Ethanol, C2H5OH, burns in oxygen gas by the following reaction. C2H5OH(l) + 3O2(g) → 2CO2(g) +...
Ethanol, C2H5OH, burns in oxygen gas by the following reaction.
C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(g); ΔH = -1235 kJ
How many grams of ethanol would be needed to provide 293 kJ of heat?
Homework Answers
when -1235.0 KJ of heat is involved, 1 mol of C2H5OH is reacting
So,
for -2.93*10^2 KJ, mol of C2H5OH = -2.93*10^2*1/-1235.0 KJ
= 0.2372 mol
Molar mass of C2H5OH,
MM = 2*MM(C) + 6*MM(H) + 1*MM(O)
= 2*12.01 + 6*1.008 + 1*16.0
= 46.068 g/mol
use:
mass of C2H5OH,
m = number of mol * molar mass
= 0.2372 mol * 46.07 g/mol
= 10.93 g
Answer: 10.9 g
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Ethanol,
C2H5OH, burns in oxygen gas by the following
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