A chunk of silver weighing 18,3 grams and originally at 97.00 °C is droped into

Question

A chunk of silver weighing 18,3 grams and originally at 97.00 °C is droped into an insulated cup containing 83.0 grams of water at 22.65 °C. Assuming that all of the heat is transferred to the water, the final temperature of the water is °C. The following information is given for benzene at 1 atm: T = 80.10°C AHrap(80.10°C) = 393.3 Jg T = 5.50°C AHjus (5.50°C) = 127.4 Jig Specific heat gas = 1.040 J/g °C Specific heat liquid =1.740 J/g °C A 20.80 g sample of liquid benzene is initially at 44.80°C. If the sample is heated at constant pressure (P= 1 atm), 95.80°C. kJ of energy are needed to raise the temperature of the sample to

Explanation / Answer

1.

Heat change = mass * specific heat * change in temperature

And it is assumed that no heat transferred out side.

SO,

18.3 * 0.233 * ( t2 - 97.00 ) + 83.0 * 4.184 * ( t2 - 22.65) = 0

4.264 t2 - 413.6 + 347.3 t2 - 7865.7 = 0

351.6 t2 = 8279.3

t2 = 8279.3 / 351.6

t2 = final temperature = 23.55 0C

2.

q = 20.80 * 1.740 * ( 80.10 - 44.80) + 20.80 * 393.3 + 20.80 * 1.040 * ( 95.80 - 80.10)

q = 9797.8 J

q = 9.80 kJ of heat is needed.

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

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