Exam 14: Chemical Kinetics

The rate data from a chemical reaction shows that doubling the concentration of A with the concentration of B remaining constant causes the rate to increase by a factor of four. What is the reaction order for [A]?

Substance A decomposes by a first-order reaction. Starting initially with [A] = 2.00 M, after 150 min [A] = 0.50 M. For this reaction what is t1/2?

In the Arrhenius equation, ln k = -Ea/RT + ln A, the symbol A denotes the initial concentration of A.

For the reaction: C₂H₄Br₂ + 3KI → C₂H₄ + 2KBr + KI₃ Initial rate data at 60°C are: The rate law is ________.

For the second order reaction A → products, the following data are obtained: [A] = 3.024 M, t = 0 min [A] = 2.935 M, t = 1.0 min [A] = 2.852 M, t = 2.0 min What is the rate constant, k?

Given the following initial rate data, calculate the specific rate constant.

Given the following initial rate data, write the rate law expression.

For the second-order reaction A → products, the following data are obtained: [A] = 1.512 M, t = 0 min [A] = 1.490 M, t = 1.0 min [A] = 1.469 M, t = 2.0 min What is the initial rate of the reaction in the experiment?

The rate constant for a first-order reaction is k = 0.00073 s-1. Determine the percent of reactant that has decomposed after 500 s.

For the second-order reaction A → products, the following data are obtained: [A] = 3.024 M, t = 0 min [A] = 2.935 M, t = 1.0 min [A] = 2.852 M, t = 2.0 min What is the initial rate of the reaction?

A heterogeneous catalyst is a catalyst that is in two phases of matter.

For the reaction: 2N₂O₅(g) → 4NO₂(g) + O₂(g) the rate law is: = k[N₂O₅] At 300 K, the half-life is 2.50 × 10⁴ seconds and the activation energy is 103.3 kJ/mol. What is the rate constant at 350 K?