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The initial temperature of 140 g of ice is −22°C. The specific heat capacity of ice...

The initial temperature of 140 g of ice is −22°C. The specific heat capacity of ice is 0.5 cal/g·C° and waters is 1 cal/g·C°. The latent heat of fusion of water is 80 cal/g.

a. How much heat is required to raise the ice to 0°C?

b. How much additional heat is required to completely melt the ice after it has reached 0°C?

c. How much additional heat is required to heat the water (obtained by melting the ice) to 27°C?

d. What is the total heat that must be added to convert the 140 g of ice at −22°C to water at +27°C?

e. Examine your answers to parts a, b, and c. Which takes the most energy; heating ice to the melting point, melting the ice, or heating the cold water to the final temperature?

f. Can we find this total heat simply by computing how much heat is required to melt the ice and adding the amount of heat required to raise the temperature of 140 g of water by 49°C? Explain.

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genius_generous answered 2 years ago
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