Based on the given system:
• The nickel sample and water are in thermal equilibrium:
▪ final temperature silver block = final temperature of water = final temperature of the system
Tf silver = Tf water = 25.0°C
• The nickel has an initial temperature of 99.8°C and a final temperature of 25.0°C.
▪ the temperature of the nickel sample decreased → lost heat → – q
• The system is in an insulated container, meaning no heat is lost to the surroundings
▪ the heat lost by the silver block is absorbed by water
▪ heat is absorbed by water → + q
A sample of nickel is heated to 99.8°C and placed in a coffeecup calorimeter containing 150.0 g water at 23.5°C. After the metal cools, the final temperature of metal and water mixture is 25.0°C. If the specific heat capacity of nickel is 0.444 J/°C ? g, what mass of nickel was originally heated? Assume no heat loss to the surroundings.
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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 Constant-Pressure Calorimetry concept. You can view video lessons to learn Constant-Pressure Calorimetry. Or if you need more Constant-Pressure Calorimetry practice, you can also practice Constant-Pressure Calorimetry practice problems.
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Based on our data, we think this problem is relevant for Professor Choudhury's class at BC.
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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.