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How much heat is produced when 500 kg of ammonia is produced according to the following equation: N₂(g) + 3h₂(g) → 2nh₃(g), Δh = -91.8 kj (n=14.0, H=1.00)? I. -1.35 x 10⁶ kj ii. 1.76 x 10³ kj iii. -23.09 kj iv. 1.25 x 10⁶ kj
Accepted Answer
The correct answer is I. -1.35 x 10⁶ kJ. Here's how to solve it:
1. Calculate the moles of ammonia:
- Molar mass of NH₃ = 14.0 g/mol + 3(1.00 g/mol) = 17.0 g/mol
- Moles of NH₃ = (500 kg
1000 g/kg) / 17.0 g/mol = 29,411.76 mol
2. Determine the heat released per mole of ammonia:
- The balanced equation shows that the formation of 2 moles of NH₃ releases -91.8 kJ of heat.
- Therefore, the heat released per mole of NH₃ = -91.8 kJ / 2 mol = -45.9 kJ/mol
3. Calculate the total heat released:
- Total heat released = (moles of NH₃)
(heat released per mole)
- Total heat released = 29,411.76 mol
-45.9 kJ/mol = -1.35 x 10⁶ kJ
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