Weather Dynamics: Energy and Water Ch 13

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Presentation transcript:

Weather Dynamics: Energy and Water Ch 13 Weather Dynamics: Energy and Water Ch 13.2 (p427-434) Calculating Specific Heat Capacity

Specific heat capacity Heat of vaporization Heat of fusion Temperatures of the oceans and very large lakes are relatively constant for several reasons: Specific heat capacity Heat of vaporization Heat of fusion We will examine Specific Heat Capacity today.

Specific Heat Capacity The amount of heat required to raise the temperature of 1 gram of a substance by 1°C.

Specific Heat Capacity (c) is the amount of heat (Q) Measured in Joules (J) taken in or given off to change the temperature (ΔT) of one gram of a substance (mass) (m) Measured in grams (g) by one degree Celsius ( °C ).

Specific heat capacity is the number of joules (J) per So… Specific heat capacity is the number of joules (J) per gram times degree celsius. The unit for Specific heat capacity is J/g°C

you can calculate the amount of heat (Q) Using the formula Q = mcΔT you can calculate the amount of heat (Q) required to raise the temperature of a mass of a substance (m) by a given temperature change (ΔT).

Substances and their calculated Specific Heat Capacities Specific Heat Capacity (J/gºC) Water (pure) 4.18 This means that it takes 4.18 Joules of heat energy to raise the temperature of 1 gram of pure water by 1 degree celsius.

Substances and their calculated Specific Heat Capacities SHC (J/gºC) Water (pure) 4.18 Sea water 3.89 Dry air 1.00 Pure water has a higher Specific Heat Capacity than sea water. This means that it takes more energy (joules) to raise the temperature of pure water than it takes to raise the temperature of sea water.

Wet mud 2.51 Ethanol (rubbing alcohol) 2.46 Limestone 0.92 Brick 0.84 Granite 0.79 Lead 0.13 Copper 0.39 Iron 0.45 Aluminum 0.90 Heavy oil 2.1 Ice

1 gram of ethanol when each absorbs 10 Joules of thermal energy. Practice Question Using the formula Q = mcΔT compare the increase in the temperature of 1 gram of water with the increase in the temperature of 1 gram of ethanol when each absorbs 10 Joules of thermal energy.

Solution For water Q = mcΔT 10 J = 1.0 g x 4.18 J x ΔT gºC 10 J = ΔT ΔT = 2.4ºC

For ethanol Q = mcΔT 10 J = 1.0 g x 2.46 J x ΔT gºC 10 J = ΔT 2.46 ºC ΔT = 4.1º C

Paraphrase of the Solution  When1.0 g of water absorbs 10 J of energy, then its temperature increases by 2.4º C.  When 1.0 g of ethanol absorbs 10 J of energy then its temperature increases by 4.1ºC. Therefore, the temperature of ethanol increases more than the temperature of water under the same conditions.