Final answer:
To find the mass of nitrogen gas produced from 25.6 g of N2H4 with excess N2O, a stoichiometric calculation is performed using the balanced chemical equation. The result is 33.6 grams of N2.
Step-by-step explanation:
The student is asking how many grams of nitrogen gas (N2) can be produced from 25.6 grams of hydrazine (N2H4), given the reaction 2 N2H4(g) + N2O(g) → 3 N2(g) + 4 H2O(g). To answer this, we'll use stoichiometry, which involves the mass/molar ratios of reactants and products in a balanced chemical equation.
First, we need to calculate the molar mass of N2H4 (M = 1x14 + 4x1 = 32 g/mol) and convert the mass of N2H4 to moles by dividing the given mass by the molar mass (25.6 g ÷ 32 g/mol = 0.8 mol).
From the balanced equation, 2 moles of N2H4 produce 3 moles of N2. So, 0.8 moles N2H4 will produce (0.8 mol ÷ 3 mol N2 / 2 mol N2H4) = 1.2 moles of N2.
The molar mass of N2 is (2x14) = 28 g/mol. Therefore, the mass of the nitrogen produced will be (1.2 mol × 28 g/mol) = 33.6 grams of N2.