# Problem: 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.

###### FREE Expert Solution

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 decreasedlost 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

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###### Problem Details

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.