Question

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.

Science   Physics   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

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.
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)
Three 100. g ice cubes are dropped in 750. grams of water (at 70.00 C) in...
Three 100. g ice cubes are dropped in 750. grams of water (at 70.00 C) in a Styrofoam cup. If the ice cubes were initially at -150C, how much energy is necessary to warm and melt the ice cubes? Will the ice cubes melt?                                  Cice = 0.53 cal/g*OC                Lf = 79.5 cal/g What is the final temperature of the system?
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 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.
You want to cool 0.2 kg of coffee, initially at temperature Th = 80° C, with...
You want to cool 0.2 kg of coffee, initially at temperature Th = 80° C, with ice initially at Tc = 0° C. The specific heat of ice is about 2108 J/kg K, and its latent heat of melting is about 334, 000 J/kg. You may take the specific heats of liquid water and coffee to be the same: 4187 J/kg K. A) Assume the coffee and ice form a closed system. You want them to equilibrate at 40° C....
What is the final equilbrium temperature when 40.0 grams of ice at -12.0 degrees C is...
What is the final equilbrium temperature when 40.0 grams of ice at -12.0 degrees C is mixed with 20.0 grams of water at 32 degrees C? The specific heat of ice is 2.10 kJ/kg degrees C, the heat of fusion for ice at 0 degrees C is 333.7 kJ/kg, the specific heat of water 4.186 kJ.kg degrees C, and the heat of vaporization of water at 100 degrees C is 2,256 kJ/kg. A. How much energy will it take to...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT