The initial concentration of [A] = 0.3 mol/lit. The concentration after 2.3 min is 0.15 moles/lit. What is the value of rate constant.

For the reaction Cl_(2)+2I^(-)toI_(2)+2CI^(-) , the initial concentration of I^(-) was 0.20 mol "lit"^(-1) and the concentration after 20 min was 0.18 mol "lit"^(-1) . If the rate of formation of I_(2) in mol "lit"^(-1) "min"^(-1) is x xx 10^(-4) then the value of x is

A_((g))toB_((g)) is a first order reaction. The initial concentration of A is 0.2 mol. "lit"^(-1) . After 10 minutes the concentration of B is found to be 0.18"mol. lit"^(-1) . The rate constant ("in min"^(-1)) for the reaction is

For the reaction, Ato products the rate of reaction is 7.5xx10^(-4)" mole. lit"^(-1)"sec"^(-1) . If the concentration of A is 0.5" mole lit"^(-1) , the rate constant is

The initial concentration of N_(2)O_(5) in the first order reaction N_(2)O_(5)to2NO_(2)+1/2O_(2) was 1.24xx10^(-2) mole /lit at 318 k. The concentration of N_(2)O_(5) after 60 min is 0.20xx10^(-2) mole/lt. Calculate the rate constant of reaction at 318 K

In a first order ractin, the concentration of the reaction is reduced from 0.6 mol /L to 0.2 mol/L in 5 min. Calculate the rate fconstnat (k).

For a reaction Ato Product, half life is 50 min, when the initial concentration of A is 4 molar Half life of same reaction is 80 min, when the initial concentration of A is 2 molar. Then

The initial concentration of ethyl acetane is 0.85 mol L^(-1) . Following the acid catalysed hydrolysis the , concentrations of ester after 30 min and 60 min of the reaction are respectively 0.8 and 0.754 mol L^(-1) . Calculate the rate constant and pseudo rate constant.

3 moles of NH_3 are allowed to dissociate in a 5 litre vessel and the equilibrium concentration of N_2 is 0.2 mole/lit . Then the total number of moles at equilibrium is

Rate constant for a reaction, XtoY , is 4.5xx10^(-3)" min"^(-1) . If the initial concentration of X is 1 M, what is the rate of reaction after one hour ?