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5 July, 10:39

An 11.98-gram sample of zinc metal is placed in a hot water bath and warmed to 78.4°C. It is then removed and placed into a Styrofoam cup containing 50.0 mL of room temperature water (T=27.0°C; density = 1.00 g/mL). The water warms to a temperature of 28.1°C. Determine the specific heat capacity of the zinc.

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  1. 5 July, 10:45
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    383.34 J/kg. K

    Explanation:

    From the question,

    Heat lost by zinc = heat gained by water in the Styrofoam cup.

    c'm' (t₁-t₃) = cm (t₃-t₂) ... Equation 1

    Where c' = specific heat capacity of zinc, m' = mass of zinc, t₁ = initial temperature of zinc, t₂ = initial temperature of water in the Styrofoam cup, t₃ = temperature of the mixture

    Make c' the subject of the equation

    c' = cm (t₃-t₂) / m' (t₁-t₃) ... Equation 2

    given: m' = 11.98 g = 0.01198 kg, m = density of water*volume of water = (1*50) = 50 g = 0.05 kg, t₁ = 78.4°C, t₂ = 27°C, t₃ = 28.1°C

    Constant: c = 4200 J/kg. K

    Substitute these values into equation 2

    c' = 0.05*4200 (28.1-27) / [0.01198 * (78.4-28.1) ]

    c' = 231/0.602594

    c' = 383.34 J/kg. K
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