A decomposes as . The rate of appearance of B, taking 2 M concentration of A, is equal to :

For the reaction A+BrarrC , the rate law is : Rate=k [A]^(2) . Which change(s) will increase the rate of the reaction? (P) Increasing the concentration of A (Q) Increasing the concentration of B

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 :

For the reaction (1)/(2)Ararr2B , what is the relation between the rate of appearance of B and the rate of disappearance of A ?

For the reaction : 2A + 2B rarr 2C+ D , if concentration of A is doubled at constant [B], the rate increase by a factor of 4. If the concentration of B is doubled with [A] being constant the rate is double. Write the rate law of the reaction.

For a reaction A+BrarrP , the rate is given by Rate =k[A][B]^(2) How is the rate of reaction affected if the concentration of B is doubled ?

A chemical reaction 2A rarr 4B+C , in gaseous phase shows an increase in concentration of B by 5xx10^(-3) M in 10 second. Calculate: (a) rate of appearance of B , (b) rate of the reaction, (c ) rate of disappearance of A .

For a reaction A+B rarr P , the rate is given by - Rate = [A][B]^2 How is the rate of reaction affected if the concentration of B,is doubled?

For the reaction 2A + 3B to 4C, rate of appearance of C is equal to

For the reaction 2A + 3B to 4C, rate of appearance of C is equal to