Ethanol can undergo decomposition to form two sets of products:
C₂H₅OH(g) → C₂H₄(g) + H₂O(g); ΔH = +50.0 kJ
CH₃CHO(g) + H₂O(g); ΔH = +86.0 kJ
If the molar ratio of C₂H₄(g) to CH₃CHO(g) in the product is 3:1, the heat absorbed in decomposition of 2.0 mole of ethanol(g) (in kJ) is

Question

Ethanol can undergo decomposition to form two sets of products:

C₂H₅OH(g) → C₂H₄(g) + H₂O(g); ΔH = +50.0 kJ

CH₃CHO(g) + H₂O(g); ΔH = +86.0 kJ

If the molar ratio of C₂H₄(g) to CH₃CHO(g) in the product is 3:1, the heat absorbed in decomposition of 2.0 mole of ethanol(g) (in kJ) is

TestHub · Accepted Answer

For every 4 mol of ethanol decomposed, the heat absorbed is calculated as 3 × 50 + 1 × 86 = 236 kJ. This means 59 kJ/mol of ethanol.

Therefore, for 2.0 mol of ethanol, the total heat absorbed is 2.0 × 59 = 118 kJ.

Answer: 0118.

Chemistry - Thermochemistry Question with Solution | TestHub