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:

Rate law for the reaction A + 2B to 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

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 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

Interpration of the rate law: For a hydrothertical reaction X+Y+Zrazrr products the rate law is determined to be "Rate" =k[X][Y]^(2) What happens to the reaction rate when we make each of the following concentration changes ? (a) We dobule the concentration of X without changing the concentration of Y or Z. (b) We double the concentration of Y without changing the concentration of X or Z. (c ) We double the concentrations of Z without changing the concentration of X or Y. (d) We double all three concentrations simultaneously. Strategy: Interpret the law to predict the changes in reaction rate. Remember that changing concentrations does not change the value of k.

Rate law for the reaction A+2BrarrC , 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 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: