Which of the following statements is true regarding reaction rate constants? Rate constants are the same for all reactions. Rate constants are temperature dependent. Rate constants are independent of temperature. Rate constants depend on the concentration of reactants.

Rate constants are temperature dependent.

Which of the following reactions would you predict to have the smallest orientation factor? \[ ext{H}_2 + ext{I}_2 ightarrow 2 ext{HI} \] \[ ext{N}_2 + 3 ext{H}_2 ightarrow 2 ext{NH}_3 \] \[ ext{C}_2 ext{H}_4 + ext{H}_2 ightarrow ext{C}_2 ext{H}_6 \] \[ ext{NOCl}_2 + ext{NO} ightarrow 2 ext{NOCl} \]

\[ ext{NOCl}_2 + ext{NO} ightarrow 2 ext{NOCl} \]

Which of the following statements is false about the half-life of a first-order reaction? The half-life remains constant throughout the reaction. The half-life is independent of the initial concentration. The half-life can be calculated using the rate constant. The half-life is dependent on the initial concentration.

The half-life is dependent on the initial concentration.

What are the characteristics of a second-order reaction with only one reactant? The rate is proportional to the reactant concentration. The rate is proportional to the square of the reactant concentration. The rate is proportional to the inverse of the reactant concentration. The rate is independent of the reactant concentration.

The rate is proportional to the square of the reactant concentration.

Identify the methods used to monitor a reaction as it occurs in the reaction flask. Spectroscopy, chromatography, and titration. Only spectroscopy. Only titration. Only chromatography.

Spectroscopy, chromatography, and titration.

Given the rate law \[ ext{Rate} = k [x][y] \], how does the rate of reaction change if the concentration of y is doubled? The rate of reaction increases by a factor of four. The rate of reaction remains unchanged. The rate of reaction decreases by half. The rate of reaction increases by a factor of two.

The rate of reaction increases by a factor of two.

For a reaction that follows the rate law \[ ext{Rate} = k[A][B]^2 \], what happens to the rate if the concentration of B is increased by a factor of 3? The rate increases by a factor of 3.00. The rate remains unchanged. The rate decreases by a factor of 3.00. The rate increases by a factor of 9.00.

The rate increases by a factor of 9.00.

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