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Exam 13: Chemical Kinetics

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Question 81

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At an elevated temperature the decomposition of a gaseous oxide,AO₂ occurs with a rate constant,k = 0.54 M^-1s^-1.If the half-life of this reaction is 926 seconds when [AO₂] = 2.0 × 10^-3 M and 462 seconds when [AO₂] = 4.0 × 10^-3 M,this reaction is ________ order.

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Question 82

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The relative initial rates of the reaction A₂ + B₂ → products in vessels (a) -(d) are 1:1:4:4.Unshaded spheres represent A₂ molecules,and shaded spheres represent B₂ molecules present at the beginning of the reaction. -What is the rate law for this reaction?

A) Rate = k[A₂]²
B) Rate = k[B₂]²
C) Rate = k[A₂][B₂]
D) Rate = k[A₂]²[B₂]²

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Question 83

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The hydrolysis of tert-butyl chloride is given in the reaction below: (CH₃) ₃CCl(aq) + H₂O(l) → (CH₃) ₃COH(aq) + H⁺(aq) + Cl^-(aq) If the rate law is: Rate = k[(CH₃) ₃CCl],what is the order of the reaction with respect to water?

The rate constant,k,for a first-order reaction is equal to 4.2 × 10^-4 s^-1.What is the half-life for the reaction?

The second-order reaction,2 Mn(CO) ₅ → Mn₂(CO) ₁₀ has a rate constant equal to 3.0 × 10⁹ M^-1s^-1 at 25°C.If the initial concentration of Mn(CO) ₅ is 1.0 × 10^-5 M,how long will it take for 90.% of the reactant to disappear?

The following set of data was obtained by the method of initial rates for the reaction: BrO₃^-(aq) + 5 Br^-(aq) + 6 H⁺(aq) → 3 Br₂(aq) + 3 H₂O(l) . Calculate the initial rate when BrO₃^- is 0.30 M,Br^- is 0.050 M,and H⁺ is 0.15 M.

What is the rate law for the elementary reaction shown below? 2 HI → H₂ + I₂

The aquation of tris(1,10-phenanthroline) iron(II) in acid solution takes place according to the equation: Fe(phen) ₃²⁺ + 3 H₃O⁺ + 3 H₂O → Fe(H₂O) ₆²⁺ + 3 phenH⁺ If the activation energy,E_a,is 126 kJ/mol and the rate constant at 30°C is 9.8 × 10^-3 min^-1,what is the frequency factor,A?

When the temperature of a gas whose activation energy is 55 kJ/mol is increased from 300 K to 320 K,the fraction of collisions with sufficient energy to react

Nitrogen dioxide decomposes at 300°C via a second-order process to produce nitrogen monoxide and oxygen according to the following chemical equation. 2 NO₂(g) → 2 NO(g) + O₂(g) . A sample of NO₂(g) is initially placed in a 2.50-L reaction vessel at 300°C.If the half-life and the rate constant at 300°C are 11 seconds and 0.54 M^-1 s^-1,respectively,how many moles of NO₂ were in the original sample?

According to kinetic molecular theory,which of the following will decrease the rate of reaction?

The reaction shown below has the rate law: Rate = k[BrO₃^-][Br^-][H⁺]².The order of reaction with respect to H⁺ is ________ and the overall order is ________. BrO₃^-(aq)+ 5 Br^-(aq)+ 6 H⁺(aq)→ 3 Br₂(aq)+ 3 H₂O(l)

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 2.00 hours?

Molecular hydrogen can be made from methane gas by the reaction below.How is the rate of disappearance of CH₄ related to the rate of appearance of H₂? - = ? CH₄ (g) + H₂O (l) → CO (g) + 3H₂ (g)

Which of the following does not affect the rate of a bimolecular reaction?

The reaction between chlorine and nitric oxide to form nitrosyl chloride is shown below.If the reaction rate doubles when the concentration of Cl₂ is doubled and the rate quadruples when the concentration of NO is doubled,by what factor will the rate increase if both concentrations,NO and Cl₂,are doubled? Cl₂(g) + 2 NO(g) → 2 NOCl(g)

Biological reactions are catalyzed by

-Which of the elementary reactions shown above has a molecularity of three?

The following reaction is first order,C₂H₆ → 2 CH₃.If the rate constant is equal to 5.5 × 10^-4 s^-1 at 1000 K,how long will it take for 0.35 mol of C₂H₆ in a 1.00 L container to decrease to 0.25 mol in the same container?

The half life of the reaction shown below is found not to depend on the concentration of H₂O₂(aq) . 2 H₂O₂(aq) → 2 H₂O(l) + O₂(g) What is the order of this reaction?