Question

CH₃Cl(g) + 3Cl₂(g) → CCl₄(g) + 3HCl(g)

[CH₃Cl](M) [Cl₂](M) Initial Rate (M/s)
0.050 0.050 0.014
0.100 0.050 0.029
0.100 0.100 0.041
0.200 0.200 0.115

Write an expression for the reaction rate law.

Answer 1

The question asks to determine the reaction rate law and rate constant for the given reactions, indicating a first-order reaction with respect to ethyl chloride and requires a two-step reaction mechanism for an ICl and H2 reaction.

Step-by-step explanation:

The subject of this question involves determining the reaction rate law and the rate constant (k) for the chemical reactions provided. Specifically, for the reaction CH3CH2Cl(g) → HCl(g) + C2H2(g), the experimental data suggests a first-order reaction with respect to ethyl chloride concentration, leading to the rate law: rate = k[CH3CH2Cl]. This conclusion was drawn from a comparison of the initial rates and concentrations of each reactant, showing that the rate changes in direct proportion to changes in the ethyl chloride concentration.

For the reaction 2 ICl(g) + H2(g) → 2 HCl(g) + I2 (s), a two-step mechanism that correlates with the experimentally determined rate law rate = k[ICl][H2], using HI as an intermediate, is requested. The details of the reaction mechanism would involve bimolecular elementary reactions that support the given rate law.