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17 April, 15:44

Carl adds a 6.70-gram cube of ice at 0.0°C to cool a glass of juice, As the ice melts, the temperature of the newly melted water rises to 25.4°C. Water's heat of fusion is 334 joules/gram, and its specific heat is 4.186 joules/gram degree Celsius. How many joules of energy did the ice cube gain?

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  1. 17 April, 15:52
    0
    2,950

    joules.

    Explanation:

    The units don't need conversion, and the formula doesn't need changing.

    First, determine the energy required to melt the ice:

    Q = mHf

    Q = 6.70 g * 334

    Q = 2,240 J

    Next, determine the energy needed to raise the temperature of the newly melted water:

    Q = mCΔT

    Q = 6.70 g * 4.186 * (25.4°C - 0.0°C)

    Q = 712 J

    Now, add the energy values. Express the answer to 3 significant figures:

    2,240 J + 712 J = 2,950 J.
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