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You add 50.0 g of ice initially at ‒20.0 °C to 1.00 x 102 mL warm...

You add 50.0 g of ice initially at ‒20.0 °C to 1.00 x 102 mL warm water at 67.0 °C. When all the ice melts, the water temperature is found to be somewhere above 0 °C. Calculate the final temperature of the water.

[ Cice = 2.06 J/g⋅°C; CH2O = 4.184 J/g⋅°C; dH2O = 1.00 g/mL; heat of fusion of water = 333 J/g ]

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Answer #1

Formulas used: Heat change in same phase = msΔT (ΔT is change in temperature, s = specific heat)

Heat change during phase change = mL (L= heat of fusiom / heat of vaporization)

Mass (m) = density*volume

Therefore, final temperature of water = 14.850C

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