A 77.5 g sample of an unknown solid is heated to 62.5°C and placed into a calorimeter containing 93 g of water at 23.3°C. If the final temperature of the solid sample and the water is 26.2°C, what is the specific heat of the solid? Assuming no heat loss.

Specific heat of solid is 0.401J/g°C

Explanation:

In this experiment, the heat losed for the unknown solid is equal to heat gained for the water.

Using calorimeter equation:

Q = m*C*ΔT

Where Q is heat, m is mass of substance, C is specific heat and ΔT is change in temperature.

It is possible to write:

m[Solid] * C[Solid] * ΔT[Solid] = m[Water] * C[Water] * ΔT[Water]

Replacing:

77.5g * C[Solid] * (62.5°C - 26.2°C) = 93g * 4.184J/g°C * (26.2°C - 23.3°C)

77.5g * C[Solid] * (62.5°C - 26.2°C) = 93g * 4.184J/g°C * (26.2°C - 23.3°C)

2813.25g°C * C[Solid] = 1128.4J

C[Solid] = 0.401 J/g°C

Specific heat of solid is 0.401J/g°C