Calculate the order of the reaction in A and B :-
`{:(A,,,B,,,Rate),(("mol"//1),,,("mol"//1),,,),(0.05,,,0.05,,,1.2xx10^(-3)),(0.10,,,0.05,,,2.4xx10^(-3)),(0.05,,,0.10,,,1.2xx10^(-3)):}`

The following data are for the reaction A+B rarr Products: {:(Conc. of A(M),,Conc. of B(M),,Initial rate),(,,,,(mol L^(-1) s^(-1))),(0.1,,0.1,,4.0xx10^(-4)),(0.2,,0.2,,1.6xx10^(-3)),(0.5,,0.1,,1.0xx10^(-2)),(0.5,,0.5,,5.0xx10^(-2)):} (a) What is the order with respect to A and B for the reaction? (b) Calculate the rate constant Determine the reaction rate when the concentrations of A and B are 0.2 M and 0.35 M respectvely.

The data given below are for the reaction of NO and Cl_(2) to from NOCl at 295 K . {:([Cl_(2)],[NO],,,"Initial rate" (mol litre^(-1) sec^(-1))),(0.05,0.05,,,1xx10^(-3)),(0.15,0.05,,,3xx10^(-3)),(0.05,0.15,,,9xx10^(-3)):} (a) What is the order with respect to NO and Cl_(2) in the reaction? (b) Write the rate expression. (c ) Calculate the rate constant. (d) Determine the reaction rate when conc. of Cl_(2) and NO are 0.2 M and 0.4 M respectively.

The experimental data for the reaction 2A+B_(2)to2AB is given below. Based on the data write the rate equation. {:("[A],mol L"^(-1),[B_(2)]", mol L"^(-1),"Rate, mol L"^(-1)s^(-1)),(0.5,0.5,1.6xx10^(-4)),(0.5,1.0,3.2xx10^(-4)),(1.0,1.0,3.2xx10^(-4)):}

For the reaction 2A+BrarrC , the values of initial rate at different reactant concentrations are given in the table below. The rate law for the reaction is : {:([A]("mol"L^(-1)),[B]("mol"L^(-1)),{:("Initial Rate"),("mol"^(-1)s^(-1)):}),(0.05,0.05,0.045),(0.10,0.05,0.090),(0.20,0.10,0.72):}

In data given below. {:(,[A],[B],"rate"),(,mol//L,mol//L,mol L ^(-1)s^(-1)),(a., 0.02,1.2,3.0xx10^(-3)),(b.,0.04,2.4,6.0xx10^(-3)):} The reaction may be

In data given below. {:(,[A],[B],"rate"),(,mol//L,mol//L,mol L ^(-1)s^(-1)),(a., 0.02,1.2,3.0xx10^(-3)),(b.,0.04,2.4,6.0xx10^(-3)):} The reaction may be

Find : 0.05xx10

From the following data answer the questions Reaction A+B rarr P {:([A]M,,[B]M,,Initially rate (M sec^(-1)),,,),(,,,,at 300K,at 400K,,),(2.5xx10^(-4),,3.0xx10^(-5),,5.0xx10^(-4),2.0xx10^(-3),,),(5.0xx10^(-4),,6.0xx10^(-5),,4.0xx10^(-3),,,),(1.0xx10^(-3),,6.0xx10^(-5),,1.6xx10^(-2),,,):} The value of rate constant at 300 K is (M^(-2)sec^(-1))

The bromination of acetone that occurs in acid solution is represented by this equation. CH_(3)COCH_(3)Br(aq)+Br_(2)(aq) to CH_(3)COCH_(2)Br(aq)+H^(+)(aq)+Br^(-)(aq) These kinetic data were obtained for given reaction concentrations. Initial concentrations, M {:([CH_(3)COCH_(3)],[Br_(2)],[H^(+)],"Initial rate, disap"),(,,,"pearance of " Br_(2)),(0.30,0.05,0.05,5.7xx10^(-5)),(0.30,0.10,0.05,5.7xx10^(-5)),(0.30,0.10,0.10,1.2xx10^(-4)),(0.40,0.05,0.20,3.1xx10^(-4)):} Based on these data, the rate equation is