The heat required to convert water is given as the product of the mas and the latent heat. 28.34 kJ heat must be removed from the water to change it into ice.
Heat energy is the product of mass, specific heat capacity, and temperature change. It is given as,
[tex]\rm Q = mc \Delta T[/tex]
Given,
Mass of water = 456 gm
Specific heat capacity = 4.186 J / g K
Temperatutre change = 14.85 K
Substituting values above:
[tex]\begin{aligned} \rm Q &= 456 \times 4.186 \times 14.85\\\\&= 28345.91\;\rm J\\\\&= 28.34\;\rm kJ\end{aligned}[/tex]
Therefore, 28.34 kJ of heat energy should be removed from the water.
Learn more about the heat here:
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