The total heat that is involved in this change is 23632.5 J.
<h3>What is the energy involved?</h3>
We know that energy is involved as matter is changing from one state to another and in this case what we have is a 75g sample of liquid water at 10°C ends up as ice at -10°C.
There are are about three steps of the change in the energy;
1) Heat required until the water would change to ice
2) Latent heat of fusion of ice
3) Heat required until the temperature drops to -10°C
Thus;
1) H = mcdT
m = mass of the water
c = specific heat capacity of water
dT = temperature change
H = 75 * 4.18 * (0 - 10)
H = -3135 J
2) Heat of fusion =
H = mL
m = mass of ice
L = latent heat of fusion of ice
336 J g^-1 * 75g
= 25200 J
3) Heat required to decrease the temperature futher
H = 75 * 2.09 * (0 - (-10))
H = 1567.5J
Total heat required = 25200 J + 1567.5J -3135 J
= 23632.5 J
Learn more about heat:brainly.com/question/28302909
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