10.2 Specific Heat Capacity

Match the term with the definition.

• Temperature

• thermal energy transferred from a hottest system to a cooler system

• Heat Capacity

• the amount of heat energy required to raise the temperature of 1 gram of a substance by 1°C.

• Heat

• the amount of heat energy required to raise the temperature of an object by 1°C.

• Joule

• the standard unit of energy

• Specific Heat Capacity

• the measure of the average kinetic energy of the particles in a substance.

Label the formula for specific heat capacity.

a

b

c

d

Temperature change

Energy

Specific heat capacity

Mass

A 200 g sample of water is heated from 20 °C to 60 °C. Calculate the heat energy absorbed by the water in joules
(Specific heat capacity of water = 4.18 J/g°C)

Mathematical Equivalence

ON

Answer explanation

A 500 g sample of a metal absorbs 7500 J of heat and its temperature increases by 15 °C. Calculate the specific heat capacity of the metal in J g^{-1 o}C^-1

Mathematical Equivalence

ON

Answer explanation

A 100 g sample of ethanol (c = 2.4 J/g°C) is heated with 9600 J of energy. If its initial temperature was 25 °C, calculate its final temperature in ^oC

Mathematical Equivalence

ON

Answer explanation

Water has a ​ (a)   specific heat capacity because of the strong (b)   between its molecules. These bonds require extra ​ (c)   to break before the temperature of the water can rise and the molecules move more. As a result, ​ (d)   heat is needed to increase the temperature of water.

• hydrogen bonds
• high
• energy
• more
• dispersion forces
• low
• less