Suppose 9.00 ? 10 5 J of energy are transferred to 1.73 kg of ice at 0°C. The la

Question

Suppose 9.00 ? 105 J of energy are transferred to 1.73 kg of ice at 0°C. The latent heat of fusion and specific heat of water are Lf = 3.33 ? 105 J/kg and c = 4186

(a) Calculate the energy (in J) required to melt all the ice into liquid water. (Enter your answer to at least three significant figures.)

J

(b) How much energy (in J) remains to raise the temperature of the liquid water? (Enter your answer to at least three significant figures.)

J

(c) Determine the final temperature of the liquid water in Celsius.

°C

Explanation / Answer

Part A

Energy required to melt the ice is given by

Q1 = m*Lf

m = 1.73 kg & Lf = 3.33*10^5 J/kg

Q1 = 1.74*3.33*10^5 = 579420 J = 5.79*10^5 J

Part B

Energy remained = 9*10^5 - 5.79*10^5 = 3.21*10^5 J

Part C

Temperature increased by energy remained will be

Q2 = m*C*dT1

Suppose final temperature is T, then

dT1 = T - 0 = T

T = Q2/(m*C)

T = 3.21*10^5/(1.73*4186)

T = 44.3 C

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