our camp fuel has an energy density of 50 kJ/g. Assuming perfect efficiency how much fuel does it take to melt 500 grams of ice starting at -10˚C and then raise it just to 100 degrees (but not boil it dry)? How much fuel do you save if the water started out as a liquid at 0˚C instead of ice at -10˚C?

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Your camp fuel has an energy density of 50 kJ/g. Assuming perfect efficiency how much fuel does it take to melt 500 grams of ice starting at -10˚C and then raise it just to 100 degrees (but not boil it dry)? How much fuel do you save if the water started out as a liquid at 0˚C instead of ice at -10˚C?

Expert Solution
Step 1

This is the question of thermodynamics.

While converting ice to water three types of heat energy are required.

1. Heat required to bring temperature of ice from -10 to 0 deg. C

2. Latent heat of fusion to convert ice of 0 deg C to water of 0 deg. C

3. Heat required to raise temp. of water from 0 to 100 deg. C

Refer attached solution :

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