Question

What is the rate constant for the decomposition of 2.00 mol/L of hydrogen peroxide (H2O2) at 25°C, given that the reaction follows first-order kinetics and the rate of decomposition is 0.050 mol/L·s?

Answer 1

For a first-order reaction, the rate law is given by:Rate = k[A]where Rate is the rate of the reaction, k is the rate constant, and [A] is the concentration of the reactant  in this case, hydrogen peroxide .We are given the rate of decomposition  Rate  as 0.050 mol/Ls and the concentration of hydrogen peroxide  [A]  as 2.00 mol/L. We need to find the rate constant  k .Plugging the given values into the rate law equation:0.050 mol/Ls = k 2.00 mol/L Now, we can solve for k:k =  0.050 mol/Ls  /  2.00 mol/L  = 0.025 s^-1 The rate constant for the decomposition of hydrogen peroxide at 25C is 0.025 s^-1 .