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April 19, 2014

Search: calculate the final temperature (once the ice has melted) of a mixture made up of initially of 75.0mL liquid water at 29 degrees Celsius and 7.0 g of ice at 0.0 degrees Celsius

Number of results: 52,101

Chemistry
Calculate the final temperature (once the ice has melted) of a mixture made up initially of 75.0 ml liquid water at 29.0 degrees C and 7.0 g ice at 0.0 degrees C.
Friday, February 26, 2010 at 11:00am by Jaclyn

Physics
Go through the numbers and you should find that there is enough energy in the water to melt all of the 75 g of ice, but not 300 g of ice. In the 75 g case, after all the ice is melted, the remaining heat in the water gets transferred to the melted ice, resulting in a final ...
Tuesday, November 30, 2010 at 11:15am by drwls

Chemistry
calculate the final temperature (once the ice has melted) of a mixture made up of initially of 75.0mL liquid water at 29 degrees Celsius and 7.0 g of ice at 0.0 degrees Celsius
Tuesday, February 23, 2010 at 2:02am by Celine

Physics _ Please help
If all the ice melts, 25*Lf = 8.33*10^6 kJ is absorbed in that process. If all of the steam condenses, 4*Lv = 9.04*10^6 kJ is released in that process. There is enough steam to melt all the ice. 0.71*10^6 J are still available from condensation of remaining to raise the ...
Friday, August 12, 2011 at 10:45am by drwls

chemistry
HELPPPP!!!! This is a lab, and i need help with the equations please!! Thank you !! Heat of fusion data table : Mass of foam cup = 3.57g Mass of foam cup + warm water = 104.58g Mass of foam cup + warm water + melted ice = 129.1g Temperature of warm water = 37 degrees celcius. ...
Sunday, December 2, 2012 at 12:32am by maryam

physics please help!
(a) If the ice block is really "very large", not all of it melts, and the final temperature remains 0 C. You end up with a large pool of 0 C liquid water including melted ice) in the ice block. (b) If mass M of original ice melts, Heat lost by poured water = Heat gained by ...
Friday, April 8, 2011 at 3:04am by drwls

Chemistry
q1 = heat to raise temperature of ice from -16.5 C to zero C. q1 = mass ice x specific heat ice x (Tfinal-Tinitial) q2 = heat to melt the ice. q2 = mass melted ice x heat fusion q3 = heat to raise temperature of melted ice from zero C to final T. q3 = mass melted ice x ...
Thursday, November 8, 2012 at 8:00pm by DrBob222

Physics PLEASE HELP
First you will have to compute the final temperature and determine if all the ice melts. (It does, in this case) Use the formula they gave you for the entropy lost by the cooling liquid water. The entropy gained by the melting ice is [80 cal/g]*3000 g/273K There will be ...
Saturday, November 10, 2012 at 2:46am by drwls

physics
Add the entropy gains of the ice cube (as it heats up to the equilibrium T) and the cooling water (as is cools down), The original liquid water actually loses entropy, but the ice gains more. You will need to calculate the equilibrium temperature first. All of the ice will ...
Sunday, September 19, 2010 at 5:59pm by drwls

Chemistry
A 63 gram block of an unknown metal at 88 degrees C was dropped into an insulated flask containing approx. 30 g of ice and 30 g of water at 0 degrees C. After the system had reached a steady temp. it was determined that 12.1 g of ice had melted. What is the specific heat of ...
Tuesday, May 15, 2007 at 5:04pm by Lindsay

Physics
A calorimeter with specific heat of 490x10^2J/kg^1K^1 has a mass of 2.00x10^-1kg that contains 3.00x10^-1kg of liquid water at 40C. If 5.00x10^-2kg of ice at 0C is dropped into the water. Find the final temperature of the mixture where the ice has melted is 23.8C. Calculate ...
Sunday, February 9, 2014 at 2:41am by Tsunayoshi

Science
A 500 mL bottle of water, which is at 25 degrees C, is poured over 120 g of ice at -8 degrees C. What will be the final temperature of the water when all the ice has melted. Assume that container is insulated and does not change temperature.
Wednesday, January 20, 2010 at 6:14pm by Bert

Science
A 500 mL bottle of water, which is at 25 degrees C, is poured over 120 g of ice at -8 degrees C. What will be the final temperature of the water when all the ice has melted. Assume that container is insulated and does not change temperature.
Thursday, January 21, 2010 at 5:44pm by Bert

Chemistry
I would work this in two stages. {mass ice x specific heat ice x [0-(-30)]} + [(mass warm water x specific heat water x (x-87)] = 0 That will take care of moving the ice T to zero C. x is the temperature of the mixture. The next step actually is three steps in one. heat to ...
Friday, March 9, 2012 at 11:10am by DrBob222

chemistry
q to raise temperature of ice from -13C to zero C (but remain as ice). q1 = mass ice x specific heat ice x (Tfinal-Tinitial) q to melt ice at zero C and remain at zero C. q2 = mass ice x heat fusion q to raise melted ice from zero C to final T. q3 = mass melted ice x specific ...
Saturday, October 15, 2011 at 2:52am by DrBob222

Chemistry
A 500 mL bottle at room temperature (25˚C) of water is poured over 120 g of ice that is (-8˚C). What will be the final temperature of the water be when all the ice has melted? You can ignore loss of heat to the room.
Saturday, November 3, 2012 at 8:04pm by Paige

What is the Final Temperature?
To melt all of the ice, 53*80= 4250 calories must be added. Cooling 120 g of water from 77 to 0 C would release 77*120 = 9240 calories. So all of the ice will melt. For the final temperature, set the heat lost by water equal to the heat gained by ice, including melted ice, and...
Sunday, January 6, 2013 at 1:03pm by drwls

Chemistry
You have three sources of heat in and heat out. 1. heat to melt ice + 2. heat to raise T of melted ice to final T - 3. heat lost from 120g H2O #1 + #2 + #3 = 0 (mass ice x heat fusion) + [mass melted ice x specific heat melted ice (H2O) x (Tfinal-Tinitial)] + [mass water ...
Monday, September 10, 2012 at 5:15pm by DrBob222

Science
Is the answer 26 celsius? Is it possible that the temp is greater than 25 celsius? A 500 mL bottle of water, which is at 25 degrees C, is poured over 120 g of ice at -8 degrees C. What will be the final temperature of the water when all the ice has melted. Assume that ...
Thursday, January 21, 2010 at 6:22pm by Bert

chem
If the ice had not been dry, you would have been measuring the two things: heat to melt ice, and heat to heat up the surface melted water, making the calculations more complex Hot water is used to get a large change in temperature of the water, and to drive the final ...
Thursday, February 11, 2010 at 10:20am by bobpursley

physics
A 1.3- block of ice is initially at a temperature of -3.5. If 6.6105 of heat are added to the ice, what is the final temperature of the system? Find the amount of ice, if any, that remains. Suppose the amount of heat added to the ice block is doubled. By what factor must the ...
Monday, November 22, 2010 at 5:20pm by katelyn

chm
You are heating crushed ice and a small amount of water and monitoring the temperature of the icy slurry until it reaches the point were the ice is nearly melted. How does the temperature change during this process? The temperature drops as the ice absorbs the heat and ...
Sunday, March 3, 2013 at 2:10am by jj

physics
A 40-g block of ice is cooled to −71C and is then added to 590 g of water in an 80-g copper calorimeter at a temperature of 27C. Determine the final temperature of the system consisting of the ice, water, and calorimeter. (If not all the ice melts, determine how much ...
Friday, April 6, 2012 at 5:46am by kevin

physics
A 40-g block of ice is cooled to −71C and is then added to 590 g of water in an 80-g copper calorimeter at a temperature of 27C. Determine the final temperature of the system consisting of the ice, water, and calorimeter. (If not all the ice melts, determine how much ...
Wednesday, April 11, 2012 at 2:05am by anthony

CHEMISTRY
If 142.38 g of l water at 21.7 degrees C is placed into a syrofoam cup with 174.36 g of ice at -27.5 degrees C what would be the final temperature of the entire contents at equilibrium? If it is partially frozen, how many g of the ice has melted? given values cp water = 4.184 ...
Sunday, October 14, 2007 at 4:27pm by Jake

Physics
25) A 75-g ice cube at 0 C is placed in 825g of water at 25 C. a) What is the final temperature of the mixture? b) If the final temperature is 0 C, then how much ice remains? c) change the ice's mass to 300g, and repeat the problem
Tuesday, November 30, 2010 at 8:46am by Y0gi

Physics
25) A 75-g ice cube at 0 C is placed in 825g of water at 25 C. a) What is the final temperature of the mixture? b) If the final temperature is 0 C, then how much ice remains? c) change the ice's mass to 300g, and repeat the problem I don't know how to work this at all!!! ...
Tuesday, November 30, 2010 at 11:15am by Y0gi

Chemistry
Hey, for chemistry class we are given days in the lab to conduct an experiment, then answer a number of questions that correlate with that experiment and how we can make use of it. This week we looked at the Molar Fusion of Ice and there are some questions i don't quite ...
Monday, December 15, 2008 at 7:13pm by Cody

physics
134 g of water at 7C is added to ice at 0C. If the final temperature of the system (which you can assume is isolated) is 0C, determine HOW MUCH ICE MELTED. The specific heat of water is 4186 J/kgC. The latent heat of fusion for H2O is 335,000 J/kg.
Wednesday, November 14, 2012 at 3:37pm by Joseph

Chemistry
heat to melt ice + heat to raise T of melted ice from zero to final T - heat lost by water at 28 in falling to final T. [mass ice x heat fusion] + [mass melted ice x specific heat water x (Tfinal-Tinitial)] + [mass warm water x specific heat water x (Tfinal-Tinitial)] = 0 ...
Friday, April 27, 2012 at 8:06pm by DrBob222

Chem
Calculate the final temperature when a 16.2 gram sample of ice at 0oC is placed into a styrofoam cup containing 128 grams of water at 79.0 oC. Assume that there is no loss or gain of heat from the surroundings. Heat of fusion of ice = 333 Jg-1 Specific heat of water = 4.184 JK...
Friday, March 23, 2012 at 7:19pm by Chase

Chemistry
heat to melt ice + heat to raise T of melted ice from zero to final T + heat lost from hot water = 0 heat to melt ice is mass x heat fusion. heat to raise T of melted ice is mass ice x specific heat water x (Tfinal-Tinitial). heat lost from hot water is mass x specific heat ...
Wednesday, October 5, 2011 at 3:18pm by DrBob222

Chemistry
when do you use the equation -qhot=qcold? -qhot=qcold is a rearrangement of heat gained (the cold in your equation) + heat lost (the hot in your equation) = 0 and that one, the one I listed as #1 above, is the one I prefer. It takes care of the signs for me and I don't need to...
Friday, November 28, 2008 at 4:37pm by DrBob222

Chemistry
Note the correct spelling of celsius. I assume the temperature of the ice is zero C. heat gained by ice + heat gained by melted ice + heat lost by 45 degree water = 0. [mass ice x heat fusion] + [mass melted ice x specific heat water x (Tfinal-Tinitial)] + [mass water x ...
Tuesday, April 12, 2011 at 12:16am by DrBob222

Chemistry
(heat to move ice from -13 to 0) + heat to melt ice) + (heat to move melted ice from 0 to final) + (heat lost by 112 g H2O @ 80) = 0 [(mass ice x specific heat ice x (0-(-13))] + [mass ice x heat fusio] + [mass melted ice x specific heat water x (Tfinal-Tinitial)] + (mass ...
Sunday, February 13, 2011 at 2:10pm by DrBob222

physics
A physical science student adds 500g of 0 degree C ice to 500g of 80 degree C coffee. What is the final temperature of the drink after thermal equilibrium is reached? How much of the ice was melted by the process? Assume coffee has same specific heat as water.
Sunday, July 17, 2011 at 5:17pm by Heat

Chemistry
A .25 g chunk of sodium metal is cautiously dropped into a mixture of 50g of water and 50 g of ice both at 0 C 2Na(s)+ 2h2o(l) -> 2naoh(aq)+ H2 Delta H = -368 kj Will the ice melt Assuming the final mixture has a heat capacity of 4.18 J/g C calculate the final ...
Sunday, January 15, 2012 at 3:29pm by Adriths

Chemistry
A .25 g chunk of sodium metal is cautiously dropped into a mixture of 50g of water and 50 g of ice both at 0 C 2Na(s)+ 2h2o(l) -> 2naoh(aq)+ H2 Delta H = -368 kj Will the ice melt Assuming the final mixture has a heat capacity of 4.18 J/g C calculate the final ...
Monday, January 16, 2012 at 2:33pm by Adriths

Physics
Suppose 100 g of water at 20C is poured over a 70-g cube of ice with a temperature of -8C. If all the ice melts, what is the final temperature of the water? If all of the ice does not melt, how much ice remains when the waterice mixture reaches equilibrium? I'm aware that ...
Thursday, July 19, 2012 at 4:46pm by James

physics
Suppose 300 g of water at 20C is poured over a 50-g cube of ice with a temperature of -6C. If all the ice melts, what is the final temperature of the water? If all of the ice does not melt, how much ice remains when the waterice mixture reaches equilibrium?
Thursday, July 26, 2012 at 8:20pm by lanre

physics
A 1.2 kg block of ice is initially at a temperature of -5C. (a) If 5.8 multiplied by 105 J of heat are added to the ice, what is the final temperature of the system? C (b) Suppose the amount of heat added to the ice block is increased by a factor of 3.0. By what factor must ...
Saturday, November 22, 2008 at 10:04pm by lyd

physics
A 1.2 kg block of ice is initially at a temperature of -5C. (a) If 5.8 multiplied by 105 J of heat are added to the ice, what is the final temperature of the system? C (b) Suppose the amount of heat added to the ice block is increased by a factor of 3.0. By what factor must ...
Saturday, November 22, 2008 at 10:06pm by lyd

Chemistry
To treat a burn on your hand, you decide to place an ice cube on the burned skin. The mass of the ice cube is 16.0 g, and its initial temperature is -11.4 C. The water resulting from the melted ice reaches the temperature of your skin, 31.0 C. How much heat is absorbed by ...
Saturday, December 8, 2012 at 12:26am by Anon

chemistry
To treat a burn on your hand, you decide to place an ice cube on the burned skin. The mass of the ice cube is 16.0 g, and its initial temperature is -10.4 C. The water resulting from the melted ice reaches the temperature of your skin, 28.3 C. How much heat is absorbed by ...
Thursday, April 25, 2013 at 12:32am by Audre

Warren
To treat a burn on your hand, you decide to place an ice cube on the burned skin. The mass of the ice cube is 13.2 g, and its initial temperature is -11.9 C. The water resulting from the melted ice reaches the temperature of your skin, 30.0 C. How much heat is absorbed by ...
Wednesday, November 20, 2013 at 11:27pm by Kyla

Chemistry
Note the correct spelling of celsius. Heat gained by ice + heat gained by melted water + heat lost by original water = 0 [mass ice x heat fusion] + [mass melted ice x specific water x (Tfinal-Tinitial)] + [mass 250mL water x specific heat water x (Tfinal-Tinitial)] = 0 Solve ...
Tuesday, April 12, 2011 at 12:20am by DrBob222

Jake
If 142.38 g of l water at 21.7 degrees C is placed into a syrofoam cup with 174.36 g of ice at -27.5 degrees C what would be the final temperature of the entire contents at equilibrium? If it is partially frozen, how many g of the ice has melted? given values cp water = 4.184 ...
Tuesday, October 16, 2007 at 6:45pm by Chemistry

physics 2
heat to melt x grams ice: x*Hfusion heat absorbed by warm water: 120*cw*(tf-85) heat absorbed by melted ice to get to final temperataure: x*cw*(tf-0) the sum of the heats gained is zero. x is the amount of ice that melted. xHf+( x)cw*(tf-0)+120(cw)(Tf-85)=0 first, see if all ...
Sunday, January 19, 2014 at 6:32pm by bobpursley

Chem
heat to melt ice + heat to raise T of melted ice to final T + heat lost by water initially at 79 C. [mass ice x heat fusion] + [mass melted ice x specific heat H2O x (Tfinal-Tinitial)] + [mass warm water x specific heat H2O x (Tfinal-Tinitial)] = 0 Solve for Tfinal.
Friday, March 23, 2012 at 7:19pm by DrBob222

Physics
heat gained in anyting changing temp =mass*c*(tf-ti) heat gained by melting ice: mass*Lf where Lf is the heat of fusion for ice per mass. Now, when this happens in a closed system, everything has the same final temperature, and the sum of all heats gained is zero (some of them...
Tuesday, December 10, 2013 at 6:10pm by bobpursley

Chemistry
Let's see now. If I had 1 g ice and it melted into water, it would form 1 g water. So grams ice and grams melted ice must be the same. right?
Wednesday, May 11, 2011 at 11:49pm by DrBob222

Taylor
To treat a burn on your hand, you decide to place an ice cube on the burned skin. The mass of the ice cube is 12.6 g, and its initial temperature is -10.4 C. The water resulting from the melted ice reaches the temperature of your skin, 28.1 C. How much heat is absorbed by ...
Friday, November 15, 2013 at 4:24pm by Aubrey

Physics
a): Two 50 g ice cubes are dropped into 200 g of water in a thermally insulated container. If the water is initially at 25 degree Celsius, and the ice comes directly from a freezer at -15 degree Celsius, what is the final temperature at thermal equilibrium? b): What is the ...
Tuesday, December 10, 2013 at 6:10pm by bano

Chemistry
A 100g sample of ice at 0C is added to 150.0 mL of liquid water at 80C in a styrofoam cup calorimeter. (The specific heat capacity of water is 1.184 J/gC, the density of water is 1.00 g/mL, and ∆Hfus = 6.01 kJ/mol) a) Does all of the ice melt?( show work to recieve ...
Monday, November 5, 2012 at 3:53pm by Lauren

Science
You would have to account for the new water created by the melting ice also. m*c*(Tf-To)+m*Hf+m*c*(Tf-To)+m*c*(Tf-To)=0 Where the first product is the warming of the ice, which would first increase from -8 to a final T of 0. The second product is the melting of that same ice ...
Wednesday, January 20, 2010 at 6:14pm by Ryan

college chemistry
melt ice + move ice from zero to final T + cool H2O from 8 to final T = 0 (mass ice x heat fusion) + (mass melted ice x specific heat H2O x (Tfinal-Tinitial) + (mass H2O x speicif heat H2O x (Tfinal-Tinitial) = 0 Solve for mass H2O. I obtained 420 g but you should confirm that...
Thursday, January 30, 2014 at 3:26pm by DrBob222

College Chemistry
heat to melt ice + heat to raise T of melted ice from zero C to the final T + heat lost by warm water = 0 1st term: mass ice x deltaH fusion. 2nd term: mass melted ice x specific heat water x (Tfinal-Tinitial) 3rd term: mass hot water x specific heat water x (Tfinal-Tinitial) ...
Friday, October 7, 2011 at 10:11pm by DrBob222

Chemistry
(g ice x heat fusion) +[g melted ice x specific heat H2O x (Tfinal-Tinitial)] + [g H2O x specific heat water x (Tfinal-Tinitial)] = 0 You have only one unknown namely g ice. Solve for that. I estimated the answer to be about 7g ice at zero. Note that I have three terms above; ...
Saturday, January 28, 2012 at 12:10pm by DrBob222

chemistry
A 2.622 g sample of almonds is ignited and used to melt ice in a can. a. If the almond sample melted 15.24g of ice what is the heat produced in Kcal grams of nuts? d.If the heat from the almond sample was used to heat 100mL of water at 0.0 degree centigrade, what would be the ...
Monday, October 15, 2012 at 10:02am by Anthony

Physics
Glass of water has mass of 240g at room temp (25C). Add 50g of 0C ice. What final temp after ice is melted. (at equilibrium).
Tuesday, April 26, 2011 at 10:19pm by Sue

Chemistry. Please help!!
Calculate the final temperature when a 18.7 gram sample of ice at 0 degrees C is placed into a styrofoam cup containing 113 grams of water at 71.6 degrees C. Assume that there is no loss or gain of heat from the surroundings. Heat of fusion of ice = 333 Jg^-1 Specific heat of ...
Friday, March 2, 2012 at 4:15pm by JJ

chemistry
A 2.622 g sample of almond is ignited and used to melt ice in a can. a. if the almond sample melted 15.24g of ice,What is the heat produced in kcal/gram? b. If the heat from the almond sample was used to heat 100.0 mL of water at 0.0 degree centigrade.What would be the final ...
Sunday, October 14, 2012 at 1:33am by adonis

Chem
A student measures the following data regarding the heat of fusion of ice: 25.8 g ice at 0.0C is placed into the calorimeter which contains 100.0 g water at 21.7C. The final temperature comes to 1.5C. The calorimeter has a heat capacity of 15.6 J/C. (a) Calculate the ...
Wednesday, January 23, 2013 at 10:08pm by Susie

Chemistry
3) You pour 240 mL of Coke into a glass, where the T of the beverage is at 10.5 *C. You then add one ice cube of 45g. Determine the final temperature and the amount of ice remaining, if any. So I know that there won't be any more ice left because they will reach thermal ...
Wednesday, May 9, 2012 at 3:06pm by Robert

Chemistry
Two 20.0g ice cubes at -10.0 C are placed into 275g 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.
Saturday, July 9, 2011 at 3:10pm by Josh

physics
A revolutionary new diet advertises that one can lose weight simply by eating ice. When one eats ice,chemical energy in the body is used to melt the ice and then raise the temperature of the melted ice to the temperature of the body, 37 degrees Celsius.Past scientific studies ...
Saturday, January 22, 2011 at 6:58pm by jenny

Physics
Assume all of the ice melts. (If it doesn't you will find out later when you compute the final temperature). Look up the specific heat of aluminum. It is 0.22 cal/C gm Assume the heat lost by the water and aluminum when being lowered to final temperature T equals the heat ...
Saturday, August 20, 2011 at 1:36pm by drwls

Chemistry - Heat of Fusion of Ice
Conclusion question(s) from a lab we did to find the heat of fusion of ice: Does the value obtained for the molar heat of fusion depend on the volume of water used? Does it depend on the mass of ice melted? Does it depend on the final temperature of the mixture? The heat of ...
Sunday, October 1, 2006 at 2:11pm by J.M.

Chemistry
This may not be the answer you are looking for but if the water is at zero and the ice is at zero and you are adding heat you know that SOME of the ice will melt. You don't know if all of it will melt until you calculate it but the problem doesn't ask for that. Nor does it ask...
Friday, May 24, 2013 at 8:16am by DrBob222

physics
Years ago, a block of ice with a mass of about 22kg was used daily in a home icebox. The temperature of the ice was 0.0 degrees Celsius when delivered. As it melted, how much heat did a block of ice that size absorb? The latent heat of fusion of water is 3.34 x 10 ^ 5 J/kg. ...
Saturday, November 20, 2010 at 10:06am by Norah

Material Science
A polystyrene ice chest contains 3 kg of ice at 0 degrees Celsius. Triangle H for melting = 3.34 x 10 to the 5 power J/kg p = 1000 kg/m cubed, CP =4190 J/ (kg K). Heat transfer is limited by conduction (k=0.06W/m K)) from the outside wall at 30 degrees Celsius. This means that...
Saturday, August 24, 2013 at 10:16pm by Joy

science
Finishing his ginger ale, Ramesh stands at the party holding his insulated foam cup that has nothing in it but 0.100kg of ice at 0 degree celsius. How much heat must be gained by the ice in order for all of it to melt? How much more heat must be gained to raise the temperature...
Monday, January 9, 2012 at 1:51am by Debra

Physics
Assume the optimal coffee drinking temperature is 75C, and further assume coffee has the same heat capacity and density as water. a. How much energy is required to raise the temperature of 1 cup (0.237 liters) of coffee initially at 25C to the optimal temperature? b. How ...
Sunday, December 5, 2010 at 7:04pm by Steve

Chem 212
To treat a burn on your hand, you decide to place an ice cube on the burned skin. The mass of the ice cube is 16.1 g, and its initial temperature is -13.3 C. The water resulting from the melted ice reaches the temperature of your skin, 31.3 C. How much heat is absorbed by ...
Tuesday, February 19, 2013 at 10:05pm by 1231az

chemistry
1. ice melts at zero C. q = mass ice x heat fusion 2. melted water at zero changes temperature to Tfinal. q = [mass melted ice x specific heat H2O x (Tfinal-Tinitial)] 3. Warm water at 100 C cools to Tfinal q = [mass warm water x specific heat H2O x (Tfinal-Tinitial)] Add 1 + ...
Thursday, October 4, 2012 at 8:32pm by DrBob222

Chemistry
On more than one occasion when our kids were small, we would come inside from playing in the snow and I would make hot chocolate by heating the chocolate milk in the microwave. Invariably, I would get the milk too hot for at least one of them. One time, rather than adding more...
Friday, January 11, 2013 at 10:49pm by Breanne

Chemistry
a. q1 needed to melt all of the ice q1 = mass ice x heat fusion. q2 = mass H2O x specific heat H2O x delta T. (and the specific heat H2O is NOT 1.184).(Consider delta T = 80 which is the maximum heat that can be released). There is more than enough to melt all of the ice. This...
Monday, November 5, 2012 at 3:53pm by DrBob222

Science
Ms Sue is right. A mixture of ice and water will have a temperature of zero Celsius. If heat is added all of it will melt but the temperature will not rise above zero C until the last bit of ice has melted. If heat is extracted all of it will freeze but the temperature of the ...
Tuesday, March 4, 2008 at 10:22pm by DrBob222

Chemistry
Calculate the temperature change in the water upon complete melting of the ice. Hint: Determine how much heat is absorbed by the melting ice and then use q =mC*Delta T to calculate the temperature change of the 314 g of water. under the following conditions: A 14.7 g ice cube ...
Thursday, November 18, 2010 at 1:32am by Ricardo

ph
calculate the heat of fusion of ice from the following data at 0c add to water : Mass of calorimetet 60 g Mass of calorimeter and water 460 Mass of calorimeter plus water and ice 618 g Initial temperature of water 38 c Final temperature of mixture 5 c Specific heat of ...
Sunday, January 26, 2014 at 3:32am by Anonymous

physics
A 5-kg block of ice is at a temperature of -27 C. How much heat must be added to the ice to produce 5 kg of liquid water with a final temperature of 35 oC?
Monday, July 29, 2013 at 11:16pm by franko

college
A quantity of ice at 0C is added to 65.0 g of water in a glass at 55C. After the ice melted, the temperature of the water in the glass was 15C. How much ice was added? The heat of fusion of water is 6.01 kJ/mol and the specific heat is 4.18 J/(gC).
Wednesday, July 14, 2010 at 6:59pm by Anonymous

Chemistry/Calorimetry
You buy coffee (200.0 ml) served in a styrofoam cup. You are up late working in a chemistry lab, and want to drink the coffee right away, but at 95.0 degrees C, it is too hot to drink. You like the temperature of your coffee to be 79.0 1.0 degrees C. You decide that the ...
Thursday, February 23, 2012 at 11:00pm by Jen

physics
Use the area, thickness, and density to calculate the mass of ice. Then mass ice x specific heat ice x 12.6 = joules necessary to raise the temperature of the ice to zero degrees C. then add in the amount to melt the ice which is mass ice x heat of fusion. Watch the units. ...
Monday, April 14, 2008 at 4:03pm by DrBob222

chemistry (heat of fusion/vaporization)
i need help setting this problem up. You have an insulated container of water that has a temperature of 83.2 C, you continue to add ice until the temperature reaches .6 C and you remove the excess ice, your volume increased by 79.8 mL. What amount of hot water did you have in ...
Monday, March 26, 2007 at 7:48pm by abby

chemistry
a 14.7g ice cube is placed into 324g og water. calvulate the temperature change in the water upon complete melting of the ice. hint: determine how ,uch heat is absorbed by the melting ice and then use q=mc delta T to calculate the temperature change. use the heat of fusiion ...
Tuesday, May 4, 2010 at 4:24pm by janny

physics
right on 1, wrong on 2. As long as ice and water are together (that is SOME ice and SOME water) the temperature of the melting mixture will stay at zero C. After the last molecule of ice as melted, then the temperature of the melt will begin to rise. Ethyl alcohol, at the ...
Friday, November 23, 2007 at 12:42am by DrBob222

physics
At equilbrium, the melted ice (mass m) and the water it changes into will gain as much heat as the original coffee (mass M) loses. 0.140g*(89 - T)*4186 = 0.011*[333,000 + T*4186] 52,160 -586 T = 3663 + 46 T 632 T = 48,497 T = 77 C Solve for final temperature T
Sunday, December 4, 2011 at 7:58am by drwls

Chemistry (Thermo)
High quality coal (anthracite) is almost pure carbon. The combustion of carbon to carbon dioxide releases 393kJ per mol of carbon burnt. If 1kg of anthracite is burnt: a) How much heat is released? b) How much ice (in kg) at 273K could be melted to give water at 273K? c) How ...
Friday, September 10, 2010 at 10:25am by Amy

Chemistry
A 19.6 g sample of ice at -10.0C is mixed with 100.0 g of water at 75.4C. Calculate the final temperature of the mixture assuming no heat loss to the surroundings. The heat capacities of H2O(s) and H2O(l) are 2.08 and 4.18 J g-1 C-1, respectively, and the enthalpy of fusion...
Tuesday, November 23, 2010 at 12:33pm by Anonymous

Chemisrty
A 10.0 g sample of ice at -14.0C is mixed with 124.0 g of water at 81.0C. Calculate the final temperature of the mixture assuming no heat loss to the surroundings. The heat capacities of H2O(s) and H2O(l) are 2.08 and 4.18 J/gC, respectively, and the enthalpy of fusion for ...
Sunday, December 9, 2012 at 10:16pm by Nancy

Chem; States of Matter
This will get you started on a part. The problem tells you that all of the ice doesn't melt; therefore, you know the temperature must be zero (or all of the ice would have melted) to find how much has melted do this. steam condensed at 100C = 175g x heat vap = ? 175g H2O from ...
Tuesday, February 11, 2014 at 11:52pm by DrBob222

Chemistry
Several years ago a company invented plastic ice cubes. These were colored plastic cubes with frozen water (or another substances) inside. That way, as the solid melted, it could cool your drink, but did not dilute it with extra water (from the melted ice). If plastic cubes ...
Sunday, April 24, 2011 at 11:13pm by Kat

Physics
Take two Styrofoam cups, partially fill them with equal amounts of cold water, and drop equal amounts of ice into each cup to obtain a mixture of ice and water. a. Stir the water and ice mixture in one of the cups vigorously with a nonmetallic stirrer until all of the ice has ...
Tuesday, December 28, 2010 at 12:31pm by Katherine

chemistry
Calculate the temperature change in the water upon complete melting of the ice. Hint: Determine how much heat is absorbed by the melting ice and then use q =mC*Delta T to calculate the temperature change of the 314 g of water. under the following conditions: A 14.7 g ice cube ...
Wednesday, November 17, 2010 at 7:54pm by jose

physics
Q.an aluminium can of mass 200gm contains 500gms of water at 50c.an ice cube of mass 50gms,initially at a temperature of -20c is thrown into the can of water. i.what is the final temperature onces the ice metls and comes into equilibrium? ii.now a 200gm piece of Iron whose ...
Saturday, June 1, 2013 at 11:05am by rosy

Physics
I was having trouble with two different physics problems when studying for a test. Any help is appreciated. 1.) A 11.6-kg block of ice has a temperature of -14.5 °C. The pressure is one atmosphere. The block absorbs 6.87 x 106 J of heat. What is the final temperature in ...
Sunday, April 13, 2008 at 11:17pm by Sam

Physics
I was having trouble with two different physics problems when studying for a test. Any help is appreciated. 1.) A 11.6-kg block of ice has a temperature of -14.5 °C. The pressure is one atmosphere. The block absorbs 6.87 x 106 J of heat. What is the final temperature in ...
Sunday, April 13, 2008 at 11:18pm by Sam

physics
Suppose that 90 g of hot water at a temperature of 75 degrees C is poured into a cavity in a very large block of ice at 0 degrees C. (a) What will be the final temperature of the water in the cavity? (b) What mass of ice must melt in order for the water to cool down to the ...
Thursday, April 7, 2011 at 6:56pm by sara

physics please help!
Suppose that 90 g of hot water at a temperature of 75 degrees C is poured into a cavity in a very large block of ice at 0 degrees C. (a) What will be the final temperature of the water in the cavity? (b) What mass of ice must melt in order for the water to cool down to the ...
Friday, April 8, 2011 at 3:04am by Dan

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