8.) 2.) A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods.
In an experiment, a 1.0860 g sample of
glutaric acid
(C5H8O4) is
burned completely in a bomb calorimeter. The calorimeter is
surrounded by 1.143×103 g of water.
During the combustion the temperature increases from
21.61 to 24.66 °C. The heat
capacity of water is 4.184 J g-1°C-1.
The heat capacity of the calorimeter was determined in a previous
experiment to be 761.1 J/°C.
Assuming that no energy is lost to the surroundings, calculate the
molar heat of combustion of glutaric acid based on
these data.
C5H8O4(s) +
5O2(g) = 4
H2O(l) + 5 CO2(g) +
Energy
there is no heat loss so we can say that all heat released in combustion is absorbed by water and calorimeter.
heat absorbed by calorimeter = heat capacity of calorimeter change in temperature of calorimeter
= 761.1 ( J/ oC) (24.66 - 21.61)
= 2321.355 J
heat absorbed by water = mass of water heat capacity of water change in temperature of water
= 1.143 103(g) 4.184 ( J K-1 oC-1) ( 24.66 - 21.61)
= 14586.05 J
we know that heat released in the combustion = heat absorbed by water + heat absorbed by calorimeter
= 14586.051 + 2321.355
heat released in the combustion = 16907.406 J
this heat is released by combustion of 1.0860 g of glutaric acid.
convert this weight in mol, molar mass of glutaric acid is 132. so mol = 1.0860/132 = 8.2272 10-3 mol
so heat released by combustion of 8.2272 10-3 mol of glutaric acid. = 16907.406 J
then heat released by 1 mol of glutaric acid = 2055.043 KJ/mol
molar heat of combustion = 2055.043 KJ/mol
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