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29 January, 16:00

Calculate the amount of energy, in Joules, required to raise the temperature of 15.5 g of liquid water from 0.00o C to 75.0 oC.

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  1. 29 January, 17:07
    0
    10043.225 J

    Explanation:

    We'll begin by calculating the amount of heat needed to change ice to water since water at 0°C is ice. This is illustrated below:

    Mass (m) = 15.5g

    Latent heat of fussion of water (L) = 334J/g

    Heat (Q1) = ... ?

    Q1 = mL

    Q1 = 15.5 x 334

    Q1 = 5177 J

    Next, we shall calculate the amount of heat needed to raise the temperature of water from 0°C to 75°C.

    This is illustrated below:

    Mass = 15.5g

    Initial temperature (T1) = 0°C

    Final temperature (T2) = 75°C

    Change in temperature (ΔT) = T2 - T1 = 75 - 0 = 75°C

    Specific heat capacity (C) of water = 4.186J/g°C

    Heat (Q2) = ?

    Q2 = MCΔT

    Q2 = 15.5 x 4.186 x 75

    Q2 = 4866.225 J

    The overall heat energy needed is given by:

    QT = Q1 + Q2

    QT = 5177 + 4866.225

    QT = 10043.225 J

    Therefore, the amount of energy required is 10043.225 J
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