According to the reaction 2 NO(g) → N₂(g) + O₂(g) , nitrogen monoxide (NO) decomposes at 400 °C. Three graphs were created when the concentration of NO was tracked throughout time:

What is the rate law for the reaction?

Consider the generic zero-order reaction: R → P
Which of the following quantities, when plotted against time, will give a straight line?

For the hypothetical second-order reaction, X → Y, which of these graphs is valid?

What are the order of the reaction and the rate constant for the reaction based on the gathered data at 250 °C?

SCN^- → NCS^-

Time [SCN^-]

0       1.00

5      0.861

10     0.741

15     0.638

20     0.549

25     0.472

At an initial concentration of 0.53 M, the half-life for the second-order decomposition of NO₂ is 30.4 s. Determine the rate constant.

For the reaction A → B, the concentration of A is observed over time and tabulated below.

Determine the rate order and calculate the rate constant. Determine the rate when [A] = 0.04 M.

The first-order rate constant for the decomposition of the hypothetical compound A₂B₅, 2 A₂B₅(g) → 4 AB₂(g) + B₂(g), at 70 °C is 2.34 × 10^-3 s^-1. Suppose we start with 0.01250 mol of A₂B₅(g) in a volume of 1.5 L. How many moles of A₂B₅ will remain after 3.0 min?