Ethanol can undergo decomposition to form two sets of products:
C₂H₅OH(g) → C₂H₄(g) + H₂O(g); ΔH = +45.0 kJ
CH₃CHO(g) + H₂O(g); ΔH = +72.0 kJ
If the molar ratio of C₂H₄(g) to CH₃CHO(g) in the product is 8:1, the heat absorbed in decomposition of 2.5 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 = +45.0 kJ

CH₃CHO(g) + H₂O(g); ΔH = +72.0 kJ

If the molar ratio of C₂H₄(g) to CH₃CHO(g) in the product is 8:1, the heat absorbed in decomposition of 2.5 mole of ethanol(g) (in kJ) is

TestHub · Accepted Answer

For every 9 mol of ethanol decomposed, the total heat absorbed is calculated as:

(8 × 45) + (1 × 72) = 360 + 72 = 432 kJ

This means the heat absorbed per mole of ethanol is 432 kJ / 9 mol = 48 kJ/mol.

Therefore, for 2.5 mol of ethanol, the heat absorbed is:

2.5 mol × 48 kJ/mol = 120 kJ

The answer is 0120.

Chemistry - Thermochemistry Question with Solution | TestHub