Question

A piece of solid lead weighing 45.3 g at a temperature of 308 °C is placed...

A piece of solid lead weighing 45.3 g at a temperature of 308 °C is placed in 453 g of liquid lead at a temperature of 374 °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.

Tfinal = ______ °C

Homework Answers

Answer #1

Heat lost by liquid water = Heat gained by solid lead

Heat lost by water = Mass of liquid lead * specific heat capacity of liquid * Change in temperature

=> 453g * 28.6 J/gC * (374-Tf)

Heat gained by water = Heat required to convert lead from 308C to 328C + Heat required to convert solid lead at 328C to liquid lead at 328C + Heat required to raise the temperature of liquid from 328 to Tf

=> 45.3g * 26.9 J/gC * (328-308)C + 4770 J/mol * 45.3/207.2 mol + 45.3g * 28.6 J/gC * (Tf - 328)

Equating both these equations to calculate the value of Tf

453 * 28.6 * (374-Tf) = 45.3 * 26.9 * 20 + 4770 * 45.3/207.2 + 45.3 * 28.6 * (Tf-328)

Hence the value of Tf will be 368.03C

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A piece of solid lead weighing 43.2 g at a temperature of 314 °C is placed...
A piece of solid lead weighing 43.2 g at a temperature of 314 °C is placed in 432 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...
A piece of solid antimony weighing 34.3 g at a temperature of 618 °C is placed...
A piece of solid antimony weighing 34.3 g at a temperature of 618 °C is placed in 343 g of liquid antimony at a temperature of 754 °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 antimony is ΔHfus = 19.6 kJ/mol at its melting point of 631 °C, and the molar heat capacities for...
Use the following information on Al to determine the amounts of heat for the three heating...
Use the following information on Al to determine the amounts of heat for the three heating steps required to convert 150.0 g of solid Al at 458oC into liquid Al at 758oC. mp = 658 oC bp = 2467 o C Molar Heat Capacities Csolid = 24.3 J/moloC Cliquid = 29.3 J/mol oC ΔHfusion = 10.6 kJ/mol ΔHvaporization = 284 kJ/mol
Sulfur dioxide is produced in enormous amounts for sulfuric acid production. It melts at −73°C and...
Sulfur dioxide is produced in enormous amounts for sulfuric acid production. It melts at −73°C and boils at −10°C. Its ΔH°fus is 8.619 kJ/mol and its ΔH°vap is 25.73 kJ/mol. The specific heat capacities of the liquid and gas are 0.995 J/g · K and 0.622 J/g · K, respectively. How much heat is required to convert 2.585 kg of solid SO2 at the melting point to a gas at 60°C?
Ethanol, C2H5OH, (MW 46.06 g/mol) melts at -114 °C. The enthalpy of fusion is 5.02 kJ/mol....
Ethanol, C2H5OH, (MW 46.06 g/mol) melts at -114 °C. The enthalpy of fusion is 5.02 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g-K and 2.3 J/g-K, respectively. How much heat (kJ) is needed to convert 20.0 g of solid ethanol at -135 °C to liquid ethanol at -50 °C? please show work
A 12.30-g block of solid gold at 63.62 °C is immersed in a 23.29-g pool of...
A 12.30-g block of solid gold at 63.62 °C is immersed in a 23.29-g pool of liquid ethanol with a temperature of 12.25 °C. When thermal equilibrium is reached, what is the temperature of the gold and ethanol? Specific heat capacities: gold = 0.129 J/g °C; ethanol = 2.44 J/g °C ________°C
Information about Acetone (C3H6O) : Boiling Point= 56.1 C Melting Point= -94.7 C Heat of Vaporization=...
Information about Acetone (C3H6O) : Boiling Point= 56.1 C Melting Point= -94.7 C Heat of Vaporization= 31.3 kj/mol Heat of Fusion= 5.71 kj/mol Specific Heat Capacities: Csolid= 1.60 J/g*K Cliquid= 2.20 J/g*K Cgas= 1.30 J/g*K a) Draw a heating curve that starts at -50 C and goes to +100 C. Take into account that since the specific heats are different, the heating rates will also differ. b) What is the total energy change of a process in which 18.4 grams...
A 10.54-g block of solid tin at 14.65 °C is immersed in a 21.35-g pool of...
A 10.54-g block of solid tin at 14.65 °C is immersed in a 21.35-g pool of liquid ethylene glycol with a temperature of 61.51 °C. When thermal equilibrium is reached, what is the temperature of the tin and ethylene glycol? Specific heat capacities: tin = 0.213 J/g °C; ethylene glycol = 2.36 J/g °C
Two 20.0-g ice cubes at –20.0 °C are placed into 285 g of water at 25.0...
Two 20.0-g ice cubes at –20.0 °C are placed into 285 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) is 37.7 J/mol*K heat capacity of H2O(l) is 75.3 J/mol*K enthalpy of fusion of H20 is 6.01 kJ/mol
Two 20.0-g ice cubes at –13.0 °C are placed into 275 g of water at 25.0...
Two 20.0-g ice cubes at –13.0 °C are placed into 275 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 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
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT