Question

Label each statement as true or false. Correct any false statement to make it true.

a. Increasing temperature increases reaction rate.

b. If a reaction is fast, it has a large rate constant.

c. A fast reaction has a large negative $\mathbf{∆}\mathbf{G}\mathbf{°}$value.

d. When ${\mathbf{E}}_{\mathbf{a}}$is large, the rate constant k is also large.

e. Fast reactions have equilibrium constants > 1.

f. Increasing the concentration of a reactant always increases the rate of a reaction.

Short answer

Answer

a. True

b. True

c. False. The correct statement is “there would be no relation between the value or sign of the $∆\mathrm{G}°$and fast or slow reaction.

d. False. The correct statement is “activation energy is inversely proportional to the rate constant.

e. False. The correct statement is “equilibrium constant is independent of slow or fast of the reaction.

f. False. The correct statement is “the reactants that appear in the rate equation can affect the rate of the reaction.

Step-by-step solution

Step-by-Step SolutionStep 1: Rate of reaction

There are many factors on which the rate of the reaction depends, such as;

• Changing the temperature of the reaction
• Changing the concentration of reactant or product
• Activation energy

Explanation for a, b, and c

a. On increasing the temperature of the reaction, the kinetic energy of the molecules will increase. Due to this, the rate of the reaction would be increased.

Thus, the given statement is true.

b. It is given that the reaction is fast which means the formation of the product is fast or the reaction is towards the forward direction. Due to this, the rate constant has a large value.

Thus, the given statement is true.

c. The sign of $∆\mathrm{G}°$is independent of fast or slow reaction. It depicts the spontaneity or non-spontaneity of the reaction.

Thus, the given statement is false. The correct statement is “there would be no relation between the value or sign of the $∆\mathrm{G}°$and fast or slow reaction.

Explanation for d, e, and f

d. There is an inverse relationship between the activation energy and the rate constant of the reaction. If the value of activation energy is large then the value of the rate constant would be small.

Thus, the given statement is false. The correct statement is “activation energy is inversely proportional to the rate constant.

e. Equilibrium constant depends on temperature and it does not depend upon the fast or slow reaction.

Thus, the given statement is false. The correct statement is “equilibrium constant is independent of slow or fast of the reaction.

f. The liquid or solid reactants does not involve in the expression of the equilibrium constant. In other words, they would not affect the rate of the reaction.

In the given statement, it is not mentioned about the state of the reactant. Thus, the given statement is false. The correct statement is “the reactants that appear in the rate equation can affect the rate of the reaction.