Question

The reaction A ---- B+C is known to be zero order in A with a rate constant of -C , / 5.0 x 10⁻² mol/L s at 25 C. An experiment was run at 25 C where Ao 1.0 x 10⁻³ write the integrated rate law.

Answer 1

The integrated rate law for the given reaction is [A]t = 1.0 x 10⁻³ + Ct/5.0 x 10⁻².

Step-by-step explanation:

The integrated rate law for a zero-order reaction is given by [A]t = [A]o - kt, where [A]t is the concentration of reactant A at time t, [A]o is the initial concentration of A, k is the rate constant, and t is the time.

In this case, the reaction A ---- B+C is known to be zero order in A with a rate constant of -C/5.0 x 10⁻² mol/L s at 25°C. Given Ao = 1.0 x 10⁻³ M, we can substitute the values into the integrated rate law to get [A]t = 1.0 x 10⁻³ - (-C/5.0 x 10⁻²)t.

Therefore, the integrated rate law for this reaction is [A]t = 1.0 x 10⁻³ + Ct/5.0 x 10⁻².