When 305.2 calories of heat are added to 32.02 g of copper (specific heat capacity of 0.0920 cal/g ℃), what is the temperature change?

How much thermal energy (in joules) is required to heat 18.1 g of a metal (specific heat = 0.397 J/g C) from 21.0 C to 40.3 C?

If a 42.0g piece of steel at 75.0 degrees C is placed in 150.0 g of water at 25.5 degrees C, what is the final temperature after thermal equilibrium is reached? The heat capacity of steel is 0.466 J/g degrees C and the heat capacity for water is 4.18 J/g degrees C. Assume that no heat is transferred to the surroundings.

A 90.0 g piece of metal, initially at 98.6°C, is placed into 120.0 g of water initially at 24.3°C. If the final temperature of the water is 34.0°C, what is the specific heat of the metal? (The specific heat of water is 4.184 J/g･°C).