The mass of `N_2F_2` produced by the reaction of `2.0g` of `NH_3 and 8.0g` of `F_2` is `3.56g`. What is the per cent yield ?

In Haber's process 50.0g of N_(2) [g] and 10.0 g of H_(2) [g] are mixed to produce NH_(3) [g]. What is the number of moles of NH_(3) [g] formed?

In Haber's process 50.0 g of N_(2)(g) and 10.0 g of H_(2)(g) are mixed to produce NH_(3)(g) . What is the number of moles of NH_(3)(g) formed?

A solution is prepared by adding 2 g of a substance A to 18 g of water. Calculate the mass per cent of the solute.

What volume of H_(2) at NTP is required to convert 2.8g of N_(2) in to NH_(3) ?

The yield of product in the reaction 2A_((g)) + B_((g)) hArr 2C_((g)) + Q K J would be lower at :

Dinitrogen and dihydrogen react with each other to produce ammonia according to the following chemical equation. N_(2)(g)+H_(2)(g)to2NH_(3)(g) i) Calculate the mass of ammonia produced if 2.00xx10^(3)g dinitrogen reacts with 1.00xx10^(3)g of dihydrogen. ii) Will any of the two reactants remain unreacted ? iii) If yes, which one and what would be its mass?

Equilibrium constant, K_(c) for the reaction N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g) at 500K is 0.061 At particular time, the analysis shows that composition of the reaction mixture is 3.0 mol L^(-1)N_(2) , 2.0 mol L^(-1)H_(2) and 0.5 mol L^(-1)NH_(3) . Is the reaction at equilibrium ? If not in which direction does the reaction tend to proceed to reach equilibrium ?