In the system X+2Y⇌Z, the equilibrium concentrations are, [X]=0.06 mol L −1 ,[Y]=0.12 mol L −1 ,[Z]=0.216 mol L −1 . Find the equilibrium constant of the reaction.

In the system X+2YhArrZ , the equilibrium concentration are, [X]=0.06" mol L"^(-1),[Y]=0.12" mol L"^(-1) , [Z]=0.216" mol L"^(-1) . Find the equilibrium constant of the reaction.

For the system A(g)+2B(g) hArr C(g) the equilibrium concentration is A=0.06 mol L^(-1), B=0.12 mol L^(-1) C=0.216 mol L^(-1) The K_(eq) for the reaction is

For a reaction X+Y = 2Z , 1.0 mo of X 1.5 mol of Y and 0.5 mol of Z where taken in a 1L vessel and allowed to react . At equilibrium , the concentration of Z was 1.0 mol L^(-1) . The equilibrium constant of the reaction is _____ (x)/(15) . The value of x is _____.

The equilibrium of formation of phosgene is represented as : CO(g)+Cl_(2)(g)hArrCOCl_(2)(g) The reaction is carried out in a 500 mL flask. At equilibrium, 0.3 mol of phosgene, 0.1 mol of CO , and 0.1 mol of Cl_(2) are present. The equilibrium constant of the reaction is

In a reaction A+2B hArr 2C, 2.0 moles of 'A' 3 moles of 'B' and 2.0 moles of 'C' are placed in a 2.0 L flask and the equilibrium concentration of 'C' is 0.5 mol // L . The equilibrium constant (K) for the reaction is

The equilibrium concentration of x, y and z are 4, 2 and 2 mol L^(-1) , respectively, at equilibrium of the reaction 2x+y hArr z . The value of K_(c) is ……………..

For A+B hArr C , the equilibrium concentration of A and B at a temperature are 15 mol L^(-1) . When volume is doubled the reaction has equilibrium concentration of A as 10 mol L^(-1) , calculate a. K_(c)

For the reaction, A(g)+2B(g)hArr2C(g) one mole of A and 1.5 mol of B are taken in a 2.0 L vessel. At equilibrium, the concentration of C was found to be 0.35 M. The equilibrium constant (K_(c)) of the reaction would be

In a first order reaction, the concentration of reactant decrease from 400 mol L^(-1) to 25 mol L^(-1) in 200 seconds. The rate constant for the reaction is

For the reaction 2X+Y+Z to X_2 YZ , the rate equation is : Rate =k [X] [Y]^2 with k = 3.0 xx 10^(-6) mol^(-2) L^(2) s^(-) If[X]=0.1 mol L^(-) ,[Y]=0.2 mol L-and [Z]=0.7 mol L^(-) , determine the initial rate of reaction.