Calorimetry is the measurement
of heat changes of physical and chemical processes. In the laboratory, these
processes are measured in a calorimeter. The Triptik for thermochemistry at
http://www.chem.vt.edu/RVGS/ACT/notes/Chap_8_Triptik.html
contains two examples of calorimeters. Make sketches of each, and then answer
the following.
How does
a bomb calorimeter differ from a simple coffee cup calorimeter?
A quantity of 2.896
g of methanol (CH3OH) was burned in a constant-volume bomb
calorimeter. Consequently, the temperature of the water rose by 6.33°C.
If the quantity of water surrounding the calorimeter was exactly 1900
g and the heat capacity of the calorimeter was 2.56 kJ/°C, calculate
the molar heat of combustion of methanol.
The Chemistry Tutor
provides help on a variety of topics such as chemical reactions, mole/gram
conversions, equations, ideal gas laws, and lab safety. Study the information
given about combustion reactions at http://tqd.advanced.org/2923/react2.html,
and answer the following questions.
Is combustion an
exothermic or endothermic reaction?
Why do you think
these reactions occur mostly in automobiles, homes, and factories?
What would you need
and do to determine the enthalpy change of a specific combustion reaction?
Calculate the work
done by carbon dioxide if it expands from 3.50 mL to 60.0 mL against a
constant pressure of 3.30 atm.
