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31 January, 21:05

How much total energy must be absorbed by a 150 g sample of ice at 0.0°C that it melts

AND then warms to 25.0°C? (Break it into steps and add them together, phase change

and temperature change)

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Answers (1)
  1. 31 January, 21:34
    0
    The answer to your question is Qt = 15750 cal

    Explanation:

    Data

    mass = m = 150 g

    Initial temperature = T1 = 0°C

    Final temperature = T2 = 25°C

    Process

    1. - Calculate the Latent heat of fusion

    Latent heat of fusion for water = l = 80 cal/g

    Heat = Q

    Formula

    Q = ml

    Substitution

    Q = (150) (80)

    Simplification and result

    Q = 12000 cal

    2. - Calculate the Specific heat

    Specific heat of water = C = 1 cal/g°C

    Formula

    Q = mCΔT

    Substitution

    Q = (150) (1) (25 - 0)

    Simplification and result

    Q = 3750 cal

    3. - Calculate the total heat

    Qt = 12000 + 3750

    Qt = 15750 cal
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