|Exercise: Thermal Chemistry||
Heat = q = mCT; C = the heat capacity of a substance
1. How much heat will it take to raise the temperature of a 15.0 g gold bracelet from 16.1 °C to 49.3 °C? Assume a constant heat capacity of 25.4 J °C-1mol-1 over this temperature range.
2. A 0.95 kg cast iron pan is heated from room temperature (20.0 °C) to 125.0 °C on a gas stove. Assuming the heat capacity of the pan remains constant over this temperature range, calculate the quantity of heat absorbed by the pan ( heat capacity of Fe = 25.1 J °C-1mol-1).
3. What is the heat capacity of a calorimeter that contains 125.0 g of water, if it took 40.0 kJ to raise the temperature of the calorimeter and the water 14.00 °C? (The heat capacity of water is 4.184 Jg-1°C-1)
The problems below are longer and more difficult than would appear on a quiz, but good practice if you wish to attempt them.
4. A 75.0 g bar of copper metal at 128.2 °C is dropped into a liter of cool water in an insulated container where its temperature drops to 24.1 °C, in equilibrium with the water. Assuming all of the heat goes to heat up the water (the container has a heat capacity of zero), what was the initial temperature of the water? (The molar heat capacity of copper is 24.4 Jmol-1°C-1, the heat capacity of water is 4.184 Jg-1°C-1.)
5. A 0.828 g sample of methanol is completely combusted in a bomb calorimeter with excess oxygen. The calorimeter contains 1.35 kg of water and the instrument has a heat capacity of 1.06 kJ °C-1 without water. Combustion of the methanol increases the temperature of the calorimeter increases from 23.10 to 25.90°C. Find the molar heat of combustion of methanol (heat released in burning one mole of methanol).
© R A Paselk
Last modified 2 October 2009