To solve this problem, we need to use the stoichiometry of the reaction. From the balanced equation, we can see that 3 moles of hydrogen gas (H2) are required to react with 1 mole of nitrogen gas (N2).
1 mole of N2 has a molar mass of 14.01 g/mol, so 3.80 g of N2 is equal to 3.80 g / 14.01 g/mol = 0.271 mol of N2.
Therefore, we need 3 times that amount of H2, so we need 0.271 mol × 3 = 0.813 mol of H2.
The molar mass of H2 is 2.02 g/mol, so 0.813 mol of H2 is equal to 0.813 mol × 2.02 g/mol = 1.64 g of H2.
Therefore, 1.64 grams of H2 are needed to react with 3.80 g of N2.
Nitrogen gas reacts with hydrogen gas to produce ammonia via the following reaction:
N2 (g) + 3H2(g) →2NH3 (g)
How many grams of H2 are needed to react with 3.80 g of N2?
Express your answer with the appropriate units
1 answer