Q#1) If 3.285g of ethanol C2H5OH(l) is burned completely in a bomb calorimeter a
ID: 847847 • Letter: Q
Question
Q#1)
If 3.285g of ethanol C2H5OH(l) is burned completely in a bomb calorimeter at 298.15 K, the heat produced is 97.11kJ.
a)Calculate ?H?combustion for ethanol at 298.15 K. ans is: -1364kJ/mol
b)Calculate ?H?f of ethanol at 298.15 K.
Q#2)
At 298 K, ?H?rxn= 131.28 kJmol?1 for the reaction
C(graphite) +H2O(g)?CO(g)+H2(g), with CP,m= 8.53, 33.58, 29.12, and 28.82 JK?1mol?1 for graphite, H2O(g), CO(g), andH2(g), respectively.
A) Calculate ?H?R at 300?C from this information. Assume that the heat capacities are independent of temperature.
Express your answer to five significant figures and include the appropriate units.
Explanation / Answer
C2H5OH(l) + 3O2(g) --> 2CO2(g) + 3H2O(g)
delta H rxn = -1235 kj
use molar mass to find moles:
(3.285g C2H5OH) (1 mole C2H5OH / 46.07 grams) = 0.0713 moles of C2H5OH
find heat released, using this relationship:
1 mole of C2H5OH(l) + 3O2(g) --> 2CO2(g) + 3H2O(g) & d H rxn = -1235 kj
(0.0713 moles of C2H5OH) (-1235 kj / mole ) = - 88 kJ
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