Question

The rate constant for the reaction at 28°C is 3.5 x 10^⁻² M⁻¹ s⁻¹. What is the rate of the reaction at a time when [H₂S] = 0.00016 M and [Cl₂] = 0.070 M?

Answer 1

The rate of the reaction at a given time, with a rate constant of 3.5 x 10⁻² M⁻¹ s⁻¹, [H₂S] = 0.00016 M, and [Cl₂] = 0.070 M, is 3.92 x 10⁻¶ M s⁻¹.

Step-by-step explanation:

The rate of the reaction can be determined by applying the provided rate constant and the concentrations of the reactants in the rate law equation. Given that the rate constant k for the reaction at 28°C is 3.5 x 10⁻² M⁻¹ s⁻¹, and the concentrations of H₂S and Cl₂ at a certain time are 0.00016 M and 0.070 M respectively, the rate of the reaction can be calculated using the rate law.

Assuming the reaction between H₂S and Cl₂ is of the form rate = k[H₂S][Cl₂], we plug in the values:

rate = (3.5 x 10⁻² M⁻¹ s⁻¹)(0.00016 M)(0.070 M) = 3.92 x 10⁻¶ M s⁻¹

Therefore, the rate of the reaction at the given concentrations is 3.92 x 10⁻¶ M s⁻¹.