Wednesday
July 30, 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: 34,758

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.
February 26, 2010 by Jaclyn

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
February 23, 2010 by Celine

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. ...
December 2, 2012 by maryam

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 ...
May 15, 2007 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 ...
February 9, 2014 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.
January 20, 2010 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.
January 21, 2010 by Bert

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.
November 3, 2012 by Paige

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 ...
January 21, 2010 by Bert

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 ...
October 14, 2007 by Jake

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 ...
March 3, 2013 by jj

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
November 30, 2010 by Y0gi

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.
November 14, 2012 by Joseph

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 ...
December 15, 2008 by Cody

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 ...
April 6, 2012 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 ...
April 11, 2012 by anthony

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!!! ...
November 30, 2010 by Y0gi

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 ...
January 15, 2012 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 ...
January 16, 2012 by Adriths

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 ...
November 22, 2010 by katelyn

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...
March 23, 2012 by Chase

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.
July 17, 2011 by Heat

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 ...
November 5, 2012 by Lauren

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 10.9 g, and its initial temperature is -12.0 C. The water resulting from the melted ice reaches the temperature of your skin, 29.6 C. How much heat is absorbed by ...
April 12, 2014 by Karen

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 ...
October 16, 2007 by Chemistry

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 ...
July 19, 2012 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?
July 26, 2012 by lanre

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 ...
December 8, 2012 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 ...
April 25, 2013 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 ...
November 20, 2013 by Kyla

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 ...
November 15, 2013 by Aubrey

physics
A 49-g bullet traveling at 290m/s penetrates a block of ice at 0∘C and comes to rest within the ice.Assuming that the temperature of the bullet doesn't change appreciably, how much ice is melted as a result of the collision? The heat of fusion of water is 333 kJ/kg.
June 4, 2014 by Anonymous

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 ...
December 10, 2013 by bano

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).
April 26, 2011 by Sue

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 ...
November 22, 2008 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 ...
November 22, 2008 by lyd

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 ...
October 15, 2012 by Anthony

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 ...
March 26, 2007 by abby

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...
August 24, 2013 by Joy

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 ...
March 2, 2012 by JJ

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 ...
May 9, 2012 by Robert

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 ...
January 23, 2013 by Susie

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 ...
October 14, 2012 by adonis

Physics!!!Please Help!
-Steam at 100 C is mixed with 166.4 g of ice at C32.8 C, in a thermally insulated container, to produce water at 44.6 C. Ignore any heat absorption by the container. -Cwater = 4186. J/(kg C) -Cice = 2090. J/(kg C) -Lf,water = 3.33 105 J/kg -Lv,water = 2.26 106...
April 10, 2013 by ken

Science
The total amount of ice in the Greenland ice sheet is estimated to be 2.85 million cubic km. Assume the Earth's surface is 70% covered by ocean, and that the Earth's radius is 6300 km. How many meters would sea level rise if the entire Greenland ice sheet were to melt? (You ...
March 19, 2014 by Bane Havoc

Physics-
-Steam at 100 C is mixed with 166.4 g of ice at C32.8 C, in a thermally insulated container, to produce water at 44.6 C. Ignore any heat absorption by the container. -Cwater = 4186. J/(kg C) -Cice = 2090. J/(kg C) -Lf,water = 3.33 105 J/kg -Lv,water = 2.26 106...
April 9, 2013 by blur oh no

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. ...
November 20, 2010 by Norah

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.
July 9, 2011 by Josh

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 ...
October 1, 2006 by J.M.

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?
July 29, 2013 by franko

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...
January 9, 2012 by Debra

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...
January 11, 2013 by Breanne

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 ...
January 22, 2011 by jenny

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 ...
February 19, 2013 by 1231az

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 ...
December 5, 2010 by Steve

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 ...
September 10, 2010 by Amy

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 ...
February 23, 2012 by Jen

chemistry
When ice at 0C melts to liquid water at 0C, it absorbs 0.334 kj of heat per gram. Suppose the heat needed to melt 31.5 g of ice is absorbed from the water contained in a glass. If this water has a mass of .210 kg and a temperature of 21.0C, what is the final temperature of the...
June 24, 2009 by Capacino

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...
November 23, 2010 by Anonymous

Chemistry
A 13.0-g sample of ice at -13.0C is mixed with 112.0 g of water at 80.0C. 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/g C, respectively, and the enthalpy of fusion ...
February 13, 2011 by Katrina

biology
A 28.0-g sample of ice at -18.0C is mixed with 124.0 g of water at 85.0C. 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/g C, respectively, and the enthalpy of fusion ...
October 15, 2011 by layla

chemistry
A 13.0-g sample of ice at -13.0C is mixed with 105.0 g of water at 78.0C. 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/g C, respectively, and the enthalpy of fusion ...
October 15, 2011 by layla

Chemistry
A 14.0-g sample of ice at -18.0C is mixed with 122.0 g of water at 87.0C. 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/g C, respectively, and the enthalpy of fusion ...
March 9, 2012 by Janesa

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 ...
December 9, 2012 by Nancy

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 ...
December 28, 2010 by Katherine

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 ...
April 24, 2011 by Kat

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).
July 14, 2010 by Anonymous

Chemistry
A 300.0g sample of ice at -30.OC is mixed with 300.0G of water at 90C. Calculate the final temperature of the mixture assuming no heat loss to the surroundings. The heat capazities of H2O(s) and H20(L) are 2.03 and 4.18 j/g*C respectivly, and the entahply fusion for ice is 6....
February 24, 2012 by Keru

math
If i place a dish of ice outside in the sun, The ice has a mass of 0.59 kg and a surface area of 0.039 m2. Assuming that the ice is originally at 0 C and using my answer for part b, which was 1370w/m^2 * 49 * 0.039m^2 = 26.18 watts, How long do i have to wait until all the ...
December 16, 2008 by trigger

Physics
A 3.9010^2kg cube of ice at an initial temperature of -18.0degreesC is placed in 0.480kg of water at 41.0degreesC in an insulated container of negligible mass. Calculate the change in entropy of the system. I found the equilibrium temperature to be at 304.9K, then used change...
December 7, 2010 by Melissa

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 ...
November 18, 2010 by Ricardo

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 ...
April 13, 2008 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 ...
April 13, 2008 by Sam

Chemistry
When ice at 0C melts to liquid water at 0C, it absorbs 0.334 kJ of heat per gram. Suppose the heat needed to melt 30.7 g of ice is absorbed from the water contained in a glass. If this water has a mass of 0.189 kg and a temperature of 21.0C, what is the final temperature of...
June 7, 2011 by Lance

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 ...
January 26, 2014 by Anonymous

physic
For a class demonstration, your physics instructor pours 1.16 kg of steam at 100.0C over 4.69 kg of ice at 0.0C and allows the system to reach equilibrium. He is then going to measure the temperature of the system. While the system reaches equilibrium, you are given the ...
April 11, 2011 by help me please

Physical Science
How do you calculate the number of grams of ice at 32 degrees celsius that can be melted by 1g of steam?
March 11, 2013 by Bella

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 ...
June 1, 2013 by rosy

Chemistry
An ice cube at 0.00 degree celsius with a mass of 23.5 g is placed into 550.0 g of water, initially at 28.0 degree celsius, in an insulated container. Assuming that no heat is lost to the surroundings, what is the temperature of the entire water sample after all the ice has ...
April 27, 2012 by Amir

more physics.
What change in entropy occurs when a 27.9-g ice cube at -12 C is transformed into steam at 115 C? Add the entropy changes due to: (1) heating the ice to 0C, (2) melting the ice, (3) heatng the water from 0 to 100 C, and (4) Evaporating the liquid water. For (2) and (3), the ...
April 26, 2007 by jean

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 ...
April 7, 2011 by sara

physics
For a class demonstration, your physics instructor pours 1.16 kg of steam at 100.0C over 4.69 kg of ice at 0.0C and allows the system to reach equilibrium. He is then going to measure the temperature of the system. While the system reaches equilibrium, you are given the ...
April 5, 2011 by please help me

What is the Final Temperature?
Four ice cubes at exactly 0 degrees C having a total mass of 53.0 g are combined with 120 g of water at 77 degrees C in an insulated container. If no heat is lost to the surroundings, what will be the final temperature of the mixture?
January 6, 2013 by Amy

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 ...
April 8, 2011 by Dan

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 ...
May 4, 2010 by janny

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 ...
November 17, 2010 by jose

Chemistry
A 24.0 g sample of ice at -19.0C is mixed with 118.0 g of water at 85.0C. 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 ...
November 28, 2008 by Rachelle

Chemistry HEAT OF FUSION
What amount of energy is required to melt a 26.9 g piece of ice at 0oC? The heat of fusion of ice = 333 Jg-1 Heat required to melt the ice = J What amount of energy must be removed from 120 g of water to cool it from 72.1oC to 12.4oC? Specific heat of water = 4.184 JK-1g-1 ...
October 6, 2011 by tanner

Chemistry
The specific heat of solid copper is 0.385 J/g*C. What thermal energy change occurs when the temperature of a 40.10g sample of copper is cooled from 42.9C to 10.0C? Be sure to give you answer the proper sign. I know this is part of the answer which (42.9-10.0)*40.10*0.385=508 ...
February 27, 2012 by Tiffany

Chemistry
The specific heat of solid copper is 0.385 J/g*C. What thermal energy change occurs when the temperature of a 40.10g sample of copper is cooled from 42.9C to 10.0C? Be sure to give you answer the proper sign. I know this is part of the answer which (42.9-10.0)*40.10*0.385=508 ...
February 27, 2012 by Tiffany

chemistry
what is the final temperature of amixture containning 25 grams of ice at -20 degree celciusadded to water at room temperature 22oC mass of water is 50g followed the steps given by you but not getting the answer (0degree celsius) ice at -20 to ice at 0 degree=mcdelta T=25*2.06*...
May 12, 2014 by treasa

Chemistry
An ice cube at 0 degrees Celsius was dropped into 30.0 g of water in a cup at 45.0 degrees Celsius. At the instant that all of the ice was melted, the temperature of the water i the cup was 19.5 degrees Celsius. What was the mass of the ice cube?
April 21, 2010 by Scoob

Chemistry
An ice cube at 0 degrees Celsius was dropped into 30.0g of water in a cup at 45 degrees Celsius. At the instant that all of the ice was melted, the temperature of the water in the cup was 19.5 degrees Celsius. What was the mass of the ice cube?
April 23, 2010 by Help1001

had
A 0.106 kg ice cube is taken out of a freezer with temperature -16C. It is then added to a glass of water with mass 0.25 kg. The water initially has a temperature of 24.2 C. Assume no heat is added or lost to the surroundings. Calculate the amount heat required to completely...
March 3, 2014 by Anonymous

chemistry
1) Calculate the specific heat capacity (J/g oC) of iron, if a 803 g sample lost 937.4 J of heat energy in going from an initial temperature of 5.50 oC to a final temperature of 2.90 oC. 2)Calculate the final temperature (oC) of a 243 g sample of water originally at a ...
February 17, 2010 by eng

physics
A 0.299-m-thick sheet of ice covers a lake. The air temperature at the ice surface is -15.0 C. In 4.90 minutes, the ice thickens by a small amount. Assume that no heat flows from the ground below into the water and that the added ice is very thin compared to 0.299 m. ...
April 18, 2012 by anonymous

physics
Dry saturated steam at 100 degree C is passed into 250 gm of a mixture of ice and water contained in a calorimeter of thermal capacity 45J/K.When all the ice has just melted,the mass of the content has increased by 10 gm due to condensed steam.Assuming no heat exchange between...
March 15, 2012 by AFOLABI .O.

Physics
Inside an insulated container, a 250-g ice cube at 0C is added to 200 g of water at 18C. (i) What is the final temperature of the system? (ii) What is the remaining ice mass?
April 27, 2013 by Meder

Chemistry
Two 20.0-g ice cubes at 20.0 C are placed into 295 g 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. Heat capacity of H2O(s)=37.7J Heat capacity of H2O(l)=75.3J Enthalpy...
June 27, 2013 by Jessica

Chemistry
Calculate the final temperature of a mixture of 350g of ice cubes at -18 degrees C and 237 g of water at 100 degrees C
January 25, 2011 by nikita

Pages: 1 | 2 | 3 | 4 | 5 | 6 | 7 | 8 | 9 | 10 | 11 | 12 | 13 | 14 | 15 | Next>>

Search
Members