Thursday
April 17, 2014

Search: How much heat is required to change 456 g of ice at -25.0°C into water at 25.0°C? The specific heat of ice is 2090 J/(kg K) and the latent heat of fusion of water is 33.5 × 104 J/kg

Number of results: 139,084

Physics
Follow the following steps: 1. Calculate the ice block's mass from its volume and density. 2. Compute heat required to raise its temp. from -19.3 degC to 0 deg - Q1 3. Consider latent heat required to change the state from ice at 0 deg. to water at 0 deg. - Q2 3. Compute heat ...
Tuesday, July 31, 2012 at 8:08pm by Ajayb

Phase Changes
The heat of fusion of water is 335 J/g, the heat of vaporization of water is 2.26 kJ/g, the specifc heat of ice is 2.05 J/deg/g, the specific heat of steam is 2.08 J/deg/g and the specific heat of liquid water is 4.184 J/deg/g. How much heat would be needed to convert 10.73 g ...
Wednesday, May 8, 2013 at 12:41pm by Jenny

chemistry
the heat of fusion water is335 J/g. The heat of evaporization of water is 2.26 kJ/g, the specific heat of ice is 2.05 J/Deg/g, the specific heat of steam is 2.08 J/deg/g and the specific heat of liquid water is 4.184 J/deg/g. How much heat would be needed to convert 12.09 g of...
Tuesday, April 24, 2012 at 10:31pm by Randy

Chemistry
How much heat is required to change 10 grams of ice at 0 deg. C to steam at 100 deg C?
Tuesday, February 23, 2010 at 8:04pm by Ally

Chemistry
How much heat is required to change 10 g of ice at 0o deg C to steam at 100 deg. C?
Tuesday, February 23, 2010 at 8:05pm by Mari

Chemistry
I would check to see how much heat is required to change T of H2O from 62 to zero. mass H2O x specific heat water x delta T. Then see if you have that much heat from melting the ice. mass ice x heat fusion = ?? I thin you will have ice left over with ice at zero and water at ...
Saturday, April 25, 2009 at 1:38pm by DrBob222

chemistry
x = grams of ice x times heat of fusion of water in cal/gram = grams of water * specific heat of water in cal/deg gm * (25-5) ------------ That assumes that the ice is separated from the water. If they mix then the ice not only has to melt but also be raised from 0 to 5. Then...
Wednesday, January 27, 2010 at 3:10pm by Damon

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

Chemistry
Consider a 27.5g piece of ice at 0.00C. a) how much heat is required to convert the ice to water that is also 0.00 C? b) how much heat would be required to warm this water from 0.00 C to 17.50 C? I don't understand the process of how to go about solving this problem.
Sunday, September 7, 2008 at 4:14pm by Jeff

physics
An ice bag containing 0C ice is much more effective in absorbing heat than one containing the same amount of 0C water. (a) How much heat in kcal is required to raise the temperature of 0.700 kg of water from 0C to 27.0C? (b) How much heat is required to first melt 0.700 kg...
Friday, July 19, 2013 at 11:03pm by Eric

Chemistry
Calculate the heat (in kJ) required to change 40.0g of ice at -30.0 deg C to steam at 150.0 deg C?
Tuesday, March 6, 2012 at 8:03pm by Caitlin

Chemistry
Consider a 27.5 g piece of ice at 0.00 C. a) how much heat is required to convert the ice to water that is also 0.00 C? b) how much heat would be required to warm this water from 0.00 C to 17.50 C? HELP!! I think the fusion is 333 J/g at 0 C... But I'm not sure what to do with...
Sunday, September 7, 2008 at 2:04pm by Jeff

Chemistry
So we start with 50,000 joules heat. mass ice x specific heat ice x delta T = 20 g x 2.092 J/g x 5 = 209.2 which is much less than 50,000 and all of the ice will move from T = -5 to T = 0 C. To change ice at zero C to liquid water at zero C we newed mass ice x heat fusion 20g ...
Saturday, December 11, 2010 at 8:50pm by DrBob222

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...
Tuesday, April 9, 2013 at 7:28am by blur oh no

Physics
How much energy is required to change a 58 g ice cube from ice at −1◦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 3.33 105 J/kg, its latent heat of ...
Wednesday, January 30, 2013 at 5:59pm by Tiffany

chemistry
an 8.5g ice cube is placed into 255g of water. Calculate the temp change in the water upon the complete melting of the ice. Hint: Determine how much heat is absorbed by the melting ice and then use q = mc^T to calculate the temp change of the 255g of water
Sunday, October 23, 2011 at 12:23pm by Monique

Phyics
How much energy is required to change a 57 g ice cube from ice at −4◦C to steam at 107◦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 3.33 105 J/kg, its latent heat of ...
Monday, July 8, 2013 at 7:12pm by Beatles Lover

chemistry
how much heat is required to completely vapporize 2.3 grams of ice starting at -50 degrees Celsius? (the specific heat of ice is 2.0 J/g.C; the specific heat of water is 4.184 J/g.C; the heat of fusion is 333 J/g; and the heat of vaporization is 22601 J/g)
Tuesday, March 22, 2011 at 12:04am by Anonymous

College Physics
Dry Ice. At standard atmospheric pressure, the solid form of carbon dioxide called dry ice undergoes a phase change not to a liquid but straight to a gas. This process is called sublimation, and like other phase transitions heat energy is required. In this case it is the ...
Wednesday, November 30, 2011 at 8:50pm by Anon

chemistry
Heat a known mass of a metal to a known temperature (say, for example, 10.00 g at 78.5 deg C) Add the metal to a known mass of water at a known temperature (say 75.00 g at 25.0 deg C) in a calorimeter. Let the metal and the water come to an equilibrium temperature, Tf. (The ...
Tuesday, April 16, 2013 at 10:48pm by Rebekah

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

physics
There is a problem that asks if an ice cube is dropped into nitrogen (boiling point of nitrogen is 77K), how much nitrogen will evaporate? heat lost by ice = heat gained by nitrogen But by is the equation m(ice)*c(ice)*deltaT = m(nitrogen)*L(vaporation) ? Why isn't it m(ice)*c...
Thursday, April 21, 2011 at 5:09pm by Pegs

Chemistry
5.91 x 10^6J = [mass ice x specific heat ice x 14]+[(mass ice x heat fusion)]+[mass water x specific heat water x 13.7]. Change your 6.01 kJ/mol for heat fusion (I assume H2 stands for heat fusion) to J/g, substitute into the above and solve for grams ice. I get something like...
Saturday, April 3, 2010 at 3:46pm by DrBob222

Chemistry
22.) The molar heats of fusion and vaporization for water are 6.02 kJ/mol and 40.6 kJ/mol, respectively, and the specific heat capacity of liquid water is 4.18 J/gC. (1) What quantity of heat is required to melt 25.0 g of ice at 0C? (2) What quantity of heat is required to ...
Tuesday, March 5, 2013 at 8:33pm by Adriana

chemistry
How much mass of ice is there? You need the specific heats of ice and of water; the heat of vaporization, and the heat of fusion to answer this question. C,ice = 0.5 Cal/g C C,water = 1.0 Cal/g C H,fusion = 80 Cal/g H,vaporization = 540 Cal/g For Joules, multiply each by 4.184...
Thursday, March 18, 2010 at 2:25am by drwls

chemistry
a) how much heat is required to convert the ice to water that is also 0.00 C? b) how much heat would be required to warm this water from 0.00 C to 17.50 C? HELP!! I think the fusion is 333 J/g at 0 C... But I'm not sure what to do with that.
Sunday, September 7, 2008 at 3:28pm by Jeff

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

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 ...
Thursday, October 6, 2011 at 8:34pm by tanner

Chemistry
how much energy would be required to change 24.7g of ice to liquid water?the heat of fusion for water is 6.01 kj/mol?
Tuesday, January 18, 2011 at 10:49am by Anonymous

Chemistry
#4. The "protection" afforded by the ice is not so much from a shielding effect (I think a common misconception) as it is from the heat. Look at it this way, ice + heat ==> liquid water. So melting ice is an endothermic reaction; that is, you put heat in to melt the ice. So...
Thursday, January 21, 2010 at 8:01pm by DrBob222

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...
Monday, March 3, 2014 at 10:09am by Anonymous

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...
Wednesday, April 10, 2013 at 2:04am by ken

Chemistry
----------------- DrBob gave you a very good outline for solving this. I will give you a more detailed procedure without the final answer. I had already typed this offline several hours ago. I had to log off in hurry and did not transfer it here at the time...
Sunday, October 26, 2008 at 1:47pm by GK

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

Chemistry
How in the world did you come up with 1883.09J for moving water from 25 to zero? You don't have a mass of water. mass H2O x specific heat H2O x (Tf-Ti) = mass H2O x 4.184 x (25) = 104.6*mass H2O How much to freeze H2O. That's mass H2O x 334 = 334*mass H2O Let x = mass H2O and ...
Sunday, November 11, 2012 at 12:32am by DrBob222

Chemistry
How much heat is required to warm 229 g of ice from -45.3C to 0.0C, melt the ice, warm the water from 0.0C to 100.0C, boil the water, and heat the steam to 173.0C?
Sunday, April 22, 2012 at 3:03pm by Skrillex

Chemistry
How much heat did the water lose in going from 45 to 19.5 degrees? Mass x specific heat water x (Tfinal-Tinitial). How much heat did the ice gain? mass ice x heat fusion. heat lost + heat gain = 0. The only unknown is mass ice.
Friday, April 23, 2010 at 5:57pm by DrBob222

Chemistry
A quantity of ice at 0.0C was added to 25.6 g of water at 21.0C to give water at 0.0C. How much ice was added? The heat of fusion of water is 6.01 kJ/mol and the specific heat is 4.18 J/(g C). I dont understand how to set this problem up (what the formula is and where to...
Wednesday, October 8, 2008 at 10:57pm by Ryan

Chemistry
A quantity of ice at 0.0C was added to 25.6 g of water at 21.0C to give water at 0.0C. How much ice was added? The heat of fusion of water is 6.01 kJ/mol and the specific heat is 4.18 J/(g C). I dont understand how to set this problem up (what the formula is and where to...
Wednesday, October 8, 2008 at 11:00pm by Ryan

physics
how much heat is required to change 400g of ice at -20c into steam at 120c
Wednesday, October 6, 2010 at 5:05pm by steve

Chemistry
Ho much energy is needed to change a 50 g ice cube at 0 deg C to a liquid water at 100 deg. C?
Tuesday, February 23, 2010 at 5:44pm by Christopher

Urgent-Chemistry Help
I need help with the heat effects and calorimetry worksheet. Please explain how to solve it! Thank you so much! A metal sample weighing 45.2g and at a temperature of 100.0 C was placed in 38.6g of water in a calorimeter at 25.6 C. At equilibrium the temperature of the water ...
Monday, December 4, 2006 at 1:25am by Tiffany

How do I solve for this??
H (joules) =ΔT*m*Q where H=energy required (joules) ΔT=change in temperature (°C) m=mass (g) Q=specific heat in j/°C/g So heat gain =12.67 °C * 100 g * 4.180 j/°C/g =5296 j
Monday, June 24, 2013 at 7:28am by MathMate

chemistry
The heat of fusion of water is 335 J/g, the heat of vaporization of water is 2.26 kJ/g, and the specific heat of water is 4.184 J/deg/g. How many grams of ice at 0 could be converted to steam at 100 C by 9,946 Joules of heat?
Friday, November 15, 2013 at 4:31pm by Dakota

Chemistry
A quantity of ice at 0.0C was added to 25.0 g of water at 21.0C to give water at 0.0C. How much ice was added? The heat of fusion of water is 6.01 kJ/mol and the specific heat is 4.18 J/(g C). _g
Saturday, January 28, 2012 at 12:10pm by jessica

Chemistry
How much heat energy, in kilojoules, is required to convert 53.0 g of ice at -18.C to water at 25.0 C ?
Friday, December 9, 2011 at 6:57pm by Morgan

Chemistry
How much heat did the water lose? mass water x specific heat water x (Tfinal-Tinitial). How much heat did the ice gain? mass ice x heat fusion. The sum of those should be zero.
Wednesday, April 21, 2010 at 12:37am by DrBob222

Physics
Because ice can absorb more heat from the soft drink to change its state from ice to water (latent heat), than water only. If you use the equation for heat released/absorbed, Let T2 = final temperature of ice (assume it's above 0C, so it became water at some temp > 0C) ...
Sunday, December 1, 2013 at 7:51pm by Jai

Chemisty
In an experiment, 23.0 g of ice at 25C is converted into steam with a temperature of 124C. How much heat is required for the process? The following data may be of use: vap = 2260 J/g; Hfus = 334 J/g; Cp(ice) = 2.06 J/g C; Cp(water) = 4.18 J/g C...
Thursday, April 8, 2010 at 11:17am by Stephen

physics
how much heat is required to vaporize 7 grams of ice initially at 0 degrees celsius when the latent fusion of ice is 80 cal/g, the vaporization of water is 540 cal/g, and the specific heat of water is 1 cal/(g x C)?
Friday, February 19, 2010 at 11:03pm by elisabeth

Physics
How much heat energy is required to convert 0.1000kg of ice at -10.0 C into water at 50 C?
Thursday, December 8, 2011 at 2:37am by Dorrito

chem
.You have an ice cube that is 150 g and is at a temperature of 0C. You drop the ice into water that is initially at 15C and the ice melts. As a result, the water cools of by exactly 1C to become 14C. How much water was there? In other words, what mass of water at 15C can ...
Wednesday, September 12, 2012 at 9:34am by chuck

Chemistry
I asked my professor and she said when the ice cube melts, it absorbs energy from the water. We can figure out how much energy using the heat of fusion. The water cools down; since we know how much energy it lost, how much mass it has (including the mass of the ice cube, now...
Friday, April 27, 2012 at 8:06pm by Anonymous

chemistry
x = grams of ice x times heat of fusion of water in cal/gram = grams of water * specific heat of water in cal/deg gm * (25-5)
Wednesday, January 27, 2010 at 3:10pm by Damon

Chemistry
heat to melt ice at zero C = 850 x heat fusion = ? heat removed from 35 C water = 1,700 x specific heat water x (0-35) = ? I get about 280,000 J to melt the ice and about 250,000 J from the water. The ice won't melt completely. The end solution will be a mixture of ice and ...
Sunday, January 29, 2012 at 4:52pm by DrBob222

CHEMISTRY
How much heat is needed to melt 150g of ice? and How much heat is needed to change 150g of ice into steam at 110 degrees? My heat of fusion is 361 and my percent error is 8 if you need that. Answers quickly please :(
Tuesday, March 8, 2011 at 8:00am by TaShe

Active physics
I think you mean heat, not hear. Add the heat required for the following steps: (1) heat ice from -25C to 0 C (2) melt the ice (3) heat water from 0 C to 100 C (4) vaporize the water to steam (5) heat the steam from 110 C to 119 C. (Assume constant pressure) You will need the ...
Monday, May 9, 2011 at 9:00am by drwls

Chemistry
q1 = heat necessary to change ice from -10 to zero = mass x specific heat ice x (Tfinal - Tinitial) where Tfinal is zero and Tinitial is -10. q2 = heat necessary to melt ice but stay at zero = mass x heat fusion of ice. q3= heat necessary to heat water at zero to 25 C. = mass ...
Monday, December 24, 2007 at 5:25pm by DrBob222

Physics
Assume a thermal equilibrium temp. T and find the heat absorbed by ice (say Q1)to raise its temp.from -35 deg. to T deg. Similarly, find heat released by water (say Q2) when its temp. lowers from 45 deg. to T deg. Putting Q1 = Q2 will give you T in deg. C. Note: Do not forget ...
Tuesday, July 31, 2012 at 8:09pm by Ajayb

Physics
2. Suppose you pour 15 g of hot water (at 55 oC) into a glass that contains 20 g of ice (at - 10 oC). Neglect the heat absorbed in the glass itself. a. How much heat would the water give up to get cooled to the melting point? b. How much heat would it take to get the ice to ...
Monday, November 19, 2012 at 10:10am by Jonathan

Physics
Suppose you pour 15 g of hot water (at 55 oC) into a glass that contains 20 g of ice (at - 10 oC). Neglect the heat absorbed in the glass itself. a. How much heat would the water give up to get cooled to the melting point? b. How much heat would it take to get the ice to the ...
Monday, November 19, 2012 at 10:10am by Jonathan

Physics HELP!
2. Suppose you pour 15 g of hot water (at 55 oC) into a glass that contains 20 g of ice (at - 10 oC). Neglect the heat absorbed in the glass itself. a. How much heat would the water give up to get cooled to the melting point? b. How much heat would it take to get the ice to ...
Monday, November 19, 2012 at 6:34pm by Jonathan

Chemistry
First the ice cube must be heated from -10 C to zero C. q = mass x specific heat x delta T. This will give you the heat required to do just that. Subtract q required from 340 J to obtain the heat remaining to melt the ice cube. Then q = mass x heat of fusion for ice. Plug in q...
Tuesday, January 15, 2008 at 11:46pm by DrBob222

chemistry
calculate the energy, in joules and calories required to heat 25.0g of water form 12.5 deg. celcius to 25.7 deg. celcius i know the answer just need to see how to do it especially the calories
Sunday, January 22, 2012 at 6:58pm by shaun

Physics
How much heat is required to bring the block of ice up to 0C? How much heat is required to melt the ice at 0C? If there is heat left over, then final temp can be calculated by Heatleftover=10kg*specificheatwater(Tf-0) solve for Tf. The statement "the block absorbs 4.10106 J of...
Sunday, April 6, 2008 at 9:01am by bobpursley

Chemistry
How much heat is required to change 2.5kg of ice at 0.0 degrees C to water at 50 degrees C?
Wednesday, October 20, 2010 at 11:45am by Cat

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

Chemistry
heat absorbed moving ice from -15 to zero + heat absorbed by ice melting + heat absorbed by moving ice from zero to final T - heat lost by 1L water initially at 25 C = 0. [mass ice x specific heat ice x (Tfinal-Tinitial)] + [mass ice x heat fusion] + [mass melted ice x ...
Monday, May 23, 2011 at 6:13pm by DrBob222

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 ...
Thursday, April 26, 2007 at 2:01am by jean

Physcial Science
Hey There, I have 4 questions that I am totally stumped on... Can anyone help? A 200-gram chunk of stuff rises in temperature by 3oC when you input 1200 calories of heat. What is its specific heat capacity? Answers A)50 cal/goC. B) 2 cal/goC. C) 5 cal/goC. D) 0.02 cal/goC. You...
Friday, September 23, 2011 at 11:11am by Anonymous

Physcial Science
Hey There, I have 4 questions that I am totally stumped on... Can anyone help? A 200-gram chunk of stuff rises in temperature by 3oC when you input 1200 calories of heat. What is its specific heat capacity? Answers A)50 cal/goC. B) 2 cal/goC. C) 5 cal/goC. D) 0.02 cal/goC. You...
Friday, September 23, 2011 at 11:20am by Anonymous

Physcial Science
Hey There, I have 4 questions that I am totally stumped on... Can anyone help? A 200-gram chunk of stuff rises in temperature by 3oC when you input 1200 calories of heat. What is its specific heat capacity? Answers A)50 cal/goC. B) 2 cal/goC. C) 5 cal/goC. D) 0.02 cal/goC. You...
Friday, September 23, 2011 at 11:37am by Anonymous

CBSE
How much heat must be removed to change 75.0 grams of water at 25.0 C to ice at -35.0 C?
Sunday, April 29, 2012 at 2:00am by tulasi

Chemistry
How much heat is required to warm 225g of ice from -48.6C melt the ice warm the water from 0.0C to 100.0C boil the water and heat the steam to 173.0C
Monday, February 22, 2010 at 11:28pm by Anonymous

Chemistry
q1=heat to move ice from -25 to zero C. (Not the correct spelling of celsius). q1 = mass ice x specific heat ice x (Tfinal-Tinitial). Tfinal = zero and Tinitial = -25 q2 = heat to melt ice at zero to liquid water at zero c. q2 = mass ice x heat fusion q3 = heat to move water ...
Saturday, July 31, 2010 at 2:49pm by DrBob222

science
Do you know the specific heat of solid water (ice)? If so, then it will take q calories = mass ice x specific heat ice x (0+10) to raise T from -10 C to zero C. Subtract that from 4500 to see how much(if any) heat is left. If some heat is available, then it can go to melting ...
Tuesday, January 3, 2012 at 3:20pm by DrBob222

Physics
Trying to beat the heat of summer, a physics grad student went to the local toy store and purchased a child's plastic swimming pool. Upon returning home, he filled it with 154 liters of water at 25C. Realizing that the water would probably not be cool enough, he threw ice ...
Saturday, November 20, 2010 at 3:37pm by BG

Physics
Latent heat question: Your car's windshield is covered with a .58 cm thick layer of ice. The ice has an area of 1.6m^2. If the temperature of the ice is -2C, how much heat is required to melt all the ice?
Wednesday, December 1, 2010 at 7:57pm by Anonymous

physics
A woman finds the front windshield of her car covered with ice at -12.6C. The ice has a thickness of 4.80 10-4 m, and the windshield has an area of 1.25 m2. The density of ice is 917 kg/m3. How much heat is required to melt the ice?
Monday, April 14, 2008 at 4:03pm by Jaime

Chemistry
I believe I worked that problem yesterday. Perhaps not for you. heat needed to move T of ice from -10 to 0 q1 = mass x specific heat ice x delta T heat needed to melt the ice. q2 = mass x heat of fusion. heat needed to move T from 0 to 25. q3 = mass x specific heat water x ...
Thursday, January 17, 2008 at 11:03pm by DrBob222

chemistry
q1 = heat required to raise T of ice from -30 to O C. q1 = mass of ice x specific heat ice x (Tf - Ti) where Tf is final T (O) and Ti is initial T (-30). q2 = heat required to melt the ice at zero; i.e., change from solid phase to liquid phase. q2 = mass of ice x heat fusion. ...
Tuesday, October 23, 2007 at 6:07pm by DrBob222

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

ap chemistry
the molar heat of fusion for water is 6.01 kJ/mol. the heat capacity for water is 75 J/mol deg. Which expresssion gives the quantity of energy needed to change one mol ice at 0 degrees celsius to liquid water at 25 degrees celsius? a.)6010/(75x25) b.)6.01+75 c.)6010+(75+25) d...
Friday, September 24, 2010 at 8:22pm by Sarah

Chemistry
the heat of fusion water is 335J/g,the heat of vaporization of water is 2.26kJ/g, the specific heat of water is 4.184J/deg/g. how many grams of ice at 0 degrees could be converted to steam at 100 degrees C by 9,574J
Friday, April 27, 2012 at 10:15pm by Randy

Physics
I'm trying to determine the specific heat of copper by experiment and I have a question about the change in temperature of the copper. If I take the copper out of boiling water at 100 deg. C and place it in water at 10 degrees C, the temp. of the water increases to 14 deg. Is ...
Thursday, May 7, 2009 at 3:26pm by Brigid

physics
q1 = heat to move ice from -20 to zero. q1 = mass ice x specific heat ice x (Tfinal-Tinitial). [Tf will be 0 and Ti will be -20 but watch that sign since it will change. q2 = heat to melt the ice. q2 = mass ice x heat fusion. q3 = heat to move ice from zero to 58. q3 = mass ...
Thursday, November 27, 2008 at 12:20pm by DrBob222

physics
Heat releasing from coffee (water in this case) is equal to the heat gain for ice melting to water at 0 deg plus water to raise for the final temp.
Sunday, December 4, 2011 at 7:58am by Shahiahi

Chemistry
How much heat must be removed from the 25.6 g H2O @ 21.0.0 C to move it to 0.0 C. That will be q = heat to be removed = mass x specific heat water x delta T. q = 25.6 g x 4.18 x 21.0 = about 2000 J (but you need to do it exactly). Then 2000 J x 1 g/heat fusion = grams ice. You...
Wednesday, October 8, 2008 at 10:57pm by DrBob222

chemistry
the heat of fusion of water is 335 J/g. How much heat would be required to melt 97.8 g of ice
Tuesday, April 24, 2012 at 10:00pm by Randy

Chemistry
q1 = heat required to change T from 25 C to 100 c. q1 = mass H2O x specific heat water x delta T. q2 = heat required to change liquid water at 100 C to steam at 100 C. q2 = mass H2O x heat vaporization total heat = q1 + q2.
Saturday, April 25, 2009 at 1:35pm by DrBob222

physics
Add the heat required for five separate processes: (1) Heating the ice from -20 to 0 C (2) Melting the ice at 0 C (3) Heating the water to 100 C (4) Evaporating the water at 100 C (5) Heating the steam from 100 to 120 C. For (1) and (5) you will need the specific heats of ice ...
Wednesday, October 6, 2010 at 5:05pm by drwls

Physics - calorie
The calorie was defined in 1824 and is meant to the the heat required to raise the temperature of pure water by 1°C. The kcal, or Calorie, or kilocalorie is meant to be 1000 calories, or the amount of heat required to raise the temperature of 1 kg of water by 1°C.
Sunday, September 20, 2009 at 4:45pm by MathMate

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
How much heat energy, in kilojoules, is required to convert 36.0g of ice at 18.0C to water at 25.0C
Wednesday, January 30, 2013 at 6:20pm by Ashley

Chemistry
How much heat in kJ is required to melt 54 grams of ice at 0 degrees C into water at 0 degrees C if delta Hvap for water = 6.01 kJ/mol?
Tuesday, December 14, 2010 at 5:10pm by Hannah

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

physic
How much energy is required to change a 40 g ice cube from ice at -25C to steam at 105C?
Sunday, April 6, 2014 at 8:33pm by Renee

Physics
How much heat is added to a 10.0 g of ice at -20.0 degrees Celsius to convert it to steam at 120.0 degrees Celsius? compute and add the following heats: heat to heat ice from -20C to 0C heat to melt ice at 0C Heat to heat water from 0 to 100C heat to convert water to steam at ...
Monday, March 5, 2007 at 7:45pm by Marie

Chemistry
heat to melt ice + heat to cool water (will be negative) from 29 + heat to heat ice to final T (positive number) = 0 [mass ice x heat fusion] + [mass water x specific heat water x (Tfinal-Tinitial)] + [mass liquid from ice x specific heat water x (Tfinal-Tinitial) = 0 Solve ...
Tuesday, February 23, 2010 at 2:02am by DrBob222

Physics
How much heat do you get out of steam when it goes from vapor (steam) to liquid water. Isn't that the heat of vaporization? I think it's something like 2257 J/g but you need to confirm that. If you have 10 g steam then the heat available to melt the ice is 10 g x 2257 J/g = ...
Wednesday, September 23, 2009 at 1:27pm by DrBob222

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

Search
Members