Question

Part A How much ice in grams would have to melt to lower the temperature of 358 mL of water from 15°C to 0 °C? (Assume that the density of water is 1.0 g/mL.) Express your answer using two significant figures. m = 67 8 Previous Answers Answer Requested Return to Acciainment Provide Feedhack

Answer 1

Data required,

Latent heat of fusion = 333 J/g

specific heat of water = 4.18 J/gC

mass of water = density*volume = 1*358 = 358 gram

Now, let the mass of ice that would have to melt = m gram

so, heat absorbed by melting of ice = heat release by water

=> 333*m = 358*4.18*(15-0)

=> m = 67.4 gram

so, the mass of ice that would melt = 67 gram (in two significant figures)

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