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April 19, 2014

Search: how much heat is required to vaporize 1.00 L

Number of results: 64,143

CHEM
A 60.0 sample of water is heated to its boiling point. How much heat (in ) is required to vaporize it? (Assume a density of 1.00 .)
Thursday, September 2, 2010 at 8:05pm by Anonymous

chemistry
65.0 mL of water is heated to its boiling point. How much heat in Kj is required to vaporize it? (Assume a density of 1.00 g/mL)
Friday, September 10, 2010 at 9:08pm by jessa

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
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
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

material science
How much heat (in BTU) would be required to heat and vaporize 100 lb of water from 25C to saturated steam at 1 atm? Assume heat capacity is constant at 1 BTU/lb-F and the latent heat of vaporization is 1,000 BTU/lb
Wednesday, January 19, 2011 at 8:37am by zura

chemistry!
The standard molar heat of vaporization for water is 40.79 kJ/mol. How much energy would be required to vaporize 4.00 mol of water? Answer in units of kJ
Thursday, March 8, 2012 at 8:44pm by urgent

Chemistry
how much heat is required to vaporize 343 g of liquid ethanol at its boiling point?
Thursday, April 8, 2010 at 4:44pm by Anonymous

chemistry
how much heat is required to vaporize 343g of liquid ethanol at its boiling point?
Monday, March 25, 2013 at 12:25pm by tanya

Chemestry
How much heat (in kJ}) is required to vaporize it? (Assume a density of 1.00 g/mL ) I have this 60.0ML/ 1.00 g/ml = 60grams 60/153/81 g/mol = .3900916715 moles .3900916715 moles / 43.9 kj/mol = 17.122 And it keeps telling me the answer is wrong.
Sunday, January 25, 2009 at 9:41pm by Creative9k

chem
how much heat is required to vaporize 34.8g of water at 100 degrees celcious?
Friday, November 16, 2012 at 12:46pm by law-rece

Chemstry Help Drbob!
How much heat (in kJ}) is required to vaporize it? (Assume a density of 1.00 g/mL ) I have this 60.0ML/ 1.00 g/ml = 60grams 60/153/81 g/mol = .3900916715 moles .3900916715 moles / 43.9 kj/mol = 17.122 And it keeps telling me the answer is wrong.
Sunday, January 25, 2009 at 9:41pm by Creative9k

Chemistry
When 25.0 g of ethanol vapor condenses, 23.6 kJ of heat is released. How much heat is required in kJ to vaporize 254 g of ethanol?
Wednesday, October 13, 2010 at 7:36pm by Jordin

chemistry
The enthalpy of vaporization at 298 K for diethylether (C4H10C) is 26.0 kj/mol. How much heat would be required to vaporize 1.00 L of the ether at 298 K if its density is 0.714 g/L ? A) 250 kj B) 74.1 kj C) 186 kj D) 130 kj E) 440 kj
Monday, June 21, 2010 at 2:28pm by Jim

Physics
the pressure is one atmosphere and determine the heat in joules required to produce 5.03 kg of water vapor at 100.0 C, starting with (a) 5.03 kg of water at 100.0 C and (b) 5.03 kg of liquid water at 0.0 C. for part (a) I used the equation Q=mL and L was a given value but I...
Friday, November 17, 2006 at 7:02pm by Jena

Chemistry
How much heat is required to vaporize 343g of liquid ethanol at its boiling point? ΔHvap+38.6 Kj\mol
Monday, February 22, 2010 at 11:26pm by Anonymous

heat of vaporization
1) Convert the 1.00 g of C3H8O to moles. (60 g per mole) 2) Compute the energy required to vaporize 1/60 mole (45.4/50 = 0.757 kJ). Call it Q 3) Compute the drop in temperature of the Al block when that amount of heat is removed. (delta T = Q/(M C) )
Saturday, January 16, 2010 at 2:35pm by drwls

Chemistry
How much heat (in BTU) would be required to heat and vaporize 100 lb of water from 25C to saturated steam at 1 atm? Assume heat capacity is constant at 1 BTU/lb-F and the latent heat of vaporization is 1,000 BTU/lb. Also, what is the temperature of the saturated steam at 1 atm?
Monday, January 17, 2011 at 7:14am by Jini

enthalpy change
The heat required to raise the beaker temperature will be 3/4 as much the second time, becasue of the delta-T rTIO. The heat required to heat the liquid will be higher by a factor (200/250)(2.43/0.67) = 2.90 Calculate the total heat required in the second case. The ratio (heat...
Sunday, October 10, 2010 at 6:30pm by drwls

chemistry
How much energy is required to vaporize 75.5 mL of ethanol (C2H5OH, d=0.789 g/cm^3) at its boiling point, if its heat of vaporization is 40.5 kJ/mol?
Sunday, September 30, 2012 at 5:48pm by Brunette

Chemistry
how much kj of heat are required to vaporize 42.8 grams of c3 h10 o (deltaH vap=26.5 kj/mol)
Saturday, October 9, 2010 at 10:43am by jesse

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

Chemistry
The heat of vaporization of benzene, C6H6, is 30.8kJ/mol at its boiling point of 80.1 degrees celsius. How much energy in the form of heat is required to vaporize 102g of benzene at its boiling point? I know that the answer is 24.2kJ but i am not sure how to get this.
Sunday, February 5, 2012 at 12:16pm by Hannah

chemistry
a 50.0 ml sample of water is heated to its boiling point. how much heat (in KJ) is required to vaporize it? (assume a density of 1.00g/ml).
Saturday, February 7, 2009 at 9:14pm by reese

AP Chemistry
Convert 93 gallons H2O to grams. I would use 1 gallon = 3.785 L, convert to mL then use density of 1.00 g/mL to solve for grams. How much heat is required to heat this much water (in grams) from 60 F to 99 F. Convert 60 F and 99 F to C using (F-32)*5/9 = C. Then q = heat ...
Friday, October 11, 2013 at 6:09pm by DrBob222

Chemistry
How much heat, in Kj, is required to melt 11.0g of ice, at -13.0 degrees C, and vaporize the H20, and rise the temperature of the steam to 114 degrees C. Need help. Anyone, please!
Monday, November 19, 2012 at 12:38am by Shelby

chem
How much heat is required to raise the temperature of 200 g CH3OH from 20 to 30 degrees and then vaporize it at 30 degrees. The molar heat capacity of CH3OH is 81.1 J/Mol/K. Okay...the answer is approximately around 254. It was a homework problem. The question is how do you ...
Monday, February 15, 2010 at 4:46pm by joseph

chemistry
484 kJ heat released from 4 g hydrogen. 44.0 kJ heat used to vaporize the water/mole or 88 kJ heat used to vaporize 4 g hydrogen. 484-88 = 396 kJ net heat released. So We need 484 x (x grams/4) = 7.46 g hydrogen burned to produce the 396 kJ. Solve for x THEN CHECK IT TO MAKE ...
Sunday, October 31, 2010 at 5:16pm by DrBob222

chemistry
What quantity of heat is required to vaporize 32.5 g of liquid water at 100C?
Tuesday, February 16, 2010 at 6:24pm by Emily

phys
How many kcal of heat are required to vaporize 25.0 kg of water at 100C?
Thursday, December 15, 2011 at 4:08pm by Dennis

Physics
How many kcal of heat are required to vaporize 25.0kg of water at 100C?
Monday, April 2, 2012 at 12:22pm by Madison

chemistry
Ammonia, NH3, is used as a refrigerant. At its boiling point of -33C, the enthalpy of vaporization of ammonia is 23.3 kJ/mol. How much heat is required to vaporize 125 g of ammonia at -33C?
Wednesday, May 12, 2010 at 6:12pm by b

chemistry
How much heat is required to raise the temperature of 200 g CH3OH from 20 to 30 degrees and then vaporize it at 30 degrees. The molar heat capacity of CH3OH is 81.1 J/Mol/K. Okay...the answer is approximately around 254. It was a homework problem. The question is how do you ...
Saturday, February 13, 2010 at 8:42pm by joseph

chemistry
How much heat is required to raise the temperature of 200 g CH3OH from 20 to 30 degrees and then vaporize it at 30 degrees. The molar heat capacity of CH3OH is 81.1 J/Mol/K. Okay...the answer is approximately around 254. It was a homework problem. The question is how do you ...
Saturday, February 13, 2010 at 9:37pm by joseph

chem
The standard molar heat of vaporiza- tion for water is 40.79 kJ/mol. How much energy would be required to vaporize 2.54 1010 molecules of water? Answer in units of kJ
Thursday, March 1, 2012 at 5:41pm by sammy

Chemistry
Compare the amount of heat required to vaporize a 200.-gram sample of H20(L) at its boiling point to the amount of heat required to melt a 200.-gram sample ofH20(s) at its melting point.
Saturday, October 9, 2010 at 10:43am by danny123

chemistry
what quantity of heat is required to vaporize 141 g of benzene at its boiling point 80.1 degrees celcius? heat of vaporization is 30.8 degrees celcius.
Thursday, January 20, 2011 at 8:00pm by Angela

Chemistry
How much heat is required to vaporize 1.00 L of CCl4 at its normal boiling point? The following data are given for CCl4. Normal melting point, -23 degree celcius , normal boiling point, 77 degree celcius density of liquid 1.59 g/mL; ; enthalpy of fusion 3.28 kJ/mol vapor ...
Monday, December 8, 2008 at 7:50pm by Ashleigh

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
Then tell me what you don't understand. All you need to do is to substitute the mass of 65.0 mL water (65.0 grams) and surely you have a table giving the heat vaporization of water. That calculates q, the heat required to vaporize water at it's boiling point. How did I get the...
Friday, September 10, 2010 at 9:08pm by DrBob222

chemistry
Some properties of aluminum are summarized in the following list. normal melting point 658C heat of fusion 0.395 kJ/g normal boiling point 2467C heat of vaporization 10.52 kJ/g specific heat of the solid 0.902 J/gC (a) Calculate the quantity of energy required to heat 1.75 ...
Saturday, May 1, 2010 at 5:54pm by Jake

Chemistry
Some properties of aluminum are summarized in the following list. normal melting point 658C heat of fusion 0.395 kJ/g normal boiling point 2467C heat of vaporization 10.52 kJ/g specific heat of the solid 0.902 J/gC (a) Calculate the quantity of energy required to heat 1.75 ...
Saturday, May 1, 2010 at 6:46pm by Charles

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
Liquid Butane, C4H10, is stored in cylinders to be used as a fuel. Suppose 39.3g of butane gas is removed from a cylinder. How much heat must be provided to vaporize this much gas? The heat of vaporization of butane is 21.3 kJ/mol.
Thursday, January 31, 2008 at 8:52pm by Lauren

Chemistry
Liquid Butane, C4H10, is stored in cylinders to be used as a fuel. Suppose 39.3g of butane gas is removed from a cylinder. How much heat must be provided to vaporize this much gas? The heat of vaporization of butane is 21.3 kJ/mol.
Thursday, January 31, 2008 at 10:00pm by Lauren

Chemistry
The molar heat of vaporization of ethanol is 43.5 kJ/mo. Calculate the heat required to vaporize 25.0 g of ethanol at its boiling point. Ethanol is (2C 5H OH) Could someone please write the equation? (is the equation q=CmT)
Tuesday, May 18, 2010 at 11:04pm by Anonymous

Chermistry
if molar enthalpy of vaporization of enthanol is 38.6 kJ/mol, how many moles of ethanol are vaporize when required heat is 200.72kJ
Tuesday, August 31, 2010 at 9:44am by Paris

Chemistry
How much heat is required to raise T of solid ethanol from -130 to -114? That will be mass ethanol x specific heat solid ethanol x (Tf-Ti) = ? How much heat has is left? 5870 J - ? = x How much heat is required to melt the ethanol. That is mass ethanol x heat fusion = y x-y = ...
Thursday, April 25, 2013 at 11:52pm by DrBob222

9th grade
add the following energyies: heat to heat ice at -10 to 0 heat to melt 20 g ice at 0C Heat to heat water from 0C to 100C heat to vaporize 20gwater at 100C. heat to heat steam from 100C to 200C
Tuesday, January 5, 2010 at 6:46pm by bobpursley

science
how matter can change from one form to another. Heat causes solids to melt, and more heat causes them to vaporize. Is this what you meant? Heat causes solids to melt, and more heat causes them to vaporize. Is this what you meant?
Friday, July 6, 2007 at 9:27pm by Anonymous

chem: gases, liquids, solids
q1 = heat to move H2O from T = 32 C to 100 C. q1 = mass water x specific heat water x (Tfinal-Tinitial) q2 = heat to vaporize water at 100 to steam at 100. q2 = mass water x delta Hvap. Total heat required = q1 + q2.
Tuesday, November 30, 2010 at 11:11pm by DrBob222

Chemistry
Ethane, C2H6, has a molar heat of vaporization of 15kJ/mole. How many kilojoules or energy are required to vaporize 5 g of ethane?
Tuesday, May 1, 2012 at 12:30pm by Ambra

chemistry
Ethane, C2H6, has a molar heat of vaporization of 15 kJ/mole. How many kilojoules or energy are required to vaporize 5 g of ethane?
Tuesday, December 1, 2009 at 7:13pm by tt

Chemistry
Ethane, C2H6 has a molar heat of vaporization of 15 kj/moles. How many kilojoules of energy are required to vaporize 5 grams of Ethane?
Monday, July 21, 2008 at 2:28pm by Persia

chemistry
If you need only the heat required to vaporize it, then most of the data provided is not useful (heat fusion, etc). First, convert 3.50 L to grams using the density listed. I looked up the heat of vap on the web and found 32.54 kJ/mol. Change that to J/gram 32.54 kJ/mol x (1 ...
Monday, December 8, 2008 at 3:14pm by DrBob222

chemistry
How much heat is required? 1.5 g x heat vaporization = q. Now if heat is added at 24.0 J/s, how many seconds will it take?
Wednesday, January 20, 2010 at 7:04pm by DrBob222

Chemistry please help
Energy/photon = hc/wavelength. Remember to change wavelength meters and use c in m/s. heat required = mass x density x specific heat x delta T. Everything is here to calculate heat required. Knowing heat/photon and the total energy required you can calculate the number of ...
Monday, November 3, 2008 at 9:51pm by DrBob222

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

Physics
figure this in three parts: heat to heat water from 25C to 100C heat to vaporize water at 100C heat to heat steam from 100C to 120C add them
Thursday, November 18, 2010 at 8:46pm by bobpursley

chemistry
q = mass x specific heat x (Tfinal-Tinitial) Note that you list the specific heat Fe but ask for how much heat is required to heat Al. You may have mixed two problems.
Wednesday, April 4, 2012 at 1:26pm by DrBob222

chemistry
How much heat is required to vaporize 3.50L of at its normal boiling point? The following data are given for Carbon Tetrachloride. Normal melting point, -23 Degrees Celsius, normal boiling point, 77 Degrees Celsius; density of liquid, 1.59g/mL; Delta H (FUSION): 3.28 kJ mol^-1...
Monday, December 8, 2008 at 3:14pm by Linda

chemistry
How much heat is required to vaporize 3.50L of at its normal boiling point? The following data are given for Carbon Tetrachloride. Normal melting point, -23 Degrees Celsius, normal boiling point, 77 Degrees Celsius; density of liquid, 1.59g/mL; Delta H (FUSION): 3.28 kJ mol^-1...
Monday, December 8, 2008 at 3:14pm by Linda

IPC
The latent heat of vaporization of water is 540 calories/gram. How many calories are required to completely vaporize 500 grams of water?
Tuesday, October 12, 2010 at 11:10am by Katy

science
The latent heat of vaporization of water is 540 calories/gram. How many calories are required to completely vaporize 500 grams of water?
Wednesday, June 5, 2013 at 9:16am by Quan

chemistry
q1 = heat required to move T from zero C to 100 C. q1 = mass water x specific heat water x (Tfinal-Tinitial). Tf = 100 C; Ti = 0 C. q2 = heat to vaporize liquid water @ 100 C to steam at 100 C. q2 = mass water x delta Hvap. qtotal = q1 + q2.
Monday, November 29, 2010 at 5:29pm by DrBob222

physics
Calculate the quantity of heat required to raise the temperature of 2.00 g of water 4.00◦C.
Tuesday, July 5, 2011 at 9:10pm by angel

11th grade
The latent heat of vaporization of water is 540 calories/gram. How many calories are required to completely vaporize 500 grams of water?
Tuesday, May 4, 2010 at 11:08am by katlyn

Chemistry
I will be happy to check your work. Do these in order (heat ice to OC), melt ice, heat water to 100C, vaporize, heat steam.
Saturday, April 17, 2010 at 8:46pm by bobpursley

Chemistry
Calculate the amount of heat (in calories) required to raise the temperature of 200g of water from 20C to 50C. The specific heat of water is 1.00 cal/g. I have done other spacific heat problems but on this one i don't know how to start...
Tuesday, November 10, 2009 at 7:08pm by Christina

physics
(a) How much heat (J) flows from 1.00 kg of water at 46.0C when it is placed in contact with 1.00 kg of 18C water in reaching equilibrium? (b) What is the change(J/K) in entropy due to this heat transfer? (c) How much work (J) is made unavailable, taking the lowest ...
Thursday, July 25, 2013 at 11:57pm by Justin

physics
(a) How much heat (J) flows from 1.00 kg of water at 46.0C when it is placed in contact with 1.00 kg of 18C water in reaching equilibrium? (b) What is the change(J/K) in entropy due to this heat transfer? (c) How much work (J) is made unavailable, taking the lowest ...
Friday, July 26, 2013 at 2:09pm by Justin

physics
(a) How much heat flows from 1.00 kg of water at 46.0C when it is placed in contact with 1.00 kg of 18C water in reaching equilibrium? (b) What is the change in entropy due to this heat transfer? (c) How much work is made unavailable, taking the lowest temperature to be 18C?
Sunday, July 28, 2013 at 3:53pm by Justin

physics
(a) How much heat (J) flows from 1.00 kg of water at 46.0C when it is placed in contact with 1.00 kg of 18C water in reaching equilibrium? (b) What is the change(J/K) in entropy due to this heat transfer? (c) How much work (J) is made unavailable, taking the lowest ...
Sunday, July 28, 2013 at 1:33am by Justin

physics
(a) How much heat (J) flows from 1.00 kg of water at 46.0C when it is placed in contact with 1.00 kg of 18C water in reaching equilibrium? (b) What is the change(J/K) in entropy due to this heat transfer? (c) How much work (J) is made unavailable, taking the lowest ...
Sunday, July 28, 2013 at 5:34pm by Justin

AP Chemistry
Ammonia, NH3, is used as a refrigerant. At its boiling point of -33 degress Celcius, the enthalpy of vaporization of ammonia is 23.3 kJ/mol. How much heat is required to vaporize 355 g of ammonia at -33 degrees Celcius? a. 1.12 kJ b. 152 kJ c. 251 kJ d. 486 kJ e. 8.27 x 10^3 kJ
Friday, April 4, 2008 at 10:18am by Joe

Chemistry
add the heat to warm the water to 100C, to the heat to vaporize it.
Thursday, February 3, 2011 at 8:01am by bobpursley

Physical Science
I studied this 2 years ago in college and am no back in school. I can't remember any of this stuff and I really need to figure it out. Please Help Me!! The Latent Heat of Vaporization for water is 540. cal/g. How much heat (in calories) must be added to 10.0 g of water at ...
Tuesday, February 5, 2013 at 10:05pm by Jessica

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

CHEM-vaporization
The iron will lose this much energy upon cooling to 100C: .45 J*g^-1*K^-1 * 50g * 52K = 1170 J The water will gain this much energy when heating to 100C 4.21 J*g^-1*K^-1 * 20g * 11K = 926.2 J The difference in those energies will be used to vaporize water: 1170 J - 926.2 J = ...
Friday, February 6, 2009 at 1:20pm by chemstudent

Physics
A 100 kg steam boiler is made of steel and contains 200 kg of water at 5.00C. How much heat is required to raise the temperature of both the boiler and water to 100C? The specific heat of Steel is 0.115kcal/kgC. The specific heat of Water is 1.00kcal/kgC
Monday, April 2, 2012 at 11:54am by Madison

Chemistry
How much energy in kilocalories is needed to vaporize 255g of water? The heat of vaporization of water is 540 cal/g.
Wednesday, April 10, 2013 at 11:14pm by Ryan

Chemistry
OK. You have 50,000 Joules of heat. How much heat do you need to move the temperature of the ice at -5.00 C to zero C? q = mass ice x specific heat ice x (0-(-5)) = ??. Solve for q and subtract joules from 50,000. What's left? Now how much does it take to melt 20 g ice? That's...
Saturday, December 11, 2010 at 8:50pm by DrBob222

specific heat capacity
How much heat would be required to heat 1 gram of pure liquid water from 10C to 20C? How would i approach this problem?
Monday, September 26, 2011 at 1:33am by D

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 (check formula please)
how much energy (in kJ) is required to change the temp of 1.00 kg of Fe from 25.0 degrees celsius to 1515 degrees celsius? the specific heat capacity of iron is 0.449 J/g*K. this is the answer i got. q=(.449)(1.00)(1490)= 669.01 kJ
Monday, April 5, 2010 at 11:32am by Danielle

physics
The engine of a large ship does 2.05 multiplied by 108 J of work with an efficiency of 4.00%. (a) How much waste heat (J) is produced? (b) How many barrels of fuel are consumed, if each barrel produces 6.00 multiplied by 109 J of heat when burned?
Wednesday, July 24, 2013 at 9:53pm by Eric

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

chemistry
How much energy would be needed to vaporize 150 grams of ethanol when it is at its boiling point? Hear of Vaporization (kj/kg)...841.00
Sunday, May 23, 2010 at 11:33am by Julia

physics
Calculate the number of Joules of heat required (Q), using the mass, specific heat of ice, temperature rise and latent heat of fusion. Q = M[10 C(ice) + Latent heat] = 1.00[10*2090 + 3.33*10^5] = 3.54*10^5 J Then divide that by the heating rate in Watts (J/s) for the answer in...
Tuesday, May 4, 2010 at 9:12pm by drwls

Physics 11th grade 'Heat' .
1) 100g*(80 cal/g + 23 C*1.0cal/gC) = 10,300 cal 2) Additional heat will be transferred to water in the bucket that does not vaporize. You need to know how much water that is. The question is poorly explained. They probably want you to answer 10g*(79C*1.0 cal/gC+540cal/g)
Friday, March 15, 2013 at 8:40am by drwls

college chemistry
Add the following: Heat to go from -40C to -33C Heat to vaporize at -33C Heat to go from -33 to-11C as a vapor.
Tuesday, May 25, 2010 at 3:21pm by bobpursley

chemistry
1. the volume of an idea gas is 2.06L at standard temperature and pressure. Calculate the volume at 1.75 atm and 27CELCIUS. 2. Ethane, C2h6 has a molar heat of vaporization of 15kj/mole. How many kilojoules or energy are required to vaporize 5 g of ethane?
Tuesday, December 1, 2009 at 7:13pm by stephanie

Chemistry
The specfic heat of iron is 0.11cal/g C. The heat of fusion of iron, the heat required to convert iron from a solid to liquid at its melting point, is 63.7cal/g. Iron melts at 1530 C. How much heat must be added to 2g of iron at 25c to completely melt it?
Friday, March 15, 2013 at 6:24pm by Dan

pyhsical science
How much heat is necessary to vaporize 100 g of water at 100 C to form steam at 100 C?
Tuesday, March 16, 2010 at 9:59pm by Anonymous

physical science
How much heat is necessary to vaporize 100 g of water at 100 C to form steam at 100 C?
Tuesday, March 16, 2010 at 10:00pm by Anonymous

physical science
How much heat is necessary to vaporize 100 g of water at 100 C to form steam at 100 C?
Tuesday, March 16, 2010 at 10:03pm by Anonymous

chemistry
I am to find how much heat is required to vaporize 3.50L of at its normal boiling point? such that the normal boiling point: 77 Degrees Celsius and the following data are provided, Normal melting point, -23 Degrees Celsius density of liquid, 1.59g/mL Delta H (FUSION): 3.28 kJ ...
Monday, December 8, 2008 at 3:14pm by Linda

chemistry
How much heat in joules is required to heat a 40g sample of aluminum from 77*C to 150*F?
Saturday, February 18, 2012 at 12:56pm by lorray

chemistry
How much heat in joules is required to heat a 44g sample of aluminum from 76 F to 148 F?
Tuesday, February 26, 2013 at 10:13pm by tish

chem
The heat of combustion of bituminous coal is 2.50 104 J/g. What quantity of the coal is required to produce the energy to convert 137.7 pounds of ice at 0.00C to steam at 100.C? specific heat (ice) = 2.10 J/gC specific heat (water) = 4.18 J/gC heat of fusion = 333 J/g ...
Wednesday, December 15, 2010 at 11:37am by Bogdanam

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