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A piece of nickel weighing 2.40 g is heated to 200.0°C, and is then dropped into 10.0mL of water at 15.0°C. The temperature of the metal falls and that of the water rises until thermal equilibrium is attained and both are 18.0°C. What is the specific heat of the metal?​

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Answer:

0.287 J K–1 g–1

Explanation:

The mass of the water is (10 mL) × (1.00 g mL–1) = 10 g. The specific heat of water is 4.18 1 J K–1 g–1 and its temperature increased by 3.0 C°, indicating that it absorbed (10 g)(3 K)(4.18 J K–1 g–1) = 125 J of energy. The metal sample lost this same quantity of energy, undergoing a temperature drop of 182 C° as the result. The specific heat capacity of the metal is:

(125 J) / (2.40 g)(182 K) = 0.287 J K–1 g–1.

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