Given the reaction 2A + B--> C+D, and it is found that the reaction is 2nd order in A and independent of B, can the reaction occur in a single step?

Explain the difference between homogeneous catalysis and heterogeneous catalysis?

The reaction A+2B ——> products was found to be first order to A and second order to B. While holding the concentration of A constant , the concentration of B is increased to 3 times its initial value . By what factor does the rate of reaction increase?

Calculate the half life, ty (in min) for the first order reaction, A - B, if the reaction is 12.2% complete in 17.7 minutes. Report your answer to THREE significant figures.

The reaction A(aq) ---> B(aq) is a first order reaction with respect to A(aq). The concentration of A(aq) is reduced to 35.0% of its initial value in 1.49 minutes. What is the value of the half-life (in s) of the reaction?

A gas phase reaction has a rate coefficient of 1.3·104 L mol–1s–1 at 300 K and its activation energy is 8.3 kJ mol–1. Indicate the order of the reaction.

The recombination reaction2 HO2(g) → H2O2(g) + O2(g)has a second-order rate constant of 2E9 M-1 s-1. Calculate the half-life of the reaction if the initial concentration of HO2(g) is 2.58E-11 M.Note: the coefficient 2 in the reaction means that the integrated rate law for this reaction is:1/ct = 1/c0 + 2kt

The reaction A → B + C is second order with respect to A. When [A]0 = 0.15 M,  the reaction is 25 % complete at 72.1 min. Calculate the half-life for this reaction

At a certain temperature this reaction follows second-order kinetics with a rate constant of 1.0M 2NH, (g) - N, (2) + 3H, (g) Suppose a vessel contains NH, at a concentration of 1.07M. Calculate how long it takes for the concentration of NH, to decrease by 91.%. You may assume no other reaction is important. Round your answer to 2 significant digits.