The reaction SO2 Cl2(g) ⟶SO2(g)+Cl2(g) is first order in SO2 Cl2 . Using the following kinetic d

step 1 If the chemical reaction provided, namely S .O2, CL2, going to S .O .2 plus CL2 is first order,

The reaction SO2 Cl2(g) ⟶SO2(g)+Cl2(g) is first order in SO2...

The reaction $\mathrm{SO}_{2} \mathrm{Cl}_{2}(g) \longrightarrow \mathrm{SO}_{2}(g)+\mathrm{Cl}_{2}(g)$ is first order in $\mathrm{SO}_{2} \mathrm{Cl}_{2} .$ Using the following kinetic data, determine the magnitude and units of the first-order rate constant:

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Key Concepts

First-Order Reaction Kinetics

In a first?order reaction, the rate is directly proportional to the concentration of a single reactant. This means that as the reactant concentration decreases, the rate decreases proportionally. The first-order rate law is expressed as d[A]/dt = -k[A], where k is the first-order rate constant.

Integrated Rate Law for First-Order Reactions

The integrated rate law for a first-order reaction relates the concentration of the reactant at any time to its initial concentration and the rate constant. It is given by ln[A] = ln[A]? - kt. This equation allows one to determine the rate constant from experimental data by plotting ln[A] versus time, where the slope of the line is equal to -k.

Rate Constant and Its Units

The rate constant in a kinetic reaction determines the speed at which the reaction proceeds under given conditions. For a first-order reaction, the units of the rate constant are reciprocal time (e.g., s?¹ or min?¹) because the rate of change of concentration is directly proportional to the concentration itself.

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