We’re being asked to calculate the amount of energy required to melt 5.60 kg of ice at 0 ˚C. The problem is not asking us to calculate the heat needed to change the temperature of ice, which means we don’t need the given temperature of 43 ˚C.
Recall that during a phase transition, the temperature is constant. The amount of energy (q) needed to melt a given mass is calculated using:
where m = mass (in g), ΔHfusion = heat of fusion (in cal/g). Note that calorie (cal) is just another unit of energy similar to Joules (J) and 1 cal = 4.184 J.
After an afternoon party, a small cooler full of ice is dumped onto the hot ground and melts. If the cooler contained 5.60 kg of ice and the temperature of the ground was 43.0°C, calculate the energy that is required to melt all the ice at 0°C. The heat of fusion for water is 80.0 cal/g.
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Heating and Cooling Curves concept. You can view video lessons to learn Heating and Cooling Curves. Or if you need more Heating and Cooling Curves practice, you can also practice Heating and Cooling Curves practice problems.
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Based on our data, we think this problem is relevant for Professor McCarty's class at NCSU.