214] versus time yields a straight line, what can be concluded about the order of the decay reaction?
a) It is zero order.
b) It is first order.
c) It is second order.
d) It is third order.
14. For the radioactive decay process described, if the concentration of Polonium-214 is measured over time and plotted against time, what type of curve would be expected?
a) A straight line
b) A parabolic curve
c) An exponential decay curve
d) A sigmoidal curve
15. If the decay constant (k) for the radioactive decay of Bismuth-214 is determined experimentally, what information does it provide about the decay process?
a) The rate of decay of Polonium-214
b) The rate of decay of Bismuth-214
c) The probability of decay per unit time for each Bismuth-214 nucleus
d) The total number of decay events occurring per unit time
16. Based on the catalyzed decomposition of NH3(g) as represented by the equation 2NH3(g)catalystN2(g)+3H2(g), and the rate of disappearance of NH3(g) measured over time for different initial concentrations, which of the following best represents the rate law for the reaction?
a) Rate=k[NH3]2
b) Rate=k[NH3]
c) Rate=k
d) Rate=k[NH3]2
17. In the catalyzed decomposition of NH3(g) at high temperature, if a plot of the initial rate of reaction versus the initial concentration of NH3(g) yields a straight line passing through the origin, what can be inferred about the reaction order concerning NH3(g)?
a) It is first-order concerning NH3(g).
b) It is second order concerning NH3(g).
c) It is zero order concerning NH3(g).
d) It is the third order concerning NH3(g).
18. If the rate constant (k) for the catalyzed decomposition of NH3(g) is determined experimentally, what information does it provide about the reaction? a) The rate of formation of N2(g) and H2(g)
b) The total amount of NH3(g) consumed
c) The rate of the reaction under specific conditions
d) The concentration of the catalyst used
19. Based on the graph depicting the change in concentration of NH3(g) over time for different initial concentrations, what can be concluded about the effect of initial concentration on the reaction rate?
a) The reaction rate is directly proportional to the initial concentration of NH3(g).
b) The reaction rate is inversely proportional to the initial concentration of NH3(g).
c) The reaction rate is independent of the initial concentration of NH3(g).
d) The reaction rate decreases as the initial concentration of NH3(g) increases.
20. For the chemical reaction mechanism represented by Step 1: H2O2+I−→IO−+H2OH2O2+I−→IO−+H2O and Step 2: H2O2+IO−→H2O+O2+I−H2O2+IO−→H2O+O2+I−, which of the following statements about the overall reaction and rate laws of the elementary responses is correct?
a) The overall reaction is second order, and the rate law for both elementary reactions is first.
b) The overall reaction is second order; the rate law for Step 1 is first order, while the rate law for Step 2 is second.
c) The overall reaction is first order, and the rate law for both elementary reactions is first.
d) The overall reaction is first order, and the rate law for Step 1 is second order, while the rate law for Step 2 is first order.
21. If the rate constant for Step 1 is much greater than that for Step 2, what effect does this have on the overall reaction rate?
a) The overall rate is determined solely by the rate constant of Step 1.
b) The overall rate is determined solely by the rate constant of Step 2.
c) The overall rate is determined by both the rate constants of Step 1 and Step 2.
d) The overall rate is unaffected by the rate constants of Step 1 and Step 2.
22. Which of the following statements accurately describes the role of the intermediate species in the given mechanism?
a) The intermediate species is consumed in the first step and regenerated in the second step.
b) The intermediate species is regenerated in the first step and consumed in the second step.
c) The intermediate species is formed in the first step and consumed in the second step.
d) The intermediate species is formed in the second step and consumed in the first.
23. If the concentration of the reactant H2O2 is doubled, how does this change affect the overall reaction rate?
a) The overall reaction rate increases by a factor of 2.
b) The overall reaction rate increases by a factor of 4.
c) The overall reaction rate decreases by a factor of 2.
d) The rate of the overall reaction remains unchanged.
24. What is the overall stoichiometry of the given chemical reaction mechanism?
a) H2O2+I−→H2O+O2+I−H2O2+I−→H2O+O2+I−
b) H2O2+IO−→H2O+O2+I−H2O2+IO−→H2O+O2+I−
c) H2O2+I−→IO−+H2OH2O2+I−→IO−+H2O
d) H2O2+IO−→IO−+H2OH2O2+IO−→IO−+H2O