The reaction is known to be zero order in A with a rate constant of 5.0 $\times$10^-² mol/L s at 25°C.An experiment was run at 25°C where [A]₀ = 2.0 $\times$ 10^-³ M.After 5.0 minutes,the rate is

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The reaction is zero order in A, so the rate is independent of the concentration of A. Therefore, the rate constant remains the same throughout the experiment. The rate can be calculated using the formula Rate = k[A]^0 = k. Substituting the given values, we get Rate = 5.0 × 10^-10 mol/L s. After 5.0 minutes, the reaction has proceeded for 5.0/60 = 0.0833 hours. Therefore, the amount of reactant remaining is [A] = [A]0 - kt = 2.0 × 10^-10 - (5.0 × 10^-10)(0.0833) = 1.6 × 10^-10 mol/L. The rate at this point is still 5.0 × 10^-10 mol/L s, which is the answer (A).

The Reaction Is Known to Be Zero Order in a with a Rate