16.0 g copper pan at 200.0∘C is plunged into 200.0 mL of water at 25.0∘C causing the water to rise to 67.0∘C. What is the specific heat of the copper?

16.52 J/g°C is the specific heat of the copper.

Explanation:

Mass of water = m

Volume of water = V = 200.0 mL

Density of water = d = 1.0 g/mL

Specific heat of water = c = 4.184 J/g°C

Initial temperature of the water = = 25.0°C

Final temperature of the water = = 67.0°C

Heat absorbed by water = Q

Mass of copper pan  = M = 16.0 g

Specific heat of copper = c' = ?

Initial temperature of the copper pan= = 200.0 °C

Final temperature of the copper pan= = 67.0°C

Heat lost by copper pan  = Q'

Q= -Q' ( law of conservation of energy)

16.52 J/g°C is the specific heat of the copper.

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