If you add 4200000 J of energy to a 9.65 kg block of -11.6 Celsius ice, what is the final temperature of the block
If you add 4200000 J of energy to a 9.65 kg block of -11.6 Celsius ice,...
3. Let a block of ice with temperature -3° Celsius be dropped in a cool container of water with temperature +12° Celsius. The water is in a copper cup of initial temperature +12° Celsius. The specific heats and latent heats are cwater = 2093 J/(kg.K). 4186 J/(kg.K), cce Ccopper = 387 J/(kg.K), Lrusion = 3.33 x 10 J/kg. 6 kg of ice, 3 kg of water and 3 kg of copper. The system is thermally insulated. There are (a) Does...
How much energy is needed to change a 2 kg block of -8.2 Celsius ice to 10.6 Celsius water
Determine the equilibrium temperature when a 5.00 kg block of ice at -10 degrees celsius is added to an insulated container partially filled with 12 kg of water at 13 degrees C.
A 2kg block of ice at 0 degrees celsius is dropped into a very large lake at 25 degrees celsius and completely melts. For water, the heat of fusion is 3.35*10^5 J/kg, the heat of vaporization is 2.25*10^5 J/kg, and the specific heat is 4190 J/kg*K. What is the net change in entropy of the system consisting of cie and the lake due to this melting process?
1 2 3 A 10.5-kg block of ice has a temperature of -22.1 °c. The pressure is one atmosphere. The block absorbs 6.99 x of heat. What is the final temperature in degrees Celsius of the liquid 10 the tolerance is +/-2% Click if you would like to show work for this question: open Show works
1 kg block of ice at 0 degrees celsius placed in cooler. How much heat will the ice remove as it melts to water at 0 degree celsius. I know the answer is 80kcal but don't know the math that backs up the answer-please help!
Ice with a mass of 0.15 kg at 0.0 degrees Celsius is added to 0.25 kg of water at 20 degrees Celsius in a thermally insulated cup at atmospheric pressure. This approximates to a thermally insulated system of ice and water. Where no heat enters of leaves the system, what is the final (equilibrium) temperature of the system? Give your value in degrees Celsius.
IP A 1.0-kg block of ice is initially at a temperature of -5.0 ∘C. A) If 2.9×105 J of heat are added to the ice, what is the final temperature of the system? B) Find the amount of ice, if any, that remains.
155 grams of ice at -10.0 degrees celsius is added to 1.17 kg of water at 70.0 degrees celsius and mixed together in thermal isolation until they come to equilibrium. The specific heat of ice is 2010 J/kgC. The specific heat of water is 4186 J/kgC. The latent heat of fusion for water is 3.34x10^5 J/kg. The latent of vaporization for water is 2.26x10^6 J/kg. What is the final equilibrium. The answer is 51.9 celsius. I just need the steps...
A 0.07 kg ice cube at -300C is placed in 0.43 kg of 30.30C water in a very well-insulated container. What is the final temperature in degrees Celsius? Specific heat of ice = 2000 J/(kg.K), Specific heat of water = 4186 J/(kg.K), Latent heat of fusion of ice = 33.5 x 104 J/kg.