Question

7.0 g of nitrogen is reacted with 5.0 g of hydrogen to produce ammonia according to the chemical equation shown below. Which of the following statements is false?

N₂(g) + 3H₂(g) --> 2NH₃​(g)
A. 3.5 g of hydrogen are left over
B. Hydrogen is the excess reactant
C. Nitrogen is the limiting reactant
D. The theoretical yield of ammonia is 15 g.

Answer 1

If you mix 5.0 moles of nitrogen and 10.0 moles of hydrogen, you would produce 10.0 moles of ammonia. Hydrogen is in excess because there are more moles of hydrogen than the stoichiometric ratio required for the reaction.

Step-by-step explanation:

According to the balanced chemical equation, 1 mole of elemental nitrogen reacts with 3 moles of elemental hydrogen to produce 2 moles of ammonia. Therefore, if you mix 5.0 moles of nitrogen with 10.0 moles of hydrogen, you would produce 10.0 moles of ammonia. In this case, hydrogen is in excess because there are more moles of hydrogen than the stoichiometric ratio required for the reaction.