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Exam 13: Chemical Kinetics

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Question 91

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A catalyst increases the rate of a reaction by providing a different reaction pathway that

A) lowers only the activation energy.
B) raises only the energy of the products.
C) lowers only the energy of the reactants and products.
D) All of these are affected by the presence of a catalyst.

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Question 92

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The isomerization reaction,CH₃NC → CH₃CN,is first order and the rate constant is equal to 0.46 s^-1 at 600 K.What is the concentration of CH₃NC after 0.20 minutes if the initial concentration is 0.10 M?

A) 4.0 × 10^-4 M
B) 9.1 × 10^-4 M
C) 4.0 × 10^-2 M
D) 9.1 × 10^-2 M

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Question 93

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Which general rate law below corresponds to an elementary bimolecular reaction?

If the units for rate are M s^-1,what are the units for the rate constant,k,if the overall order of the reaction is five?

A reaction has the rate law Rate = k[NO]²[H₂].If the concentration of NO is reduced by half and the concentration of H₂ is quadrupled,the rate of reaction will ________ (increase,decrease,not change).

The rate-determining step in a reaction is shown below.The molecularity of this reaction is ________. NO₂(g)+ NO₂(g)→ NO(g)+ NO₃(g)

A three-step mechanism has been suggested for the formation of carbonyl chloride: Step 1: Cl₂→ 2 Cl (fast,equilibrium) Step 2: Cl + CO → COCl (fast,equilibrium) Step 3: COCl + Cl₂ → COCl₂ + Cl (slow) What is the molecularity of the rate-determining step?

A reaction has the rate law Rate = k[NO]²[H₂].If the concentration of NO is reduced by 1/3,the rate of reaction will be ________ (increased,decreased)by ________.

The data below were collected for the following reaction: 2 NO₂ (g) + F₂ (g) 2 NO₂F (g) What is the expression for the rate law of the reaction?

What fraction of collisions will have sufficient energy to react for a gas whose activation energy is 68 kJ/mol at 25°C?

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 is 126 kJ/mol and frequency factor is 8.62 × 10¹⁷ s^-1,at what temperature is the rate constant equal to 3.63 × 10^-3 s^-1 for the first-order reaction?

The first-order isomerization reaction: cyclopropane → propene,has a rate constant of 1.10 × 10^-4 s ^-1 at 470°C and an activation energy of 264 kJ/mol.What is the temperature of the reaction when the rate constant is equal to 4.36 × 10^-3 s^-1?

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 44 seconds and 0.54 M^-1 s^-1,respectively,how many moles of NO₂ were in the original sample?

When the concentration of A is doubled,the rate for the reaction: 2 A + B → 2 C quadruples. When the concentration of B is doubled the rate remains the same.Which mechanism below is consistent with the experimental observations?

The fraction of collisions with sufficient energy to react is equal to

For the first-order reaction,2 N₂O(g) → 2 N₂(g) + O₂(g) ,what is the concentration of N₂O after 3 half-lives if 0.15 mol of N₂O is initially placed into in a 1.00-L reaction vessel?

Hydrogen iodide decomposes at 800 K via a second-order process to produce hydrogen and iodine according to the following chemical equation. 2 HI(g) → H₂(g) + I₂(g) At 800 K it takes 142 seconds for the initial concentration of HI to decrease from 6.75 × 10^-2 M to 3.50 × 10^-2 M.What is the rate constant for the reaction at this temperature?

The following reaction is first order in A and first order in B: A + B → Products Rate = k[A][B] What is the initial rate of this reaction in vessel (b) relative to the initial rate of this reaction in vessel (a) ? Each vessel has the same volume.Shaded spheres represent A molecules,and unshaded spheres represent B molecules present at the beginning of the reaction.

A reaction with an activation energy,E_a = 51.2 kJ/mol will proceed ________ times faster when the temperature is raised from 20 °C to 30 °C.

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 0.10 mol in the same container?