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Calculate the energy required to heat a beaker of water at 23°C to boiling. The mass of the water is 68.9 g.
Determine the temperature change that will occur when 269 J of energy is applied to 24.7 g of gold.
A silver ring has a mass of 137.62 g. How many calories of heat are required to increase the temperature from 13.4°C to 173.6°C?
What is the mass of copper that increases its temperature by 312°C when 186,000 J of energy is applied?
A 278.96 g ingot of unknown metal is heated from 22.89°C to 267.29°C. This requires 3.91 kcal of energy. Calculate the specific heat of the metal and determine its identity.

Here's the table to help you find the answer.

Substance

Specific Heat Capacity

(J/g°C)

Water:4.184 (J/g°C)

Aluminum:0.89 (J/g°C)

Silicon:0.703 (J/g°C)

Iron:0.45 (J/g°C)

Copper:0.387 (J/g°C)

Silver:0.24 (J/g°C)

Gold:0.129 (J/g°C)

Lead:0.128 (J/g°C)