In this problem, we’re being asked to determine the final temperature of both the substances at thermal equilibrium.
Recall that heat can be calculated using the following equation:
q = heat, J
• +q → absorbs heat
• –q → loses heat
m = mass (g)
c = specific heat capacity = J/(g·°C)
ΔT = Tf – Ti = (°C)
Recall that heat always travel from high-temperature object to lower-temperature object.
Based on the given system:
A 31.5 g wafer of pure gold initially at 69.7 oC is submerged into 63.6 g of water at 27.2 oC in an insulated container.
What is the final temperature of both substances at thermal equilibrium?
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 Calorimetry concept. You can view video lessons to learn Calorimetry. Or if you need more Calorimetry practice, you can also practice Calorimetry practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Salsbery's class at WWU.