The reaction between A and B is first order with respect to A and zero order with respect to B. Fill in blanks in the following table: 1)A and B =0.1,Initial rate=2.0*10^2, 2)B=0.2 and initial rate=4.0*10^2,3)A=0.4 and B=0.4,4)B=0.2 and initial rate =2.0*10^2

The reaction A+2 B rarr C obeys the rate equation rate=k[A]^0.5[B]^1.5 what is the order of the reaction?

For a reaction A + BrarrC + D . The order with respect to A is 1 and that of B is 2. How is the rate affected when the concentration of B Is trippled?

Will the following statement be consistent? why? for two events A and B P(A) =0.3 , P(B)=0.2 and P(A cap B) is 0.1

The value of E.N of atom A and B are 1.2 and 4.0 respectively. The percentage ionic character of A-B and bond is

The rate law for the reaction below is given by the expression k[A][B] A + B to product. If the concentration of B is increased from 0.1 to 0.3 mol, keeping the value of A at 0.1 mol, the rate constant will be

The reaction A rarr X is a first order reaction which takes place in a vessel with initial concentration of A as 10 M. The rate constant for this reaction is 4.16 h^(-1) . In the presence of a catalyst, the reaction A rarr Y follows second-order kinetics and the rate constant is 0.2 min^(-1) M^(-1) . What should be the initial concentration of A in the presence of catalyst so that the value of t_(1//2) for both the reactions is the same?

For the zero order reaction A to B + C , initial concentration of Ais 0.1 M. lf[A] = 0.08 M after 10 minutes, then its half-life and completion time are respectively:

In a first order reaction mathbf(A) rarr (B) if (k) is rate con stant and initial concentration of the reactant A. is 0.5 . M then the.half life is