Rate law for the reaction, `A + 2B to C` is found to be
Rate `= k [A] [B]`
Concentration of reactant 'B' is doubled keeping the concentration of 'A' constant, the value of rate constant will be _______

Rate law for the reaction A + 2B rarr C , is found to be Rate = k [A] [B]. If the concentration of reactant B is doubled keeping the concentration of A constant, the value of rate constant will be

The rate law for a certain reaction is found to be : Rate = k[A] [B]^(2) How will the rate of this reaction compare if the concentration of A is doubled and the concentration of B is halved ? The rate will :

[A] = reactant concentration at time 't', k = rate constant

For a hypothetical reaction, A + B + C to Products, the rate law is determined to be rate = k[A][B]^(2) . If the concentration of B is doubled without changing the concentration of A and C, the reaction rate:

In the reaction 2A+B to A_2B , Rate = k[A]^2 [ B ] if the concentration of A is doubled and that of B is halved, then the rate of reaction will:

For the reaction A + B rarr C , it is found that doubling the concentration of A increases the rate by 4 times, and doubling the concentration of B doubles the reaction rate. What is the overall order of the reaction ?