Chemistry 2e - Chapter 5 - Thermochemistry

A burning match and a bonfire may have the same temperature, yet you would not sit around a burning match on a fall evening to stay warm. Why not?

Prepare a table identifying several energy transitions that take place during the typical operation of an automobile.

Explain the difference between heat capacity and specific heat of a substance.

Calculate the heat capacity, in joules and in calories per degree, of the following: (a) 28.4 g of water (b) 1.00 oz of lead

Calculate the heat capacity, in joules and in calories per degree, of the following: (a) 45.8 g of nitrogen gas (b) 1.00 pound of aluminum metal

How much heat, in joules and in calories, must be added to a 75.0–g iron block with a specific heat of 0.449 J/g °C to increase its temperature from 25 °C to its melting temperature of 1535 °C?

How much heat, in joules and in calories, is required to heat a 28.4-g (1-oz) ice cube from −23.0 °C to −1.0 °C?

How much would the temperature of 275 g of water increase if 36.5 kJ of heat were added?

If 14.5 kJ of heat were added to 485 g of liquid water, how much would its temperature increase?

A piece of unknown substance weighs 44.7 g and requires 2110 J to increase its temperature from 23.2 °C to 89.6 °C. (a) What is the specific heat of the substance? (b) If it is one of the substances found in [Table 5.1], what is its likely identity?