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Yesterday, 19:54

A 2.575 g piece of gold (specific heat = 0.129 J/g°C) at a temperature of 75°C is placed into cold water at 10°C. If the gold loses 10.0 J of energy, what is its final

temperature in the water? Enter your answer to the

nearest whole number of °C.

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Answers (1)
  1. Yesterday, 20:01
    0
    The final temperature of the mixture is 44.9°C

    Explanation:

    Mass of the substance (gold) = 2.575g

    Specific heat capacity of gold = 0.129J/g°C

    Initial temperature (T1) = 75°C

    Final temperature (T2) = ?

    Energy lost = 10J

    Heat energy (Q) = MC∇T

    Q = heat energy (in this case lost)

    M = mass of the substance

    C = specific heat capacity of the substance

    ∇T = change in temperature of the substance = (T2 - T1)

    Q = MC∇T

    Q = MC (T2 - T1)

    -10 = 2.575 * 0.129 * (T2 - 75) energy is - ve because it was energy lost.

    -10 = 0.3321 * (T2 - 75)

    -10 = 0.3321T2 - 24.9075

    Collect like terms

    0.3321T2 = 24.9075 - 10

    0.3321T2 = 14.9075

    T2 = 14.9075 / 0.3321

    T2 = 44.88

    T2 = 44.9°C

    The final temperature of the mixture is 44.9°C
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