For the following first-order reaction: 

X → Y + Z

What information is needed and how will it be used to calculate the reaction's activation energy?

Step 1: Measure the change in concentration of X vs time at different temperatures.
Step 2: Plot 1/[X] vs t for each temperature. From each linear graph, calculate the rate constant at each temperature using k = (slope).
Step 3: Plot ln k vs. 1/T then using the graph calculate the activation energy using E_a = –(slope)R.

Step 1: Measure the change in concentration of X vs time at different temperatures.
Step 2: Plot 1/[X] vs t for each temperature. From each linear graph, calculate the rate constant at each temperature using k = (slope).
Step 3: Plot ln k vs. T then using the graph calculate the activation energy using E_a = (slope)R.

Step 1: Measure the change in concentration of X vs time at different temperatures.
Step 2: Plot ln [X] vs t for each temperature. From each linear graph, calculate the rate constant at each temperature using k = (slope).
Step 3: Plot ln k vs. 1/T then using the graph calculate the activation energy using E_a = –(slope)R.

Step 1: Measure the change in concentration of X vs time at different temperatures.
Step 2: Plot ln [X] vs t for each temperature. From each linear graph, calculate the rate constant at each temperature using k = –(slope).
Step 3: Plot ln k vs. 1/T then using the graph calculate the activation energy using E_a = –(slope)R.

Step 1: Measure the change in concentration of X vs time at different temperatures.
Step 2: Plot ln [X] vs t for each temperature. From each linear graph, calculate the rate constant at each temperature using k = (slope).
Step 3: Plot ln k vs. T then using the graph calculate the activation energy using E_a = (slope)R.