HomeworkLib
Question

A piece of solid lead weighing 32.6 g at a temperature of 311 °C is placed...

A piece of solid lead weighing 32.6 g at a temperature of 311 °C is placed in 326 g of liquid lead at a temperature of 367 °C. After a while, the solid melts and a completely liquid sample remains. Calculate the temperature after thermal equilibrium is reached, assuming no heat loss to the surroundings.

The enthalpy of fusion of solid lead is ΔHfus = 4.77 kJ/mol at its melting point of 328 °C, and the molar heat capacities for solid and liquid lead are Csolid = 26.9 J/mol K and Cliquid = 28.6 J/mol K.

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

Do rate if you understood

let the final Equilibrium temperature ET° Heat used in melting of lead 32.6 - 0.157 moles of 32.69 pb - 2012 q=0.15184.12 = 0

0 0
Add a comment
Know the answer?
Add Answer to:
A piece of solid lead weighing 32.6 g at a temperature of 311 °C is placed...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • A piece of solid lead weighing 34.2 g at a temperature of 315 °C is placed...

    A piece of solid lead weighing 34.2 g at a temperature of 315 °C is placed in 342 g of liquid lead at a temperature of 376 °C. After a while, the solid melts and a completely liquid sample remains. Calculate the temperature after thermal equilibrium is reached, assuming no heat loss to the surroundings. The enthalpy of fusion of solid lead is ΔHfus = 4.77 kJ/mol at its melting point of 328 °C, and the molar heat capacities for...

  • A piece of solid cadmium weighing 37.6 g at a temperature of 311 °C is placed...

    A piece of solid cadmium weighing 37.6 g at a temperature of 311 °C is placed in 376 g of liquid cadmium at a temperature of 370 °C. After a while, the solid melts and a completely liquid sample remains. Calculate the temperature after thermal equilibrium is reached, assuming no heat loss to the surroundings. The enthalpy of fusion of solid cadmium is ΔHfus = 6.11 kJ/mol at its melting point of 321 °C, and the molar heat capacities for...

  • For lead, Pb, the heat of fusion at its normal melting point of 328 °C is...

    For lead, Pb, the heat of fusion at its normal melting point of 328 °C is 4.8 kJ/mol. The entropy change when 2.46 moles of solid Pb melts at 328 °C, 1 atm is _______J/K. b. For tin, Sn, the heat of fusion at its normal melting point of 232 °C is 7.1 kJ/mol. The entropy change when 1.73 moles of liquid Sn freezes at 232 °C, 1 atm is ______ J/K.

  • Two 20.0‑g ice cubes at −17.0 °C are placed into 225 g of water at 25.0...

    Two 20.0‑g ice cubes at −17.0 °C are placed into 225 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts. heat capacity of ?2?(?) 37.7 J/(mol⋅K) heat capacity of ?2?(?) 75.3 J/(mol⋅K) enthalpy of fusion of ?2? 6.01 kJ/mol

  • Two 20.0 g ice cubes at −14.0 ∘C are placed into 235 g of water at...

    Two 20.0 g ice cubes at −14.0 ∘C are placed into 235 g of water at 25.0 ∘C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tf, of the water after all the ice melts. heat capacity of H2O(s) 37.7 J/(mol⋅K) heat capacity of H2O(l) 75.3 J/(mol⋅K) enthalpy of fusion of H2O. 6.01 kJ/mol

  • Two 20.0 g ice cubes at -12.0 °C are placed into 215 g of water at...

    Two 20.0 g ice cubes at -12.0 °C are placed into 215 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, T, of the water after all the ice melts. heat capacity of H2O(s) heat capacity of H2O(1) enthalpy of fusion of H,O 37.7 J/(mol-K) 75.3 J/(mol-K) 6.01 kJ/mol Ti =

  • Two 20.0 g ice cubes at −17.0 ∘C−17.0 ∘C are placed into 265 g265 g of...

    Two 20.0 g ice cubes at −17.0 ∘C−17.0 ∘C are placed into 265 g265 g of water at 25.0 ∘C.25.0 ∘C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, ?f,Tf, of the water after all the ice melts. Heat Capacity of H2O(s) 37.7 J/(mol K) Heat Capacity of H2O (l) 75.3 J/(mol K) Enthalpy of Fusion of H2O 6.01 kJ/mol

  • Two 20.0 g ice cubes at -12.0 °C are placed into 215 g of water at...

    Two 20.0 g ice cubes at -12.0 °C are placed into 215 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, T. of the water after all the ice melts. heat capacity of H,O() heat capacity of H,O(1) enthalpy of fusion of H,0 37.7J/(mol-K) 75.3 J/(mol-K) 6.01 kJ/mol Ti = 24.99 "C Incorrect

  • Determine the amount of heat, in kJ, required to heat 16 g of solid Ca at 851C to 1,375 C. Meltin...

    Determine the amount of heat, in kJ, required to heat 16 g of solid Ca at 851C to 1,375 C. Melting Point = 851C Boiling Point = 1487C Molar Heat Capacities: Csolid​ = 26.2 J/mol C C liquid​ = 31.0 J/molC ΔH_fusion​ = 9.33 kJ/mol ΔH_vaporization​ = 162 kJ/mol

  • by Two 20 0g ice cubes at-13.0 ℃ are placed into 205 g of water at...

    by Two 20 0g ice cubes at-13.0 ℃ are placed into 205 g of water at 25.0 ℃ Assuming no transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts heat capacity of H20(s) 37.7J(mol K) heat capacity of H20() 75.3 J(mol K) enthalpy of fusion of H2O 6.01 kJ/mol

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT