Problem: A 110.-g sample of copper (specific heat capacity = 0.20 J/°C•g) is heated to 82.4°C and then placed in a container of water at 22.3°C. The final temperature of the water and copper is 24.9°C. What is the mass of the water in the container, assuming that all the heat lost by the copper is gained by the water?

🤓 Based on our data, we think this question is relevant for Professor Curtiss' class at AU.

FREE Expert Solution

Gaining heat = +q
Losing heat = - q

Therefore:            qwater = - qcopper

View Complete Written Solution
Problem Details

A 110.-g sample of copper (specific heat capacity = 0.20 J/°C•g) is heated to 82.4°C and then placed in a container of water at 22.3°C. The final temperature of the water and copper is 24.9°C. What is the mass of the water in the container, assuming that all the heat lost by the copper is gained by the water?