For the reaction : $CO(g)+\frac{1}{2}{O}_2(g)\rightleftharpoons C{O}_2(g);K_p\mathrm{/}{K}_{c}CO(g)\; +\; \backslash frac12O\_2(g)\backslash rightleftharpoons\; CO\_2(g)\; ;\; K\_p\; /\; K\_c$ is

What is the equilibrium expression for the following reaction?$P_{4(s)}+5O_{2(g)}\rightleftharpoons P_4{O}_{10(s)}P\_\{4(s)\}\; +\; 5O\_\{2(g)\}\backslash rightleftharpoons\; P\_4O\_\{10(s)\}$

A mixture of $N_{2}N\_2$ and $H_{2}H\_2$ in the molar ratio 1:3 attains equilibrium when 50% of the mixture has reacted. If P is the total pressure of the mixture then partial pressure of $N{H}_{3}NH\_3$ formed is

A and B are gaseous substances which react reversibly to give two gaseous substances C and D, accompanied by the liberation of heat. When the reaction reaches equilibrium, it is observed that $K_p=K_{c}K\_p\; =\; K\_c$. The equilibrium cannot be disturbed by

The value of equilibrium constant for an endothermic reaction

A reaction reaches a state of chemical equilibrium only when

According to Le Chatelier’s principle, adding heat to a solid and liquid in equilibrium will cause the

Vapour density of $PC{l}_{5}PCl\_5$ is 104.16 but when heated at $230^{\circ }C230^\backslash circ\; C$ its vapour density is reduced to 62. The degree of dissociation of $PC{l}_{5}PCl\_5$ at this temperature will be

The vapour density of completely dissociated $N{H}_{4}ClNH\_4Cl$ would be :

If the reaction $N_2{O}_4\rightleftharpoons 2N{O}_{2}N\_2O\_4\backslash rightleftharpoons\; 2NO\_2$, is started with one mole of $N_2{O}_{4}N\_2O\_4$ and $\alpha \backslash alpha$ is degree of dissociation of $N_2{O}_{4}N\_2O\_4$ then the number of moles at equilibrium will be :