How do I solve this? What is the answer?

Question

4HCl(g) + 6NO(g)        5N2(g) + 6H2O(g)

Given the reaction how many grams of nitrogen gas would be produced when 25 moles of hydrochloric acid react completely with nitrogen monoxide?

Answer 1

From the question, we can determine that 25 moles of hydrochloric acid reacts COMPLETELY with nitrogen monoxide. Using this information, we can determine that hydrochloric acid is the limiting reactant and use dimensional analysis to find the number of moles of nitrogen gas that would be produced.

25 mol HCl * [5 mol N₂ / 4 mol HCl] = 31.25 mol N₂

Now that we've determined that 31.25 moles of N₂ will be produced, we can use dimensional analysis again to find the grams of nitrogen gas that will be produced. Note that because N₂ is a diatomic, we multiple its mass by 2 to convert from moles to grams.

31.25 mol N₂ * [(14.007*2) g N₂ / 1 mol N₂] = 875.4375 g N₂

Taking significant figures into account, the final answer would be that 880 grams of nitrogen gas will be produced. Hope this helps!