In the following reaction, how many moles of CH₃OH are required to produce -1.501 × 10³ kJ of heat?
2 CH₃OH (l) + 3 O₂ (g) → 2 CO₂ (g) + 4 H₂O(g) ∆H° = -1280. kJ
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Given:
- The amount of heat required is equal to 1501 kJ
- Two moles of CH₃OH produces 1280 kJ of heat.
To find:
The number of moles of CH₃OH required to produce 1501 KJ of heat.
Solution:
- Its given that two moles of CH₃OH produces 1280 kJ of heat, hence one mole of CH₃OH will produce 640 KJ of heat.
- So, the number of moles of CH₃OH required will be equal to (1501/640) = 2.345 moles.
Answer:
The number of moles of CH₃OH required to produce 1501 KJ of heat is equal to 2.345
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