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How much ice (in grams) would have to melt to lower the temperature of 350 mL...

How much ice (in grams) would have to melt to lower the temperature of 350 mL of water from 26 ∘C to 4 ∘C? (Assume the density of water is 1.0 g/mL.) Express your answer using two significant figures.

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Answer #1

mass of water= volume of water* density of water= 350 ml*1g/ml= 350 gm

specific heat of water= 4.184 J/gm.deg.c

heat to be removed from water in bringing the temperature from 26 deg.c to 4 deg.c= mass* specific heat of water* temperature difference= 350*4.184*(26-4) =32217 joules

during melting of ice, latent heat of fusion is added. heat of fusion of ice= 333.55 J/gm

mass of ice required to be melted= heat to be removed/ latent heat of fusion of ice= 32217/333.55 =96.6 gm

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