A certain reaction A $\rarr$ products is second order with respect to A with a rate constant, k, 0.122 M^-1min^-1. Starting with [A]_o = 1.01M, how many seconds will it take for A to reach a concentration of 0.750M

Question

Quizplus · Accepted Answer

The rate law for the reaction is given as:

rate = k[A]^2

We can use the integrated rate law for a second-order reaction to solve for the time required to reach a particular concentration:

1/[A] - 1/[A]₀ = kt

where [A]₀ is the initial concentration, [A] is the concentration at time t, and k is the rate constant. Rearranging,

t = 1/(k[A]₀) × (1/[A] - 1/[A]₀)

Substituting the given values gives:

t = 1/(0.122 M⁻¹ min⁻¹ × 1.01 M) × (1/0.750 M - 1/1.01 M)

t = 168.8 s ≈ 169 s

Therefore, the answer is D) 169 s.

A Certain Reaction A →\rarr→ Products Is Second Order with Respect to a with a Respect

A Certain Reaction A $\rarr$ Products Is Second Order with Respect to a with a Respect