The rate law for the reaction below is rate = k[N2]*[H2]Y %3D - 2 NH3 N2 + 3 H2 Which of the following is true? OAX = 3 and y = 1 O B. The reaction is 4th order overall OC The order of reaction needs to be determined experimentally OD.X = 1 and y = 1 OEX = 1 and y = 3

4. Consider three hypothetical reactions of the type A → products. One of the reactions is zeroth order, one is first order, and one is second order. If they all have the same numerical value of the rate constant k (in units of M s ¹, s and M¹s¹, -1 -1 9 respectively), what must be the initial concentration [A]o if the half-lives are equal for a) the zeroth- and first-order reactions, b) the zeroth- and second-order reactions, and c) the first- and second-order reactions.

The half-life of a first order reaction is constant and equal to 0.693/k. CA first order reaction with k= 3.465 x 10-2 s-1 is started with [A]o=0.800 M. What is the concentration of A after 60 seconds? Oa. 0.100 M Ob. 0.400 M Oc. c. 0.200 M Od. 0.0800 M

Nitesh

A certain reaction has the following rate law: rate = k[X]³[Y]² Which of the following are the correct units for k? Select one: L³mol-3s-1 Ms-1 M³s O L?mol2s1 L5mol 5s1 Lmol-'s mol³L-3s-1 M's-1 L*mol-4s-1 mol?L-2s1

The decomposition of N»Os(g) to NO2(g) and O2(g) obeys first-order kinetics. Assuming the form of the rate law is: A[N,05] Rate = *[N,Os] At where k = 3.4 x 10-5 s-l at 25°C, what is the initial rate of reaction at 25°C where [N2O5]o = 4.1 x 10-2 M? а. 1.4x 10-6 mol/L's b. 3.4 x 10-5 mol/L's О с. 8.3 х 10-4 mol/L s d. 4.1 x 10-2 mol/L's e. none of these