Question

An insulated thermos contains 102.0 cm3 of hot coffee at a temperature of 80.0 °C. You...

An insulated thermos contains 102.0 cm3 of hot coffee at a temperature of 80.0 °C. You put in 14.0 g of ice cube at its melting point to cool the coffee. What is the temperature of the coffee once the ice has melted and the system is in thermal equilibrium? Treat the coffee as though it were pure water. (Answer in °C)

Science   Physics   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Lf = specific latent heat of fusion of ice = 334,000J/kg (energy to melt 1kg of ice at 0degC)
Heat supplied to melt ice = m_ice x Lf = 0.0140 x 334000 = 4676J

Final temp = T deg C
Heat lost by coffee cooling from 80degC to T = m.c.delta_T = 0.080 x 4200 x (80 - T)
Heat gained by water from melted ice being raised from 0degC to T = m.c.delta_T
= 0.014 x 4200 x (T - 0)
______________________________________...
Heat lost by cofee = Heat needed to melt ice + Heat needed to rais melted ice from 0degC to T
0.080 x 4200 x (80 - T) = 4676 + 0.014 x 4200 x T

26880-336T=58.8T+4676

394.8T=22204

T=56.24 C

0 0
Know the answer?
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
Similar Questions
An insulated thermos contains 124.0 cm3 of hot coffee at a temperature of 80.0 °C. You...
An insulated thermos contains 124.0 cm3 of hot coffee at a temperature of 80.0 °C. You put in 12.0 g of ice cube at its melting point to cool the coffee. What is the temperature of the coffee once the ice has melted and the system is in thermal equilibrium? Treat the coffee as though it were pure water. (Answer in °C)
An insulated thermos contains 106 cm3 of hot coffee at a temperature of 67.0◦C. You put...
An insulated thermos contains 106 cm3 of hot coffee at a temperature of 67.0◦C. You put in 12.0 g of ice at its melting point to cool the coffee. By how many degrees has your coffee cooled just after all the ice has melted and equilibrium is reached? Treat the coffee as though it were pure water and neglect energy exchanges with the environment.
A thermos contains 153 cm3 of coffee at 89.2 °C. To cool the coffee, you drop...
A thermos contains 153 cm3 of coffee at 89.2 °C. To cool the coffee, you drop two 12.0-g ice cubes into the thermos. The ice cubes are initially at 0 °C and melt completely. What is the final temperature of the coffee in degrees Celsius? Treat the coffee as if it were water.
An insulated Thermos contains 115 g of water at 78.7 ˚C. You put in a 10.0...
An insulated Thermos contains 115 g of water at 78.7 ˚C. You put in a 10.0 g ice cube at 0.00 ˚C to form a system of ice + original water. The specific heat of liquid water is 4190 J/kg•K; and the heat of fusion of water is 333 kJ/kg. What is the net entropy change of the system from then until the system reaches the final (equilibrium) temperature?
An insulated Thermos contains 113 g of water at 77.3 ˚C. You put in a 10.3...
An insulated Thermos contains 113 g of water at 77.3 ˚C. You put in a 10.3 g ice cube at 0.00 ˚C to form a system of ice + original water. The specific heat of liquid water is 4190 J/kg•K; and the heat of fusion of water is 333 kJ/kg. What is the net entropy change of the system from then until the system reaches the final (equilibrium) temperature?
An insulated Thermos contains 119 g of water at 75.1 ˚C. You put in a 9.16...
An insulated Thermos contains 119 g of water at 75.1 ˚C. You put in a 9.16 g ice cube at 0.00 ˚C to form a system of ice + original water. The specific heat of liquid water is 4190 J/kg•K; and the heat of fusion of water is 333 kJ/kg. What is the net entropy change of the system from then until the system reaches the final (equilibrium) temperature?
An 11 g ice cube at -12˚C is put into a Thermos flask containing 145 cm3...
An 11 g ice cube at -12˚C is put into a Thermos flask containing 145 cm3 of water at 24˚C. By how much has the entropy of the cube-water system changed when a final equilibrium state is reached? The specific heat of ice is 2200 J/kg K and that of liquid water is 4187 J/kg K. The heat of fusion of water is 333 × 103 J/kg. and A 6.0 g ice cube at -21˚C is put into a Thermos...
An 10 g ice cube at -13˚C is put into a Thermos flask containing 115 cm3...
An 10 g ice cube at -13˚C is put into a Thermos flask containing 115 cm3 of water at 20˚C. By how much has the entropy of the cube-water system changed when a final equilibrium state is reached? The specific heat of ice is 2200 J/kg K and that of liquid water is 4187 J/kg K. The heat of fusion of water is 333 × 103 J/kg.
Your 300 mL cup of coffee is too hot to drink when served at 90°C. An...
Your 300 mL cup of coffee is too hot to drink when served at 90°C. An ice cube, taken from a −20°C freezer is used to cool your coffee to a pleasant 60°C. Assume that you have a well-insulated cup. a. Provide the statement of energy conservation for this closed “coffee-ice” system. b. What is the heat lost by coffee in bringing down the temperature to 60°C? c. How much heat is consumed in converting ice to water at 0°C?...
You decide to put a 40.0 g ice cube at -10.0°C into a well insulated coffee...
You decide to put a 40.0 g ice cube at -10.0°C into a well insulated coffee cup (of negligible heat capacity) containing  of water at 5.0°C. When equilibrium is reached, how much of the ice will have melted? The specific heat of ice is 2090 J/kg ∙ K, that of water is 4186 J/kg ∙ K, and the latent heat of fusion of water is 33.5 × 104 J/kg.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT