Write the rate law for the following elementary reaction:CH2CH2(g) + Cl2(g) → CH2CH2Cl+(g) + Cl−(g)Use k1 to stand for the rate constant.
Question
Write the rate law for the following elementary reaction:CH2CH2(g) + Cl2(g) → CH2CH2Cl+(g) + Cl−(g)Use k1 to stand for the rate constant.
Solution
The rate law for an elementary reaction can be written directly from the stoichiometry of the reaction. In this case, the reaction is:
CH2CH2(g) + Cl2(g) → CH2CH2Cl+(g) + Cl−(g)
The rate law for this reaction would be:
Rate = k1[CH2CH2][Cl2]
Here, k1 is the rate constant, [CH2CH2] is the concentration of CH2CH2, and [Cl2] is the concentration of Cl2. The rate of the reaction is directly proportional to the product of the concentrations of the reactants, each raised to the power of its stoichiometric coefficient in the balanced chemical equation. Since the coefficients of both reactants are 1 in this case, the rate law is as written above.
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