Answer:
Approximately 56.98 kJ of heat will be released in this chemical reaction when 0.3987 moles of NH₃ are mixed with 0.200 mol of O₂.
Step-by-step explanation:
To calculate the quantity of heat released in this chemical reaction, we need to find the moles of N₂H₄ (hydrazine) formed and then use the given enthalpy change (∆H°) to determine the heat released.
From the balanced chemical equation, we can see that the stoichiometric ratio between NH₃ and N₂H₄ is 4:2, meaning that 4 moles of NH₃ produce 2 moles of N₂H₄.
Step 1: Determine moles of N₂H₄ formed
Given that 0.3987 moles of NH₃ are mixed, we need to find how many moles of N₂H₄ are produced:
0.3987 moles NH₃ × (2 moles N₂H₄ / 4 moles NH₃) = 0.3987 * (2 / 4) moles N₂H₄
0.3987 moles NH₃ → 0.19935 moles N₂H₄
Step 2: Calculate the heat released
Now that we know the number of moles of N₂H₄ formed, we can calculate the quantity of heat released using the enthalpy change (∆H°) given in the reaction.
∆H° = -286 kJ/mol (given)
The heat released can be calculated as follows:
Heat released = ∆H° × moles of N₂H₄ formed
Heat released = -286 kJ/mol × 0.19935 moles N₂H₄
Now, perform the calculation:
Heat released ≈ -56.98 kJ
So, approximately 56.98 kJ of heat will be released in this chemical reaction when 0.3987 moles of NH₃ are mixed with 0.200 mol of O₂.