We’re being asked to determine the identity of the unknown substance in the given system.
Recall that heat (q) 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)
Based on the given system:
A hot lump of 106.2 g of an unknown substance initially at 153.2°C is placed in 35.0 mL of water initially at 25.0°C and allowed to reach thermal equilibrium. The final temperature of the system is 53.2°C. What is the identity of the unknown substance? Assume no heat is lost to the surroundings.
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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.
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Based on our data, we think this problem is relevant for Professor Giles' class at VCU.