The reaction A $\rarr$ Products is a zero-order reaction with a rate constant of 2.56 × 10^-³ M s^-¹. If the concentration of A is 75.6 M after 12.7 minutes, what was the initial concentration of A?

Question

Quizplus · Accepted Answer

For a zero-order reaction, [A] = [A]₀ - kt. Rearranging gives [A]₀ = [A] + kt. Substituting [A] = 75.6 M, k = 2.56 × 10⁻³ M s⁻¹, and t = 12.7 min (762 s), we find [A]₀ = 75.6 M + (2.56 × 10⁻³ M s⁻¹ × 762 s) = 77.6 M.

The Reaction A →\rarr→ Products Is a Zero-Order Reaction with a Rate Constant of a Rate

The Reaction A $\rarr$ Products Is a Zero-Order Reaction with a Rate Constant of a Rate