At equilibrium, the concentrations of `N_2 = 3.0 xx 10^-3M, O_2 - 4.2 xx 10^-3M` and `NO = 2.8 xx 10^-3M ` in a sealed vessel at 800K. What will be `K_c` for the reaction
`N_2(g) +O_2(g) iff 2NO(g)`

For the equilibrium N_2 (g) + O_2(g) = 2 NO (g)

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

Establish the relation between K_p and K_c for the reaction 2SO_2(g)+O_2(g)iff2SO_3(g)

The equilibrium constant (K_c) for the reaction 2HCl(g) iff H_2(g) + Cl_2(g) Is 4 xx 10^(-34) at 25^@C . What is the equilibrium constant for the reaction ? 1/2 H_2(g) + 1/2Cl_2(g) iff HCl(g)

K_1 and K_2 are the respective equilibrium constants for the following two reactions : (i) N_2 (g) + O_2 (g) iff 2NO(g) (ii) 2NO(g) + O_2(g) iff 2NO_2(g) Then the equilibrium constant for the reaction N_2 (g) + 2O_2(g) iff 2NO_2(g) will be

Write the expressions of K_(c) and K_(p) for the reaction: 3O_(2)(g)hArr2O_(3)(g) .

At 527^@C , the reaction given below has K_c = 4 NH_3(g) iff 1/2 N_2(g) +3/2 H_2(g) What is the K_p for the reaction ? N_2(g) + 3H_2(g) iff 2NH_3(g)

If K_p=K_cxx(RT)^xx for the reaction SO_2(g)+1/2O_2(g)iffSO_3(g) . Then x will be

The equilibrium constant (K_c) for the reaction N_2(g) + O_2(g) rarr 2NO (g) at temperature T is 4 xx 10^-4 . The value of K_c for the reaction NO(g) rarr 1/2 N_2(g) + 1/2 O_2(g) at the same temperature is