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How much ice (in grams) would have to melt to lower the temperature of 355 mL...

How much ice (in grams) would have to melt to lower the temperature of 355 mL of water from 26 ∘C to 5 ∘C? (You must consider the enthalpy in cooling the water, as well as the enthalpy in melting the ice and the enthalpy to heat the melted ice from 0∘C up to the system's final temperature of 5 ∘C. Also assume that 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 * density

                        = 355*1 = 355g

         q            = mcT

                     = 355*4.184*(5-26)   = -31191.72J

                    = 31191.72J/334J/g   = 93.4g of ice

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