Dinitrogen and dihydrogen react with each other to produce ammonia according to the chemical equation :
`N_2 (g) + 3H_2 (g) rarr 2NH_3 (g)`
Calculate the mass of ammonia produced produced if `2.00 xx 10^3 g` nitrogen react with`1.00 xx 10^3 g` dihydrogen.

N_(2) and H_(2) react with to produce ammonia according to the equation: N_(2)(g)+3H_(2)(g) to 2NH_(3)(g) (1) Calculate the mass of ammonia produced if 2.00xx10^(3)g" "N_(2) reacts with 1.00xx10^(3)g off H_(2) . (2) Will any of the two reactants remain unreacted ? (3) If yes, which one and what would be its mass?

Express the equilibrium constant of the reaction in the forms of K_p and K_c - for the reaction, N_2 (g) + 3H_2 (g) rarr 2NH_3 (g) .

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

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

The enthalpy of formation of ammonia is x KJ mol^(-1) . The enthalpy of the reaction 2N_2(g)+6H_2(g) rarr 4NH_3(g)

N_2(g) + 3H_2(g) → 2 NH_3(g) . For the above reaction the correct statement is

For the reversible reaction N_2(g)+3H_2(g) iff 2NH_3(g) +heat The equilibrium shifts in forward direction

Predict which of the following facts for the equilibrium reaction 2NH_3(g) iff N_2(g) + 3H_2(g) holds good?