The reaction `2NO+O_(2)rarr2NO_(2)` follows the rate law `=k[NO]^(2)[O_(2)]`. What is the order of the reaction? If `k=2.0xx10^(-6) "mol"^(-2) L^(2)s^(-1)`. What is the rate of the reaction when `=[NO]=0.04 "mol"L^(-1) and [O_(2)]=0.2"mol" L^(-1)` ?

The rate of a reaction is 1.2xx10^-3 L mol^-1 s^-1 . What is the order of the reaction?

The rate of a reaction is 1.2xx10^-3 L mol^-1s^-1 , What is the order of the reaction?

The rate of a reaction is 1.209 xx10^-4L^2 mol^-2 s^-1 . The order of the reaction is :

For the following reaction: 2A + B +C rarr A_(2)B + C The rate law has been determined to be Rate = k[A][B]^(2) with k = 2.0 xx 10^(-6) mol^(-2) L^(2) s^(-1) For this reaction, determine the initial rate of the reaction with [A] = 0.1 mol L^(-1), [B] = 0.2 mol L^(-1), C = 0.8 mo, L^(-1) . Determine the rate after 0.04 mol L^(-1) of A has reacted.

For the reaction 2A+B +C rarr A_(2)B+C the rate law has been found to be Rate = k[A] [B]^(2) with k = 2.0xx10^(-6) mol^(-2) L^(2)s^(-1) . The initial rate of reaction with [A] =0.1 mol L^(-1) [B] = 0.2 mol L^(-1) and [C] = 0.8 mol L^(-1) s^(-1)

The rate constant of a reaction is 2.5xx10^(-2)" L mol"^(-1)s^(-1) . Calculate the initial rate with concentration 0.2" mol L"^(-1) .

The rate equation for the reaction 2A + B rarr products is rate = k[A][B]^(2) . If k at T (K) is 5.0 xx 10^(-6) mol^(-2) L^(2)s^(-1) , the initial rate of the reaction, when [A] = 0.05 mol L^(-1) and [B] = 0.1 mol L^(-1) is