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21 April, 20:40

g An ice cube has a mass of 54 g and is initially at a temperature of 0°C. The ice cube is heated until 47.4 g has become water at 100°C and 6.6 g has become steam at 100°C. How much energy (in kJ) was transferred to the ice cube to accomplish the transformation?

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  1. 21 April, 20:49
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    55536.6 J

    Explanation:

    Given:

    Mass of the ice = 54g

    Initial temperature = 0°C

    Final Temperature = 100°C

    Mass of the steam = 6.6g

    Now the energy required for the transformation of the ice to vapor will involve the heat requirement in the following stages as:

    1) The energy required to melt ice = mass of ice * heat of fusion of water = 54g * 334 J/g = 18036 J

    (because heat of fusion for water = 334 J/g)

    2) The energy to heat water from 0 to 100 = mass of water * specific heat of water * change in temperature = 54g * 4.186 J/g°C * 100 °C = 22604.4 J

    lastly,

    3) the energy required to vaporize 6.6g of water = mass of water * heat of vaporization of water = 6.6 * 2257 J/g = 14896.2 J

    Thus,

    the total energy required to transform the ice cube to accomplish the transformation = 18036 + 22604.4 + 14896.2 = 55536.6 J.
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