Question

A reaction's rate constant is measured to be 0.145 1/(M x s). Later on, the same reaction is run again, but this time, the rate constant is measured to be 0.456 1/(M x s). Compare the temperatures at which both measurements were made.

A) The first reaction took place at a higher temperature.

B) The second reaction took place at a higher temperature.

C) Both reactions took place at the same temperature.

D) There is not enough information given to compare the temperatures.

Answer 1

Answer: The second reaction took place at a higher temperature

Step-by-step explanation:

Rate is affected by temperature, as higher temperatures cause the reacting molecules to have more energy.

Collision theory states that in order for a reaction to occur, each reacting molecule must collide with one another in the correct orientation and with enough energy, called the activation energy.

A higher energy caused by a higher temperature will cause the molecules to collide much more frequently, leading to a higher chance of a successful collision, and with more energy to satisfy the activation energy.

Therefore, the second reaction must have taken place at a higher temperature, since the molecules had more energy than the first reaction leading to a higher rate of reaction, and a higher rate constant.