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What data should be plotted to show that experimental concentration data fit a first-order reaction?


A) What data should be plotted to show that experimental concentration data fit a first-order reaction? A) <sub> </sub>vs. time B) [reactant] vs. time C) ln[reactant] vs. time D) ln(k) vs. E) ln(k) vs. E<sub>a</sub> vs. time
B) [reactant] vs. time
C) ln[reactant] vs. time
D) ln(k) vs. What data should be plotted to show that experimental concentration data fit a first-order reaction? A) <sub> </sub>vs. time B) [reactant] vs. time C) ln[reactant] vs. time D) ln(k) vs. E) ln(k) vs. E<sub>a</sub>
E) ln(k) vs. Ea

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The first-order reaction, SO2Cl2 → SO2 + Cl2, has a rate constant equal to 2.20 × 10-5 s-1 at 593 K. What percentage of the initial amount of SO2Cl2 will remain after 6.00 hours?


A) 1.00%
B) 37.8%
C) 40.2%
D) 62.2%

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Without performing complex calculations, determine the order of a reaction that has the following initial rates for the specified starting concentration: Without performing complex calculations, determine the order of a reaction that has the following initial rates for the specified starting concentration: A) zero order B) first order C) second order D) third order E) impossible to determine


A) zero order
B) first order
C) second order
D) third order
E) impossible to determine

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Given the following balanced equation, determine the rate of reaction with respect to [H2]. N2(g) + 3H2(g) → 2NH3(g)


A) Rate = + Given the following balanced equation, determine the rate of reaction with respect to [H<sub>2</sub>]. N<sub>2</sub>(g) + 3H<sub>2</sub>(g) → 2NH<sub>3</sub>(g) A) Rate = + B) Rate = - C) Rate = + D) Rate = - E) It is not possible to determine the answer without more information.
B) Rate = - Given the following balanced equation, determine the rate of reaction with respect to [H<sub>2</sub>]. N<sub>2</sub>(g) + 3H<sub>2</sub>(g) → 2NH<sub>3</sub>(g) A) Rate = + B) Rate = - C) Rate = + D) Rate = - E) It is not possible to determine the answer without more information. Given the following balanced equation, determine the rate of reaction with respect to [H<sub>2</sub>]. N<sub>2</sub>(g) + 3H<sub>2</sub>(g) → 2NH<sub>3</sub>(g) A) Rate = + B) Rate = - C) Rate = + D) Rate = - E) It is not possible to determine the answer without more information.
C) Rate = + Given the following balanced equation, determine the rate of reaction with respect to [H<sub>2</sub>]. N<sub>2</sub>(g) + 3H<sub>2</sub>(g) → 2NH<sub>3</sub>(g) A) Rate = + B) Rate = - C) Rate = + D) Rate = - E) It is not possible to determine the answer without more information. Given the following balanced equation, determine the rate of reaction with respect to [H<sub>2</sub>]. N<sub>2</sub>(g) + 3H<sub>2</sub>(g) → 2NH<sub>3</sub>(g) A) Rate = + B) Rate = - C) Rate = + D) Rate = - E) It is not possible to determine the answer without more information.
D) Rate = - Given the following balanced equation, determine the rate of reaction with respect to [H<sub>2</sub>]. N<sub>2</sub>(g) + 3H<sub>2</sub>(g) → 2NH<sub>3</sub>(g) A) Rate = + B) Rate = - C) Rate = + D) Rate = - E) It is not possible to determine the answer without more information. Given the following balanced equation, determine the rate of reaction with respect to [H<sub>2</sub>]. N<sub>2</sub>(g) + 3H<sub>2</sub>(g) → 2NH<sub>3</sub>(g) A) Rate = + B) Rate = - C) Rate = + D) Rate = - E) It is not possible to determine the answer without more information.
E) It is not possible to determine the answer without more information.

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Which of the following reactions would you predict to have the largest orientation factor?


A) NOF(g) + NOF(g) → 2NO(g) + F2(g)
B) Br2(g) + H2C=CH2(g) → H2BrC-CBrH2(g)
C) NH3(g) + BCl3(g) → H3N-BCl3(g)
D) H(g) + Cl(g) → HCl(g)
E) All of these reactions should have nearly identical orientation factors.

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What are the units of k in a first-order reaction?


A) mol L-1 s-1
B) mol L-1 s
C) L mol-1 s-1
D) M2 s-1
E) s-1

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Calculate the activation energy, Ea, for a reaction with a frequency factor, A, of 8.12 × 109 s-1 and a rate constant of 3.05 × 104 s-1 at 375 K.


A) 72.5 kJ mol-1
B) 38.9 kJ mol-1
C) 104 kJ mol-1
D) 68.0 kJ mol-1
E) 71.6 kJ mol-1

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Which rate law is bimolecular?


A) rate = k[A][B]2
B) rate = k[A][B]
C) rate = k[A]
D) rate = k[A][B][C][D]
E) rate = k[A][A][B]

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Given the following balanced equation, determine the rate of reaction with respect to [SO2]. 2SO2(g) + O2(g) → 2SO3(g)


A) Rate = - Given the following balanced equation, determine the rate of reaction with respect to [SO<sub>2</sub>]. 2SO<sub>2</sub>(g) + O<sub>2</sub>(g) → 2SO<sub>3</sub>(g) A) Rate = - B) Rate = + C) Rate = - D) Rate = + E) It is not possible to determine the answer without more information. Given the following balanced equation, determine the rate of reaction with respect to [SO<sub>2</sub>]. 2SO<sub>2</sub>(g) + O<sub>2</sub>(g) → 2SO<sub>3</sub>(g) A) Rate = - B) Rate = + C) Rate = - D) Rate = + E) It is not possible to determine the answer without more information.
B) Rate = + Given the following balanced equation, determine the rate of reaction with respect to [SO<sub>2</sub>]. 2SO<sub>2</sub>(g) + O<sub>2</sub>(g) → 2SO<sub>3</sub>(g) A) Rate = - B) Rate = + C) Rate = - D) Rate = + E) It is not possible to determine the answer without more information. Given the following balanced equation, determine the rate of reaction with respect to [SO<sub>2</sub>]. 2SO<sub>2</sub>(g) + O<sub>2</sub>(g) → 2SO<sub>3</sub>(g) A) Rate = - B) Rate = + C) Rate = - D) Rate = + E) It is not possible to determine the answer without more information.
C) Rate = - Given the following balanced equation, determine the rate of reaction with respect to [SO<sub>2</sub>]. 2SO<sub>2</sub>(g) + O<sub>2</sub>(g) → 2SO<sub>3</sub>(g) A) Rate = - B) Rate = + C) Rate = - D) Rate = + E) It is not possible to determine the answer without more information.
D) Rate = + Given the following balanced equation, determine the rate of reaction with respect to [SO<sub>2</sub>]. 2SO<sub>2</sub>(g) + O<sub>2</sub>(g) → 2SO<sub>3</sub>(g) A) Rate = - B) Rate = + C) Rate = - D) Rate = + E) It is not possible to determine the answer without more information.
E) It is not possible to determine the answer without more information.

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Without performing complex calculations, determine the order of a reaction that has the following initial rates for the specified starting concentration: Without performing complex calculations, determine the order of a reaction that has the following initial rates for the specified starting concentration: A) zero order B) first order C) second order D) third order E) impossible to determine


A) zero order
B) first order
C) second order
D) third order
E) impossible to determine

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Write a balanced reaction for which the following rate relationships are true. Rate = Write a balanced reaction for which the following rate relationships are true. Rate = = = - A) N<sub>2</sub> + O<sub>2 </sub>→<sub> </sub> <sub> </sub> N<sub>2</sub>O B) 2N<sub>2</sub>O → 2N<sub>2</sub> + O<sub>2</sub> C) N<sub>2</sub>O → N<sub>2</sub> + 2O<sub>2</sub> D) N<sub>2</sub>O → N<sub>2</sub> + O<sub>2</sub> E) 2N<sub>2</sub> + O<sub>2 </sub>→ 2N<sub>2</sub>O Write a balanced reaction for which the following rate relationships are true. Rate = = = - A) N<sub>2</sub> + O<sub>2 </sub>→<sub> </sub> <sub> </sub> N<sub>2</sub>O B) 2N<sub>2</sub>O → 2N<sub>2</sub> + O<sub>2</sub> C) N<sub>2</sub>O → N<sub>2</sub> + 2O<sub>2</sub> D) N<sub>2</sub>O → N<sub>2</sub> + O<sub>2</sub> E) 2N<sub>2</sub> + O<sub>2 </sub>→ 2N<sub>2</sub>O = Write a balanced reaction for which the following rate relationships are true. Rate = = = - A) N<sub>2</sub> + O<sub>2 </sub>→<sub> </sub> <sub> </sub> N<sub>2</sub>O B) 2N<sub>2</sub>O → 2N<sub>2</sub> + O<sub>2</sub> C) N<sub>2</sub>O → N<sub>2</sub> + 2O<sub>2</sub> D) N<sub>2</sub>O → N<sub>2</sub> + O<sub>2</sub> E) 2N<sub>2</sub> + O<sub>2 </sub>→ 2N<sub>2</sub>O = - Write a balanced reaction for which the following rate relationships are true. Rate = = = - A) N<sub>2</sub> + O<sub>2 </sub>→<sub> </sub> <sub> </sub> N<sub>2</sub>O B) 2N<sub>2</sub>O → 2N<sub>2</sub> + O<sub>2</sub> C) N<sub>2</sub>O → N<sub>2</sub> + 2O<sub>2</sub> D) N<sub>2</sub>O → N<sub>2</sub> + O<sub>2</sub> E) 2N<sub>2</sub> + O<sub>2 </sub>→ 2N<sub>2</sub>O Write a balanced reaction for which the following rate relationships are true. Rate = = = - A) N<sub>2</sub> + O<sub>2 </sub>→<sub> </sub> <sub> </sub> N<sub>2</sub>O B) 2N<sub>2</sub>O → 2N<sub>2</sub> + O<sub>2</sub> C) N<sub>2</sub>O → N<sub>2</sub> + 2O<sub>2</sub> D) N<sub>2</sub>O → N<sub>2</sub> + O<sub>2</sub> E) 2N<sub>2</sub> + O<sub>2 </sub>→ 2N<sub>2</sub>O


A) Write a balanced reaction for which the following rate relationships are true. Rate = = = - A) N<sub>2</sub> + O<sub>2 </sub>→<sub> </sub> <sub> </sub> N<sub>2</sub>O B) 2N<sub>2</sub>O → 2N<sub>2</sub> + O<sub>2</sub> C) N<sub>2</sub>O → N<sub>2</sub> + 2O<sub>2</sub> D) N<sub>2</sub>O → N<sub>2</sub> + O<sub>2</sub> E) 2N<sub>2</sub> + O<sub>2 </sub>→ 2N<sub>2</sub>O N2 + O2 →
Write a balanced reaction for which the following rate relationships are true. Rate = = = - A) N<sub>2</sub> + O<sub>2 </sub>→<sub> </sub> <sub> </sub> N<sub>2</sub>O B) 2N<sub>2</sub>O → 2N<sub>2</sub> + O<sub>2</sub> C) N<sub>2</sub>O → N<sub>2</sub> + 2O<sub>2</sub> D) N<sub>2</sub>O → N<sub>2</sub> + O<sub>2</sub> E) 2N<sub>2</sub> + O<sub>2 </sub>→ 2N<sub>2</sub>O N2O
B) 2N2O → 2N2 + O2
C) N2O → N2 + 2O2
D) Write a balanced reaction for which the following rate relationships are true. Rate = = = - A) N<sub>2</sub> + O<sub>2 </sub>→<sub> </sub> <sub> </sub> N<sub>2</sub>O B) 2N<sub>2</sub>O → 2N<sub>2</sub> + O<sub>2</sub> C) N<sub>2</sub>O → N<sub>2</sub> + 2O<sub>2</sub> D) N<sub>2</sub>O → N<sub>2</sub> + O<sub>2</sub> E) 2N<sub>2</sub> + O<sub>2 </sub>→ 2N<sub>2</sub>O N2O → Write a balanced reaction for which the following rate relationships are true. Rate = = = - A) N<sub>2</sub> + O<sub>2 </sub>→<sub> </sub> <sub> </sub> N<sub>2</sub>O B) 2N<sub>2</sub>O → 2N<sub>2</sub> + O<sub>2</sub> C) N<sub>2</sub>O → N<sub>2</sub> + 2O<sub>2</sub> D) N<sub>2</sub>O → N<sub>2</sub> + O<sub>2</sub> E) 2N<sub>2</sub> + O<sub>2 </sub>→ 2N<sub>2</sub>O N2 + O2
E) 2N2 + O2 → 2N2O

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The elementary reaction 2NO2(g) → 2NO(g) + O2(g) Is second order in NO2 and the rate constant at 501 K is 7.93 × 10-3 L mol-1 s-1. The reaction half-life at this temperature when [NO2]0 = 0.45 mol L-1 is ________ s.


A) 3.6 × 10-3
B) 0.011
C) 126
D) 87
E) 280

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A reaction with an activation energy of 65.4 kJ mol-1 has a rate constant of 1.15 s-1 at 354 K. At what temperature will the rate constant be double?


A) 365 K
B) 708 K
C) 181 K
D) 340 K
E) 378 K

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Define half-life.

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A half-life of a reaction is t...

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In aqueous solution, hypobromite ion, BrO-, reacts to produce bromate ion, BrO3-, and bromide ion, Br-, according to the following chemical equation: 3BrO-(aq) → BrO3-(aq) + 2BR-(aq) A plot of 1/[BrO-] vs. time is linear and the slope is equal to 0.056 L mol-1 s-1. If the initial concentration of BrO- is 0.80 mol L-1, how long will it take one-half of the BrO- ion to react?


A) 4.5 × 10-2 s
B) 7.1 s
C) 12 s
D) 22 s

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Given the following balanced equation, determine the rate of reaction with respect to [NH3]. N2(g) + 3H2(g) → 2NH3(g)


A) Rate = + Given the following balanced equation, determine the rate of reaction with respect to [NH<sub>3</sub>]. N<sub>2</sub>(g) + 3H<sub>2</sub>(g) → 2NH<sub>3</sub>(g) A) Rate = + B) Rate = - C) Rate = + D) Rate = - E) It is not possible to determine the answer without more information.
B) Rate = - Given the following balanced equation, determine the rate of reaction with respect to [NH<sub>3</sub>]. N<sub>2</sub>(g) + 3H<sub>2</sub>(g) → 2NH<sub>3</sub>(g) A) Rate = + B) Rate = - C) Rate = + D) Rate = - E) It is not possible to determine the answer without more information.
C) Rate = + Given the following balanced equation, determine the rate of reaction with respect to [NH<sub>3</sub>]. N<sub>2</sub>(g) + 3H<sub>2</sub>(g) → 2NH<sub>3</sub>(g) A) Rate = + B) Rate = - C) Rate = + D) Rate = - E) It is not possible to determine the answer without more information. Given the following balanced equation, determine the rate of reaction with respect to [NH<sub>3</sub>]. N<sub>2</sub>(g) + 3H<sub>2</sub>(g) → 2NH<sub>3</sub>(g) A) Rate = + B) Rate = - C) Rate = + D) Rate = - E) It is not possible to determine the answer without more information.
D) Rate = - Given the following balanced equation, determine the rate of reaction with respect to [NH<sub>3</sub>]. N<sub>2</sub>(g) + 3H<sub>2</sub>(g) → 2NH<sub>3</sub>(g) A) Rate = + B) Rate = - C) Rate = + D) Rate = - E) It is not possible to determine the answer without more information. Given the following balanced equation, determine the rate of reaction with respect to [NH<sub>3</sub>]. N<sub>2</sub>(g) + 3H<sub>2</sub>(g) → 2NH<sub>3</sub>(g) A) Rate = + B) Rate = - C) Rate = + D) Rate = - E) It is not possible to determine the answer without more information.
E) It is not possible to determine the answer without more information.

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The rate of disappearance of HBr in the gas phase reaction 2HBr(g) → H2 (g) + Br2 (g) Is 0.130 mol L-1 s-1 at 150 °C. The rate of reaction is ________ mol L-1 s-1.


A) 3.85
B) 0.0650
C) 0.0169
D) 0.260
E) 0.0860

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The rate constant for a first-order reaction is 0.54 L mol-1 s-1. What is the half-life of this reaction if the initial concentration is 0.27 mol L-1?


A) 2.0 s
B) 5.0 s
C) 0.25 s
D) 6.9 s
E) 1.3 s

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The rate constant for a zero-order reaction is 0.54 L mol-1 s-1. What is the half-life of this reaction if the initial concentration is 0.27 mol L-1?


A) 2.0 s
B) 5.0 s
C) 0.25 s
D) 6.9 s
E) 1.3 s

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The first-order reaction, SO2Cl2 → SO2 + Cl2, has a half-life of 8.75 hours at 593 K. How long will it take for the concentration of SO2Cl2 to fall to 16.5% of its initial value?


A) 0.143 hr
B) 2.28 hr
C) 6.99 hr
D) 22.7 hr

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