Suppose 300 g of water at 20°C is poured over a 50-g cube of ice with a temperat

Question

Suppose 300 g of water at 20°C is poured over a 50-g cube of ice with a temperature of -4°C. If all the ice melts, what is the final temperature of the water? If all of the ice does not melt, how much ice remains when the water–ice mixture reaches equilibrium?

Specific heat (c) for Ice: 2.06 kJ/(kg K)

Specific heat (c) for water: 4.19 kJ/(kg K)

Suppose 300 g of water at 20 degree C is poured over a 50-g cube of ice with a temperature of -4 degree C. If all the ice melts, what is the final temperature of the water? If all of the ice does not melt, how much ice remains when the water?ice mixture reaches equilibrium? Specific heat (c) for Ice: 2.06 kJ/(kg K) Specific heat (c) for water: 4.19 kJ/(kg K)

Explanation / Answer

maxm heat required by ice to reach to 0 degrees = ms(t) = (50)(0.1)(4) = 100 cal.........(2)

maxm heat required by ice at 0 degrees to convert to ice at 0 degrees:

mL = 50(80) = 4000 cal.......(3)

maxm heat released by water 300 gm to reach at 0 degrees is ms(t) = (300)(1)(20) = 6000 cal ...(1)

as we see, 1>(2+3)

hence, temp will be >0 degrees.

300(1)(20-t) = 100+4000+50(1)(t)

6000-300t = 4100+50t

t = 190/35 = 5.4 degrees celcius

pl rate lifesaver

Related Questions

Navigate

• Browse (All)
• Browse S
• Subjects

---

---

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