for the reaction a+b > products , the rate is first order wrt a and second order wrt to b . if 1 mol each of a and b were introduced into a 1 l vessel and the initial rate were 1x10^-2. calculate the rate when half the reactants have been turned into product Share with your friends Share 10 Sakshi Ganotra answered this Dear student According to the question, the reaction can be written as: A+B →productthe reaction is first order wrt A and second order wrt BInitial number of moles of A = 1 mol and B= 1 molInitial volume = 1LInitial rate is 10-2Thus the rate equation can be written as:Rate = k [a]1[b]2where k is the rate constantSince the initial concentration is 1mol/L for both Aand Bthus k = 10-2 mol-3L3Now when halk the reactants have been converted to the products,a = 0.5 mol, b = 0.5molthus the rate will be:Rate = k[0.5mol/l][0.5molL]2Rate = k/8= 10-28Regards 46 View Full Answer Riddhi answered this the final ans is 1.25 x 10-3 2 Riddhi answered this The moles left of both the compond will be .5moles and because the B is of secound order it will be .00125 7