The gas-phase reaction of hydrogen and iodine monochloride...

The gas-phase reaction of hydrogen and iodine monochloride is first order in $\mathrm{H}_{2}$ and first order in ICl. What is the rate law, and what are the units of the rate constant?
$$\mathrm{H}_{2}(g)+2 \mathrm{ICl}(g) \longrightarrow 2 \mathrm{HCl}(g)+\mathrm{I}_{2}(g)$$

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Key Concepts

Rate Law

The rate law in chemical kinetics describes how the rate of a reaction depends on the concentration of its reactants. For a reaction that is first order with respect to hydrogen (H2) and first order with respect to iodine monochloride (ICl), the rate law is written as rate = k[H2][ICl]. This means that the reaction rate is directly proportional to the concentration of each reactant.

Reaction Order

The reaction order is determined by the sum of the individual orders with respect to each reactant. In this case, since the reaction is first order in H2 and first order in ICl, the overall reaction order is 2. The overall order indicates the degree of dependence of the reaction rate on the concentrations of the reactants.

Rate Constant and Its Units

The rate constant, k, is a key factor in the rate law that captures the influence of temperature and other conditions on the reaction. For a second-order reaction, the units of the rate constant are typically expressed as L mol?¹ s?¹ (or equivalently M?¹ s?¹), ensuring that when multiplied by the concentrations (in mol L?¹), the rate is given in the appropriate units of mol L?¹ s?¹.

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