For the equilibrium, `Ag_2CO_3(s) iff Ag_2O(s)+ CO_2(g),` equilibrium constants are `3.98 xx 10^-4` and `1.41 xx 10^-2` respectively at 250K and 400K. Calculate the standard enthalpy of decomposition.

The equilibrium constants for the reaction, N_2(g) + O_2(g) iff 2NO(g) , at 1727^@C and 2227^@C are 4.08 xx 10^-4 and 3.6 xx 10^-3 respectively. Calculate the enthalpy change for the reaction. (Given R = 1.987 cal.)

In the equilibrium reaction CO_(2(g))+C_((s))hArr 2CO_((g)) the partial pressure of CO2 and CO are 0.78 atm and 1.22 atm respectively at equilibrium. Calculate the equilibrium constant

2N_2O_5 iff 4NO_2 +O_2 If rate and rate constant for above reaction are 2.40 xx 10^-5 mol L^-1s^-1 and 3xx10^-5s^-1 respectively, then calculate the concentration of N_2O_5

For the reaction, A_(g) + 2B_(g) iff 2C_(g) , the rate constants for the forward and the reverse reactions are 1 xx 10^-4 and 2.5 xx 10^-2 respectively. The value of equilibrium constant, K for the reaction would be

For the equilibrium 2NOCl_((g))hArr2NO_((g))+Cl_(2(g)) the value of the equilibrium constant K_(c) is 3.75xx10^(-6) at 790^(@)C . Calculate K_(p) for this equilibrium at the same temperature.

If the equilibrium constant for N_2(g) + O_2(g) iff 2NO(g) is K, the equilibrium constant for 1/2N_2(g) +1/2 O_2(g) iff NO(g) will be:

For the equilibrium 2SO_(3(g))hArrSO_(2(g))+O_(2(g)) , the value of equilibrium constant is 4.8xx10^(-3) at 700^(@)C . At equilibrium, if the concentration of SO_(3) and SO_(2) are 0.60M and 0.15M respectively. Calculate the concentration of O_(2) in the equillibrium mixture.

Calculate the approximate pH of 0.1 M aqueous H_2S solution. K_1 and k_2 for H_2S are 1.0 xx 10^(-7) and 1.3 xx 10^(-13) respectively at 25^@C