Heat & Specific Heat

Q = m C ∆T

Q = m ∆T

Q = C m T

Q = m C T

30,000 J

34,700 J

40,000 J

25,500 J

2.09 J/g°C

4.18 J/g°C

1.00 J/g°C

3.50 J/g°C

As temperature increases, thermal energy decreases.

As temperature increases, thermal energy remains constant.

As temperature increases, thermal energy increases.

There is no relationship between temperature and thermal energy.

0.5 °C

1.0 °C

1.2 °C

2.0 °C

J/g°C

cal/g°C

kJ/kg·K

J/kg·°F

It requires more energy to change temperature.

It changes temperature quickly with little energy.

It has a low capacity for storing heat.

It can easily evaporate at low temperatures.

The energy stored in chemical bonds of a substance.

The total kinetic energy of particles in a substance.

The energy associated with the motion of an object.

The energy released during a phase change.

The total heat energy in joules.

The mass of the substance in kilograms.

The change in temperature in degrees Celsius.

The specific heat capacity in joules per kilogram per degree Celsius.

The volume of the substance in liters.

The mass of the substance in grams.

The temperature change in Celsius.

The specific heat capacity of the substance.