Choose the correct answer for each question.

- The rate law for a particular reaction is determined to be R = k[A]
^{2}[B]^{2}. What is the overall order for this reaction?- zero
- first
- second
- third
- fourth

- KClO
_{3}decomposes according to the reaction:2KClOIf the rate of decomposition of potassium chlorate at a certain time is determined to be 2.4 x 10_{3}→ 2KCl + 3O_{2}^{-2}mol s^{-1}. What is the rate of formation of O_{2}at the same time?- 2.4 x 10
^{-2}mol s^{-1} - 1.2 x 10
^{-2}mol s^{-1} - 3.6 x 10
^{-2}mol s^{-1} - 7.2 x 10
^{-2}mol s^{-1} - 1.6 x 10
^{-2}mol s^{-1}

- 2.4 x 10
- For a reaction between X and Y, the following data was obtained:What is the rate law for this reaction?
**[X]**_{0}**[Y]**_{0}**Initial Rate**0.10 0.10 2.0 x 10 ^{3}0.20 0.10 4.0 x 10 ^{3}0.10 0.20 8.0 x 10 ^{3}- R = k[X][Y]
- R = k[X]
^{2}[Y]^{2} - R = k[X][Y]
^{2} - R = k[X]
^{2}[Y] - R = k[Y]
^{2}

- For the following reaction:A → B + Cthat is second order, a linear plot will result when time is plotted against:
- ln[A]
- [A]
- 1/[A]
- ln[B]
- ln[B][C]

- For a first order reaction with a rate constant k = 1.2 x 10
^{-3}s^{-1}, how long will it take for the amount of reactant to be decreased from 0.10 mol to 0.05 mol?- 580 seconds
- 6.7 seconds
- 8.3 x 10
^{3}seconds - 8.3 x 10
^{2}seconds - none of these

- For a first order reaction with a rate constant k = 3.13 x 10
^{2}s^{-1}, how long does it take for the concentration of the only reactant to become 40% of the original amount?- 0.00128 seconds
- 0.00293 seconds
- 0.0450 seconds
- 0.00479 seconds
- 43.2 seconds

- For a second order reaction with a rate constant k = 3.13 x 10
^{2}L mol^{-1}s^{-1}, how long does it take for the concentration of the only reactant to become 70% of the original amount?- 0.00137 seconds
- 0.00746 seconds
- 0.00114 seconds
- 0.0761 seconds
- 0.912 seconds

- Catalysts lower the activation energy of a reaction by:
- adding heat to the reaction system
- providing an alternate pathway for the reaction
- increasing the energy content of the reactants
- changing the value of Δ
*H*for the reaction - none of these

- The following data give the concentration of gaseous butadiene as a function of time at 500 K. Determine the order of the reaction, and the value of the rate constant.
t(sec) C(moles/liter) 195 1.62 x 10 ^{-2}604 1.47 x 10 ^{-2}1246 1.29 x 10 ^{-2}2180 1.10 x 10 ^{-2}4140 0.89 x 10 ^{-2}4655 0.80 x 10 ^{-2}6210 0.68 x 10 ^{-2}8135 0.57 x 10 ^{-2}- first order, k = 1.4 x 10
^{2}s^{-1} - first order, k = 1.4 x 10
^{-2}L mol^{-1}s^{-1} - second order, k = 1.4 x 10
^{-2}L mol^{-1}s^{-1} - second order, k = 1.4 x 10
^{2}L mol^{-1}s^{-1} - zero order, k = -1.4 x 10
^{-2}mol L^{-1}s^{-1}

- first order, k = 1.4 x 10
- The reaction X
_{2}Y → 2X + Y is determined to be first order. What is the integrated rate law for this reaction?- ln[2X + Y] = kt - ln[2X + Y]
_{0} - (1/[X
_{2}Y]) = -kt + (1/[X_{2}Y]_{0}) - [X
_{2}Y] = -kt + [X_{2}Y]_{0} - ln[X
_{2}Y] = -kt + ln[X_{2}Y]_{0} - (1/[2X + Y]) = -kt + (1/[2X + Y]
_{0})

- ln[2X + Y] = kt - ln[2X + Y]
- A certain first-order reaction is 50.0% complete in 4.25 minutes. What is the rate constant for this reaction?
- 0.163 min
^{-1} - 2.95 min
- 6.13 min
- [A]
_{0}/(2t_{1/2}) - 0.0252 min
^{-1}

- 0.163 min
- A certain first order decomposition reaction reaches 65% completion in 18.9 seconds. What is the rate constant for this reaction?
- 18 s
^{-1} - 19.8 s
^{-1} - 9.56 x 10
^{-2}s^{-1} - 2.38 x 10
^{-2}s^{-1} - 5.55 x 10
^{-2}s^{-1}

- 18 s
- The activation energy for the reaction:

Xis 125 kJ/mol and Δ_{2}(*g*) + Y_{2}(*g*) → 2XY(*g*)*E*for the reaction is -45 kJ/mol. The activation energy for the decomposition of XY is:- 45 kJ/mol
- 80 kJ/mol
- 170 kJ/mol
- -80 kJ/mol
- -125 kJ/mol

- Increasing the temperature at which a reaction occurs speeds up the reaction by:
- increasing the frequency of collisions
- increasing the energy of collisions
- activating catalysts
- improving the orientation of collisions
- two of these

- Which of the following statements is TRUE for the catalyzed and uncatalyzed versions of the same reaction?
- The activation energies are the same
- The reaction pathway is the same
- The energy content of the reactants is higher for the uncatalyzed reaction
- Δ
*E*is the same - The energy content of the activated complex is higher for the catalyzed reaction