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13 January, 04:56

A sample of nickel is heated to 99.8C and placed in a coffeecup calorimeter containing 150.0 g water at 23.5C. After the metal cools, the final temperature of metal and water mixture is 25.0C. 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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  1. 13 January, 04:59
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    The mass of the nickel sample is 28.35 °C

    Explanation:

    Step 1: Data given

    Mass of water = 150 grams

    Initial temperature of nickel = 99.9 °C

    Initial temperature of water 23.5 °C

    Final temperature of water and nickel = 25 °C

    Specific heat capacity of nickel = 0.444 J/g°C

    Specific heat capacity of water = 4.184 J/g°C

    Step 2: Calculate mass of nickel

    heat lost by nickel = heat gained by the water

    Q = m*c*ΔT

    Qnickel = - Qwater

    m (nickel) * c (nickel) * ΔT (nickel) = - m (water) * c (water) * ΔT (water)

    m (nickel) * 0.444 J/g°C * (25°C - 99.8°C) = - 150 grams * 4.184 J/g°C * (25-23.5)

    m (nickel) * (-33.2112) = - 941.4

    m (nickel) = - 941.4 / - 33.2112

    m (nickel) = 28.35 °C

    The mass of the nickel sample is 28.35 °C
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