After an afternoon party, a small cooler full of ice is dumped onto the hot ground and melts. If the cooler contained 5.00 kg of ice and the temperature of the ground was 43.5 °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. cal energy required:
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
![**Problem Statement:**
After an afternoon party, a small cooler full of ice is dumped onto the hot ground and melts. If the cooler contained 5.00 kg of ice and the temperature of the ground was 43.5 °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.
**Solution Box:**
Energy required: _______ cal
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In this problem, we are asked to calculate the energy needed to melt ice at 0 °C. Given the mass of the ice and the heat of fusion for water, we can use the formula:
\[ \text{Energy required} = \text{mass} \times \text{heat of fusion} \]
Converting the mass of ice from kilograms to grams (since the heat of fusion is in cal/g):
\[ 5.00 \, \text{kg} = 5000 \, \text{g} \]
Thus, the energy required is:
\[ \text{Energy required} = 5000 \, \text{g} \times 80.0 \, \text{cal/g} = 400,000 \, \text{cal} \]
So, the calculation for this problem will conclude that 400,000 calories are required to melt 5.00 kg of ice at 0 °C.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F70d1a455-c159-48a6-a4a3-cd41b63d10e2%2F5ef7dee0-8999-4a2f-a984-72d16563ba6c%2Fzy447t_processed.jpeg&w=3840&q=75)
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