Question

I’ve actually had negative caloric content. How much energy, in each of the following units, does your body lose from eating (and therefore melting) 57g of ice? Heat of fusion for water is 6.02 kJ/mol

A. Express in joules

B. Express in kilojoules

C. Express in cal

D. Express in Cal

Answer 1

temperature of body = 37 C

now moles of water = mass/ molar mass of water , molar mass of water = 18

= 57/ 18 = 3.167 moles

total heat of fusion = 3.167 * 6.02 =19.06534 kj

now temperature rises from 0 to 37 C

total heat = mass * specific heat * change in temperature , specific heat = 4.186 , change in temperature = 37 88

57* 4.186 * 37= 8828.274 j

total heat required =19065.34 + 8828.274 =27893.614 j

1. in joules = 27893.614 j

2 . in kilojoules = 27.893614 Kj

3 . in cal = total energy in joule / 4.186 = 27893.614/ 4.186 = 6663.5484 cal

4 .in kcal = 6.66354 Cal

here in this problem i considered that the ice is melt from 0 C to 0 C and then reaches the body temperature of human being.

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