The following reaction is first order. (CH2)3(g) →CH2=CH-CH3(g) What change in reaction rate wou

step 1 In this question, for the first part, we're going to be looking at the equilibrium where we've g

The following reaction is first order. (CH2)3(g)...

The following reaction is first order.
$$\left(\mathrm{CH}_{2}\right)_{3}(g) \rightarrow \mathrm{CH}_{2}=\mathrm{CH}-\mathrm{CH}_{3}(g)$$
What change in reaction rate would you expect if the pressure of $\left(\mathrm{CH}_{2}\right)_{3}$ doubled?

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Key Concepts

Rate Law

The rate law expresses the mathematical relationship between the reaction rate and the concentrations (or pressures) of the reactants. For first-order reactions, the rate law is given by Rate = k[Reactant], which indicates that any change in the reactant's concentration or pressure results in a proportional change in the reaction rate.

Ideal Gas Relationship

In gaseous reactions, the ideal gas law relates pressure to concentration. Because the concentration of a gas is directly proportional to its pressure under constant temperature and volume, doubling the pressure of a gaseous reactant effectively doubles its concentration, thereby doubling the reaction rate in a first-order process.

First-Order Kinetics

In a first-order reaction, the rate depends linearly on the concentration or partial pressure of one reactant. This means that if the concentration or pressure of the reactant is doubled, the reaction rate will also double, as the rate is directly proportional to it.

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