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?

FREE Expert Solution

Gaining heat = +q
Losing heat = - q

Therefore:            qwater = - qcopper

93% (434 ratings)
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?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Thermal Equilibrium concept. You can view video lessons to learn Thermal Equilibrium. Or if you need more Thermal Equilibrium practice, you can also practice Thermal Equilibrium practice problems.

What professor is this problem relevant for?

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

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.