For the reaction, `A+B hArr C,K_c=2` at a particular temperature. Initial concentrations of A, B and C are `2mol*L^(-1),1mol*L^(-1)` & `1mol*L^(-1)` respectively. Express graphically the change in concentrations of A, B and C with time.

For the reaction A+2Brarr3C , the rate in terms of change in concentration of A, B and C are x, y and z "mol .L "^(-1).s^(-1) , respectively, Establish a relation between x , y and z .

The pressure of a certain amount of gas is 1 atm. At what temperature will be concentration of this gas be 1 mol*L^(-1) ?

For the reaction, H_2(g)+CO_2(g)to CO(g)+H_2O(g) occurring in a closed vessel at a particular temperature. the initial concentrations of the reactants are [H_2]=[CO_2]=1 mol*L^(-1) . Before reaching the equilibrium, if x mol*L^(-1) of H_2 has reacted then prove that : x=(sqrt(K_c))/(1+sqrt(K_C)) where K_c =equilibrium constant.

The inversion temperature Ti(K) of hydrogen is (Given van der Waal’s constant a and b are 0.244 atm L^2 mol^(-2) and 0.027 L mol^(-1) respectively.)

In the process AtoBtoC , the change in internal energy of the system in the steps AtoB and B to C are -x jK*mol^(-1) and ykJ*mol^(-1) , respectively. What will be the change in internal energy of the system in the step C toA ?

At a particular temperature, the values of rate constant of forward and backward reactions are 1.5xx10^(-2)L*mol^(-1)*s^(-1) and 1.8xx10^(-3)L*mol^(-1)*s^(-1) respectively for the reaction A+B hArr C+D . Determine the equilibrium constnt of the reaction at that temperature.

Consider the reaction 2Ararr4B+C taking place in a closed container. If the concentration of B increases to 5xx10^(-3)"mol".L^(-1) in 10s , then find the rate of formation of B

Consider the reaction 2Ararr4B+C taking place in a closed container. If the concentration of B increases to 5xx10^(-3)"mol".L^(-1) in 10s , then find the reaction -rate in the given interval.

The initial concentration of the reactant in a zero order reaction is 1.386 "mol.L"^(-1) The half-life of the reaction is 20s. Calculate: the rate constant

2Ararr4B+D , in this reaction, concentration of B increases to 2xx10^(-3)"mol.L"^(-1) after 10s from the start of the reaction . Calculate : rate of formation of B