Given the reaction between 2 gases represented by A₂ and B₂ to give the compound AB_(g),

A₂(g) + B_2(g) $$\rightleftharpoons$$ 2AB_(g)

At equilibrium, the concentration of
A₂ = 3.0 $$ \times $$ 10^$$-$$3 M, of B₂ = 4.2 $$ \times $$ 10^$$-$$3 M, of AB = 2.8 $$ \times $$ 10^$$-$$3 M
If the reaction takes place in a sealed vessel at 527^oC, then the value of K_c will be

The value of $$\Delta $$H for the reaction
X_2(g) + 4Y_2(g) $$\rightleftharpoons$$ 2XY_4(g)
is less than zero. Formation of XY_4(g) will be favoured at

For the reaction, N_2(g) + O_2(g) $$\rightleftharpoons$$ 2NO_(g), the equilibrium constant is K₁. The equilibrium constant is K₂ for the reaction,
2NO_(g) + O_2(g) $$\rightleftharpoons$$ 2NO_2(g)
What is K for the reaction,
NO_2(g) $$\rightleftharpoons$$ $${1 \over 2}$$N_2(g) + O_2(g)

The reaction,
2A_(g) + B_(g) $$\rightleftharpoons$$ 3C_(g) + D_(g)
is begun with the concentrations of A and B both at an initial value of 1.00 M. When equilibrium is reached, the concentration of D is measuread and found to be 0.25 M. The value for the equilibrium constant for this reaction is given by the expression