Final answer:
To react with 50.0 g of nitrogen, approximately 10.8 g of hydrogen is required according to the stoichiometric relationship in the balanced chemical equation for the formation of ammonia.
Step-by-step explanation:
The question pertains to a stoichiometry problem in chemistry involving the reaction of hydrogen (H2) with nitrogen (N2) to produce ammonia (NH3). First, we need to use the molar mass of nitrogen to convert grams to moles. Nitrogen has a molar mass of approximately 28.0 g/mol, so 50.0 g of nitrogen is equivalent to 50.0 g / 28.0 g/mol = 1.79 moles of N2.
According to the balanced chemical equation N2 + 3 H2 → 2 NH3, one mole of nitrogen reacts with three moles of hydrogen. So, 1.79 moles of nitrogen will react with 3 × 1.79 = 5.37 moles of hydrogen.
To find out how many grams of hydrogen this corresponds to, we use the molar mass of hydrogen, which is approximately 2.0 g/mol (since each hydrogen molecule has 2 atoms of hydrogen). Therefore, 5.37 moles of H2 × 2.0 g/mol = 10.74 g of H2, which we can round to 10.8 g of H2 as the answer to the original question.
Thus, to completely react with 50.0 g of nitrogen, you would need approximately 10.8 g of hydrogen.