For an elementary reaction : `2A + B rarr 3C` the rate of appearance of C at time ‘t’ is `1.3 xx 10^(-4) mol l^(-1)s^(-1) `. Calculate at this time : rate of disappearance of A.

For the reaction, N_2+3H_2 rarr 2NH_3 the rate of reaction measured as (Delta [NH_3])/(Delta t) was found to be 2.4 xx 10^-4 mol L^(-1) s^(-1) . Calculate the rate of reaction expressed in terms of (i) N_2 and (ii) H_2 .

For the reaction : 2N_2O_5 rarr 4NO_2+O_2 the rate of reaction measured as (Delta[NO_2])/(Deltat) was found to be 4 xx 10^(-3)" mol L"^(-1) is s^(-1) . Calculate the rate of reaction, expressed in terms of N_2O_5

For the reaction : 2N_2O_5 rarr 4NO_2+O_2 the rate of reaction measured as (Delta [NO_2])/(Delta t) was found to be 1 xx 10^-3 mol L^(-1) s^(-1) . Calculate rate of reaction expressed in terms of N_2O_5 .

For the reaction: 2A + B rarr A2B the rate = k[A][B]^2 with k = 2.0 × 10^(-6) mol^(-2) L^2 s^(-1) . Calculate the initial rate of the reaction when [A] =0.1 mol L^(-1), [B] = 0.2 mol L^(-1) . Calculate the rate of reaction after [A] is reduced to 0.06 mol L^(-1) .

The rate constant of a reaction is 1.2 xx10^(-5) mol^(-2)"litre"^(2)s^(-1) . The order of the reaction is:

Identify the reaction order from each of the following rate constants. k = 2.3 xx 10^(-5) L mol^(-1) s^(-1)