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) to 2NH_3(g) Will any of the reactant remain unreacted?

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

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 ]

If the K_(c) of the reaction N_(2)(g)+3H_(2)(g) iff 2NH_(3)(g) at 750 K is 49, then the K_(c) of the reaction NH_(3)(g) iff 1/2N_(2)(g)+3/2H_(2)(g) at the same temperature is

If 6.023xx10^23 molecules of N_2 react completely with H_2 according to the equation: N_(2(g)) + 3H_(2(g)) rarr 2NH_(3(g)) , then calculate the numbers of molecules of NH_3 formed.

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?

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?

H_2(g)+I_2(g)harr2HI(g) What is the total number of moles of reactants?

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 balanced chemical equation of a reaction (at STP) is given below. 2H_(2((g))+O_(2(g))rarr2H_2O_((g)) : Calculate the mass of water formed as a result of the reaction (a).