Dinitrogen and dihydrogen react as `N_2(g)+3H_2(g) to 2NH_3(g)` Will any of the reactant remain unreacted?

Dinitrogen and dihydrogen react as N_2(g)+3H_2(g) to 2NH_3(g) If yes, calculate the mass of the reactant.

Dinitrogen and dihydrogen react as N_2(g)+3H_2(g)to2NH_3(g) Calculate the mass of produced if 2.00xx10^3g dinitrogen reacts with 1.00xx10^3g of dihydrogen

Dinitrogen and dihydrogen react with each other to produce ammonia according to the following chemical equation: 'N_2(g)+3H_2(g) rarr 2NH_3(g)' i. Calculate the mass of ammonia produced if '2.00 xx 10^3' g dinitrogen reacts with '1.00 xx 10^3 g of dihydrogen. ii. Will any of the two reactants remain unreacted? iii. If yes, which one and what would be its mass?

A mixture of 1 mol of Al and 3 mol of Cl_2 are allowed to react as 2Al_(s) + 3Cl_(2(g)) rarr 2AlCl_3 How many moles of excess reactant left unreacted?

In the manufacture of NH_(3) by Haber process N_(2)(g) + 3H_(2)(g) to 2NH_(3)(g) the rate of the reaction was measured as - (d[N_(2)])/(dt) = 2 xx 10^(-4) "mol" L^(-1)s^(-1) . The rate of the reaction expressed in terms of H_2 is:

The CHEical equation for the manufacture of ammonia is N_2(g)+3H_2(g) to 2NH_3(g) Calculate the amount of H_2 required to react with 28 g of N_2 , completely. [Hint Molecular mass of N_2 = 28 , H_2 =2 ]

1.5 g of H_2 react with 14.5 g of O_2 to form water Calculate the amount of the reactant which remains unreacted

The CHEical equation for the manufacture of ammonia is N_2(g)+3H_2(g) to 2NH_3(g) What will be the volume of NH_3 , formed at STP, if 22.4L of N_2 is completely reacted?

3g of hydrogen reacts with 30g of oxygen to yield H_2O . Calculate the amount of reactant: which is unreacted.