Question

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.

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
( A = 18, B = 93). A (10.0+A) g ice cube at -15.0oC is placed...
( A = 18, B = 93). A (10.0+A) g ice cube at -15.0oC is placed in (125+B) g of water at 48.0oC. Find the final temperature of the system when equilibrium is reached. Ignore the heat capacity of the container and assume this is in a calorimeter, i.e. the system is thermally insulated from the surroundings. Give your answer in oC with 3 significant figures. Specific heat of ice: 2.090 J/g K Specific heat of water: 4.186 J/g K...
A = 13 B = 27 A (10.0+A) g ice cube at -15.0oC is placed in...
A = 13 B = 27 A (10.0+A) g ice cube at -15.0oC is placed in (125+B) g of water at 48.0oC. Find the final temperature of the system when equilibrium is reached. Ignore the heat capacity of the container and assume this is in a calorimeter, i.e. the system is thermally insulated from the surroundings. Give your answer inoC with 3 significant figures. Specific heat of ice: 2.090 J/g K Specific heat of water: 4.186 J/g K Latent heat...
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...
How much energy is required to change a 23 g ice cube from ice at −...
How much energy is required to change a 23 g ice cube from ice at − 12 ◦ C to steam at 101 ◦ C? The specific heat of ice is 2090 J / kg · ◦ C and of water 4186 J / kg · ◦ C. The latent heat of fusion of water is 3 . 33 × 10^5 J / kg, its latent heat of vaporization is 2 . 26 × 10^6 J / kg, and the...
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 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.
A 25 g ice cube at -15.0oC is placed in 169 g of water at 48.0oC....
A 25 g ice cube at -15.0oC is placed in 169 g of water at 48.0oC. Find the final temperature of the system when equilibrium is reached. Ignore the heat capacity of the container and assume this is in a calorimeter, i.e. the system is thermally insulated from the surroundings. Give your answer in oC with 3 significant figures. Specific heat of ice: 2.090 J/g K Specific heat of water: 4.186 J/g K Latent heat of fusion for water: 333...
A 16 g ice cube at -15.0oC is placed in 140 g of water at 48.0oC....
A 16 g ice cube at -15.0oC is placed in 140 g of water at 48.0oC. Find the final temperature of the system when equilibrium is reached. Ignore the heat capacity of the container and assume this is in a calorimeter, i.e. the system is thermally insulated from the surroundings. Give your answer in oC with 3 significant figures. Specific heat of ice: 2.090 J/g K Specific heat of water: 4.186 J/g K Latent heat of fusion for water: 333...
An ice cube of mass 0.041 kg and temperature -13 ∘C is heated until it is...
An ice cube of mass 0.041 kg and temperature -13 ∘C is heated until it is now fully melted and at a temperature of 11∘C now. What percentage of the total energy was used to melt the ice? (Assume that there is no heat exchange with any container or the environment.) The specific heat of ice is 2200 J/kg ∘C and the specific heat of water is 4186 J/kg ∘C. The latent heat of fusion of ice is 334000 J/kg...
A 100g ice cube at 0°C is placed in 400g of water at 30°C. If the...
A 100g ice cube at 0°C is placed in 400g of water at 30°C. If the container is perfectly insulated, what will be the final temperature when all the ice has been melted? The specific heat of water is 4.184 kJ/kg. K. The latent heat of fusion for water at 0°C is approximately 334 kJ/kg (or 80 cal/g).
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT