Question

13. Nitrogen gas is reacted with hydrogen gas to form nitrogen trihydride. a. Write and balance the chemical equation. b. How many liters of nitrogen trihydride are produced at STP if 80.28 grams of hydrogen gas is reacted in an excess of nitrogen? How many grams of hydrogen are needed to fully react 621.9 grams of nitrogen gas? How many liters of nitrogen gas are needed to completely react 90.38 L of hydrogen gas at STP?

Answer 1

13 @ N2 (9) + 3H₂(g) → 2NH3 (8) 6 Mole of hydrogen = 80.28 g = 40.14 mol 2 g/mol Mole of nitrogen tri hydside = 2 x mole of hydrogen 2 x 40.14 = 26.76 mol 1 mol = 22.42 26.76 mol = 22.4x 26.76 = 599.4 L © Mole of N2 = 621.9 g = 22.2 mol 28 g/mol Mole of H₂ = 3x mole of N2 = 34 22.2 = 66.6 mol Mass of hydrogen = 66.6 mol x 2g /mol = 133.26 91 d Mole of hydrogen = . 90.38L 22.4 L/mol = 4.035 mol 1 x 4.035 mol = 1.34 5 mol Volume of nitrogen at STP = 1.345 mol X 22 4 4mol 530.134