In an insulated vessel, 500 g of ice at -5C is added to 250 g of water at 50.0C.

Question

In an insulated vessel, 500 g of ice at -5C is added to 250 g of water at 50.0C.

(a) What is the final temperature of the system?
(b) How much ice remains when the system reaches equilibrium?

Specific heat for water and ice are Cw = 4186 J/(kg C) and Cice = 2108 J/(kg C), respectively, and latent heat of fusion for water is Lf = 3.33 × 105 J/kg

NOTES:
- If all ice melts OR if no ice melts, please state so
- SI unit for mass is kg; 1 kg = 1000 g

** I have attempted this problem on my own, but I am unsure if the work is correct. Please show your work so I can compare and better understand the problem! thank you! **

Explanation / Answer

(A) heat required to raise temp of ice to 0 deg C,

Q = m C deltaT

Q1 = (0.500)(2108)(0 - (-5)) = 5270 J

heat released by water as cools down to 0d eg C

Q2 = (0.250) (4186)(50 - 0)

Q2 = 52325 J

energy available to melt the ice = Q2 - q1 = 47055 J

Q = m Lf

47055 = m (3.33 x 10^5)

m = 0.141 kg

so all of ice is not melted.

final temp = 0 deg C

(B) ice remains = 0.500kg - 0.141 kg

= 0.359 kg or 359 grams

Related Questions

Navigate

• Browse (All)
• Browse I
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.