The reaction N2 (g)+ 3H2 (g)→ 2NH3 (g) is used to produce ammonia (NH3) commercially. If 1.4 g of N2 is used in the reaction, how many grams of H2 will be needed?

Question

I need help in chemistry very much!

Answer 1

Hi John,

So first you need to the grams of N2 to moles of N2:

1.4 g N2*(1 mol N2/28.0314g of N2)=0.03447 mols of N2

Then you have to convert moles of N2 to Moles of NH3 by multiplying it by the mole to mole ratio.

0.03447 mol N2 * (3 mol NH3 /1 mol N2)= 0.1034 mol of H2

Now we convert this to grams by multiplying by the molar mass of H2

0.1034 mol H2 * (1.00784 g H2/1 mol H2)= 0.1042 g of H2 is the amount you need.