Question

If 10.81g of N₂H₄ is used, what mass of nitrogen produced?

2N₂H₄(l) + NaO₄(l) → 3N₂(g) + 4H₂O(l)

Answer 1

Using the stoichiometry of the balanced equation, the amount of nitrogen gas is calculated in moles and converted to grams, resulting in approximately 14.16 g of nitrogen gas.

Step-by-step explanation:

To find the mass of nitrogen produced from 10.81g of N₂H₄, we can use the stoichiometry of the given reaction. Firstly, we calculate the molar mass of N₂H₄ (14.01x2 + 1.01x4 = 32.05 g/mol) and use it to find out the number of moles of N₂H₄ used:

(10.81 g N₂H₄) / (32.05 g/mol) = 0.337 moles N₂H₄
The balanced equation shows that 2 moles of N₂H₄ produce 3 moles of N₂. So the mole ratio of N₂H₄ to N₂ is 2:3.

(0.337 moles N₂H₄) x (3 moles N₂ / 2 moles N₂H₄) = 0.5055 moles N₂
Now we convert the moles of N₂ to mass using its molar mass (14.01 g/mol per N, so 28.02 g/mol for N₂):

(0.5055 moles N₂) x (28.02 g/mol) = approximately 14.16 g N₂