Consider the equilibrium:
`N_(2)(g)+3H_(2)(g)hArr 2NH_(3)(g)+`heat. Apply the i.e., chatelier's principle to explain the effect of pressure, temperature and addition of inert gas at constant volume on the equilibrium yield of `NH_(3)`.

Consider the equilibrium : N_2(g)+3H_2(g)rarr2NH_3(g)+heat Apply the Le Chatelier’s principle to explain the effects of pressure, temperature, and addition of inert gas at constant volume on the equilibrium yield of NH_3 . What is buffer solution? Give one example of the buffer solution.

Addition of inert gas at constant volume to the equilibrium N_2(g)+3H_2(g)iff2NH_3(g) results.

For the equilibrium reaction H_(2(g))+I_(2(g))hArr 2HI_((g))

PCl_(5) (g) to PCl_(3) (g) + Cl_(2) (g) , DeltaH^(0) = +124 kJ * mol^(-1) Applying Le Chatelier's principle , discuss the effect of increase in pressure , temperature and addition of inert gas at constant volume on the equilibrium of this reaction .

For reaction N_2(g)+3H_2(g)hArr 2NH_3(g) which of the following is valid

For the reaction, N_2(g)+3H_2(g)hArr2NH_3(g) +heat the equilibrium shifts in forward direction-

In the equilibrium N_(2)+3H_(2)hArr2NH_(3) , the maximum yield of ammonia will be obtained with the process having

For the relation, H_(2)(g)+CO_(2)(g) hArr H_(2)O(g)+CO(g) show the equilibrium yield of the products is independent of pressure at constant temperature.

For the reaction, 2NH_(3)(g) to N_(2)(g)+3H_(2)(g) -

For the reaction, N_(2)(g)+3H_(2)(g)rarr2NH_(3)(g) express the rate of the reaction with respect to the reactants and the product formed.