The following concentrations were obtained for the formation of `NH_3` from `N_2` and `H_2` at equilibrium at `500K. [N_2] = 1.5 xx 10^-2M. [H_2] = 3.0 xx10^-2 M` and `[NH_3] =1.2 xx 10^-2 M`. Calculate equilibrium constant.

Given, the reaction between two gases represented by A_2 and B_2 to give the compound AB(g). A_2(g) + B_2(g) iff 2AB(g) At equilibrium, the concentration of A_2 = 3.0xx10^-3M of B_2 = 4.2 xx 10^-3M of AB = 2.8 xx 10^-3M If the reaction takes place in a sealed vessel at 527^@C , then the value of K_c will be

The following observations were taken for determining surface tension T of water by capillary method: diameter of capillary, D = 1.25 xx 10^(-2) m rise of water h = 1.45 xx10^(-2) m. Using g = 9.80 ,m//s^(2) and the simplified relation T = (rhg)/(2) xx 10^(3) N//m , the possible error in surface tension is closest to:

Predict which of the following facts for the equilibrium reaction 2NH_3(g) iff N_2(g) + 3H_2(g) holds good?

At 448^@C , the equilibrium constant (K_C) for the reaction H_2(g) + I_2(g) iff 2HI(g) is 50.5. Predict the direction in which the reaction will proceed to reach equilibrium at 448^@C , if we start with 2.0 xx 10^-2 mol of HI, 1.0 xx 10^-2 mol of H_2 and 3.0 xx 10^-2 mol of I_2 In a 20L- container.

At 25^(@)C temperature, the molar concentrations of NH_(3),NH_(4)^(+) and OH^(-) at equilibrium are 9.6xx10^(-3)(M),4.0xx10^(-4)(M) and 4.0xx10^(-4)(M) respectively. Determine the ionisation constant of NH_(3) at that temperature.

If Ag + 2NH_3 iff [Ag(NH_3)_2] K_1 = 1.8 xx 10^7 Ag^+ +Cl^- iff AgCl K_2 = 5.6 xx 10^9 Then for AgCl + 2NH_3 iff [Ag(NH_3)_2]^+ + Cl^- What will be the value of equilibrium constant?

The following euilibrium constants are given: N_2+3H_2 H_2+1/2O^2 The equilibrium constant for the oxidation of 2 mol of NH_3 to give NO is-

A buffer solution is prepared in which the concentration of NH_3 is 0.30 M and the concentration of NH_4^(+) is 0.20 M. If the equilibrium constant, K_b for NH_3 equals 1.8xx10^-5 , what is the pH of this solution?

An aqueous solution contains 0.10 M H_(2) S and 0.20 M HCl . If the equilibrium constants for the formation of HS^(-) from H_(2) S is 1.0 xx 10^(-7) and that of S^(2-) from HS^(-) ions is 1.2 xx 10^(-13) then the concentration of S^(2-) ions in aqueous solution is -

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.