To treat a burn on his hand, a person decides to place an ice cube on the burned skin. The mass of the ice cube is 11.4 g, and its initial temperature is − 11.1 ∘ C. The water resulting from the melted ice reaches the temperature of his skin, 28.0 ∘ C. How much heat is absorbed by the ice cube and resulting water? Assume that all of the water remains in the hand.
Specific heat of ice = 2.03 J/goC
Specific heat of water = 4.18 J/goC
Heat of fusion of ice = 334 J/g
Heat absorbed by ice in reaching 0 oC from -11.1 oC = mass of ice x specific heat of ice x temperature difference
= 11.4 g x 2.03 J/goC x (0 - (-11.1))oC
= 257 J
Heat absorbed on ice melting = mass of ice x heat of fusion of ice
= 11.4 g x 334 J/g
= 3808 J
Heat absorbed by water in reaching the temperature from 0 oC to 28.0 oC = mass of water x specific heat of water x temperature difference
= 11.4 g x 4.18 J/goC x (28 - 0)oC
= 1334 J
Hence, the total heat absorbed by ice and water = (257 + 3808 + 1334) J
= 5339 J
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