The equilibrium constant for the following reactio is `1.6 xx 10^5` at 1024 K. `H_2(g) + Br_2(g) hArr 2HBr(g)` Find the equilibrium pressure of all gases if 10.0 bar of HBr is introduced into a sealed container at 1024 K.

The equilibrium constant for the following reaction at 25^@C is 2.9 xx 10^9 . Calculate standard voltage of the cell. Cl_(2(g)) +Br_(aq)^- narr Br(2(i))+2CI_((aq))^- .

Write expressions of k_c for following chemical reactions. 2SO_2(g) + O_2(g) harr 2SO_3(g) .

The equilibrium constant for the reaction H_2 (g) +I_2 (g) hArr 2 HI (g) is 32 at a given temperature.The equilibrium concentrations of I_2 and HI are 0.5 xx 10 ^(-3) and 8xx 10^(-3)M respectively.The equilibrium concentration of H_2 is.

Write the expression for the equilibrium constant, K_C for each of the following reactions: 2Cu(NO_3)_2 hArr 2CuO(s) + 4 NO_2(g)

For the following reaction at 298 K, H_(2(g))+1/2 O_(2(g))to H_2 O_((l)) , Which of the following alternative is CORRECT?

Write expressions of k_c for following chemical reactions. N_2 O_4(g) harr 2NO_2(g) .

In the equilibrium reaction involving then diansociation of CaCO_3(s) : CaCO_3(s) hArr CaO (s) + CO_2 (g) , the equilibrium constant is given by

At 700 K , equilibrium constant for the reaction, H_2(g) + I_2(g) hArr 2HI(g) is 54.8 if 0.5 mol L^(-1) of HI(g) is present at equilibrium at 700K,what are the concentration of H_2(g) and I_2(g) assuming that we initially started with HI(g) and allowed it to reach equilibrium at 700K?

Equilibrium constants K_1 and K_2 for the following equilibria NO_(g) +1/2O_2 hArr NO_(2(g)) and 2NO_(2(g)) overset(K_2)(hArr) 2NO_(g)+ O_(2(g) are related as