# 6.9: Heat Capacity and Specific Heat

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If a swimming pool and wading pool, both full of water at the same temperature, were subjected to the same input of heat energy, the wading pool would certainly rise in temperature more quickly than the swimming pool. The heat capacity of an object depends both on its mass and its chemical composition. Because of its much larger mass, the swimming pool of water has a larger heat capacity than the wading pool.

## Heat Capacity and Specific Heat

Different substances respond to heat in different ways. If a metal chair sits in the bright sun on a hot day, it may become quite hot to the touch. An equal mass of water under the same sun exposure will not become nearly as hot. This means that water has a high heat capacity (the amount of heat required to raise the temperature of an object by $$1^\text{o} \text{C}$$). Water is very resistant to changes in temperature, while metals generally are not. The specific heat of a substance is the amount of energy required to raise the temperature of 1 gram of the substance by $$1^\text{o} \text{C}$$. The table below lists the specific heats of some common substances. The symbol for specific heat is $$c_p$$, with the $$p$$ subscript referring to the fact that specific heats are measured at constant pressure. The units for specific heat can either be joules per gram per degree $$\left( \text{J/g}^\text{o} \text{C} \right)$$ or calories per gram per degree $$\left( \text{cal/g}^\text{o} \text{C} \right)$$. This text will use $$\text{J/g}^\text{o} \text{C}$$ for specific heat.

Substance Specific Heat $$\left( \text{J/g}^\text{o} \text{C} \right)$$
Table $$\PageIndex{1}$$: Specific Heats of Some Common Substances
Water (l) 4.18
Water (s) 2.06
Water (g) 1.87
Ammonia (g) 2.09
Ethanol (l) 2.44
Aluminum (s) 0.897
Carbon, graphite (s) 0.709
Copper (s) 0.385
Gold (s) 0.129
Iron (s) 0.449
• Heat capacity is the amount of heat required to raise the temperature of an object by $$1^\text{o} \text{C}$$.
• The specific heat of a substance is the amount of energy required to raise the temperature of 1 gram of the substance by $$1^\text{o} \text{C}$$.