If the decomposition of reactant A follows first-order kinetics, what concentration of A remains if:
[A]₀ = 0.273 M, k = 1.53 × 10^{− 2} minutes^{− 1}, and the elapsed time = 1.61 hr?

Question

If the decomposition of reactant A follows first-order kinetics, what concentration of A remains if: [A]₀ = 0.273 M, k = 1.53 × 10^{− 2} minutes^{− 1}, and the elapsed time = 1.61 hr?

Quizplus · Accepted Answer

The concentration of A can be calculated using the first-order kinetics formula: [A] = [A]₀ * e^(-kt). Converting time to minutes (1.61 hr = 96.6 min) and substituting the values, [A] = 0.273 * e^(-1.53 × 10^(-2) * 96.6) ≈ 0.109 M.

If the Decomposition of Reactant a Follows First-Order Kinetics, What