Question

Consider the following data for the given reaction
 \(2\)\(\text{HI}_{(g)}\) \(\rightarrow\) \(\text{H}_2{(g)}\)$ + $\(\text{I}_2{(g)}\)

The order of the reaction is __________.

Answer 1

Correct Answer: 2

Assuming the rate law:

$$\text{Rate} = k[\text{HI}]^n$$

Using any two of the given data points:

$$\frac{3.0 \times 10^{-3}}{7.5 \times 10^{-4}} = \left(\frac{0.01}{0.005}\right)^n$$

Solving, we find \( n = 2 \), so the reaction is second order.