For the reaction:
`N_(2)+3H_(2)hArr2NH_(3)`
If the initial concentration of `N_(2)` and `H_(2)` are a and b moles per litre and x moles per litre of ammonia is formed at equilibrium, what is the equilibrium concentration of hydrogen?

For the reaction, N_(2) + 3H_(2) hArr 2NH_(3) in a vessel, equal moles of N_(2) and H_(2) are mixed to attain equilibrium.

For the reaction, N_(2)+3H_(2)hArr2NH_(3) , in a vessel equal moles of N_(2) and H_(2) are mixed to attain equilibrium. At equilibrium:

For the reaction H_(2)(g)+CO(g)hArrCO(g)+H_(2)O(g), if the initial concentration of [H_(2)]=[CO_(2)] and x moles /litres of hydrogen is consummed at equilibrium , the correct expression of K_(p) is :

For the reaction H_(2)(g)+CO(g)hArrCO(g)+H_(2)O(g), if the initial concentration of [H_(2)]=[CO_(2)] and x moles /litres of hydrogen is consummed at equilibrium , the correct expression of K_(p) is :

A reaction N_(2)+ 3H_(2) hArr 2NH_(3) + 92 k.j is at equilibrium. If the concentration of N_(2) is increased the temperature of the system

A reaction N_(2)+ 3H_(2) hArr 2NH_(3) + 92 k.j is at equilibrium. If the concentration of N_(2) is increased the temperature of the system

In the process N_(2)+3H Leftrightarrow 2NH_(3) , the initial concentration of Nitrogen and Hydrogen are one mole per litre and 3 moles per litre respectively. The equilibrium constant of the reaction is x. Then K_(C)" for "2NH_(3) Leftrightarrow N_(2)+3H_(2) is

In the reaction, N_2(g) +3H_2(g) hArr2NH_3(g) increase in H_2 concentration equilibrium: