Asked Nov 10, 2019

Given the equation below, what is ΔH for burning 13.0 g of C2H5OH (g) in excess oxygen?
C2H5OH (l) + 3 O2 (g) → 2 CO2 (g) + 3 H2O (l) ΔH = -1370 kJ


Expert Answer

Step 1

According to the chemical equation, when one mole of ethanol is burned, -1370 kJ of energy is realised.

С,Н.ОН (1) +30, (8) —>2с0, (8) + зн,о (1). дн
-1370 kJ

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С,Н.ОН (1) +30, (8) —>2с0, (8) + зн,о (1). дн -1370 kJ

Step 2

The number of moles in 13 g of ethanol (C2H5OH) is calculated as in equation (1) where n, w, and M is the number of moles, mass, and molar ...

n =
13 g
46.07 g mol
= 0.282 mol

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...(1) n = 13 g 46.07 g mol = 0.282 mol


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Chemical Thermodynamics

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