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April 16, 2014

Search: the latent heat of fusion and the melting point of lead are 2.45 × 104 J/kg and 327°C

Number of results: 64,954

College Physics
100 grams of molten lead (600oC) is used to make musket balls. If the lead shot is allowed to cool to room temperature (21oC), what is the change in entropy (in J/K) of the lead? (For the specific heat of molten and solid lead use 1.29 J/g oC; the latent heat of fusion and the...
Sunday, June 12, 2011 at 4:38am by Chris

physics
If 50,000joules of heat is added to 10kg of lead at its melting point of 330 degrees celsius.If 2kg of lead melts,calculate the latent heat of fusion of lead
Thursday, January 12, 2012 at 10:20am by chrystabelle1

Physics
How much energy is needed to melt 0.225 kg of lead so that it can be used to make a lead sinker for fishing? The sample has an initial temperature of 27.3 degrees celsius and is poured in the mold immediately after it has melted. Not sure if this is relevant to finding the ...
Tuesday, March 30, 2010 at 10:11pm by Kim

Physics
How much energy is needed to melt 0.225 kg of lead so that it can be used to make a lead sinker for fishing? The sample has an initial temperature of 27.3 degrees celsius and is poured in the mold immediately after it has melted. Not sure if this is relevant to finding the ...
Tuesday, March 30, 2010 at 10:15pm by Kim

Science
I'm going crazy! The heat necessary to change the state of water between a solid and a liquid is called the latent heat of vaporization, latent heat of solidification, latent heat of fusion, latent heat of liquefaction, or none of the above. I thought it was none of the above...
Friday, December 8, 2006 at 11:25am by Pat

Chemistry
Lead has a melting point of 327C, its specific heat is J/gdeg, and its molar enthalpy of fusion is 4.80 kJ/mol. How much heat, in kilojoules, will be required to heat a 500.0-g sample of lead from 23.0C to its melting point and then melt it?
Sunday, November 4, 2012 at 9:59pm by steph

Chemistry
Lead has a melting point of 327C, its specific heat is J/gdeg, and its molar enthalpy of fusion is 4.80 kJ/mol. How much heat, in kilojoules, will be required to heat a 500.0-g sample of lead from 23.0C to its melting point and then melt it?
Sunday, November 4, 2012 at 10:30pm by steph

physics
lead is a soft, dense metal with a specific heat of 0.028 kcal/kg degrees C, a melting point of 328.0 degrees C and a heat of fusion of 5.5 kcal/kg. How much heat must be provided to melt a 250.0 kg sample of lead with a temperature of 20.0 degrees Celsius? q1 = heat to move ...
Tuesday, November 21, 2006 at 1:26pm by Erica

SCIENCE QUESTION
LEAD IS A SOFT, DENSE METAL WITH A SPECIFIC HEAT OF 0.028KCAL/KGC, A MELTING POINT OF 328.0C, AND A HEAT FUSION OF5.5KCAL/KG. HOW MUCH HEAT MUST BE PROVIDED TO MELT A 250.0KG SAMPLE OF LEAD WITH A TEMPERATURE OF 20.0C? Figure the heat to heat if from 20C to the melting point (...
Saturday, October 7, 2006 at 10:14pm by priscilla

Chemistry
Just for your information, the heat of fusion and the heat of solidification are the same. Just like the heat of vaporization and heat of condensation are the same. The only difference is heat fusion is melting at the melting point and heat of solidification is the solidifying...
Wednesday, February 24, 2010 at 10:49pm by DrBob222

physics
KE=1/2 massbullet* velocity^2 heat required to melt=heat required to change temp to melting poing+heat to change lead to liquid = mass*specifHeatLead*(Tm-40)+mass*HeatfusionLead look up the specifice heat of lead, the temperature of melting lead, and finally the heat of fusion...
Friday, July 19, 2013 at 7:51pm by bobpursley

chemistry
q1 = heat required to move T from 25 to melting point of Pb. You will need to look up the melting point value. q1 = mass Pb x specific heat Pb x (Tfinal-Tinitial). q2 = heat to melt solid lead at the melting pont to liquid at the melting point. q2 = mass Pb x heat fusion. ...
Wednesday, December 8, 2010 at 9:43pm by DrBob222

physics
Besides the heat energy needed to raise the temperature of the lead to the 327.4 C melting poing, you need to provide the heat of fusion of lead, in order to melt it. The heat of fusion of lead is 27 kJ/kg. See if that raises the required velocity enough to give the "correct" ...
Sunday, April 15, 2012 at 3:24am by drwls

physics
Objects A and B have the same mass of 3.4 kg and are at their melting points. They melt when 4.9 104 J of heat is added to A and when 11 104 J is added to B. (a), (b) Determine the latent heat of fusion for the substance from which each object is made. (c) Find the heat ...
Wednesday, April 24, 2013 at 1:25pm by Anonymous

physics
What mass (in grams) of steam at 100C must be mixed with 341 g of ice at its melting point, in a thermally insulated container, to produce liquid water at 57.0C? The specific heat of water is 4186 J/kgK. The latent heat of fusion is 333 kJ/kg, and the latent heat of ...
Friday, April 15, 2011 at 8:28am by tim

physics
What mass (in grams) of steam at 100C must be mixed with 446 g of ice at its melting point, in a thermally insulated container, to produce liquid water at 65.0C? The specific heat of water is 4186 J/kgK. The latent heat of fusion is 333 kJ/kg, and the latent heat of ...
Monday, April 1, 2013 at 8:07am by safc

HELP URGENT Phyiics
What mass (in grams) of steam at 100C must be mixed with 446 g of ice at its melting point, in a thermally insulated container, to produce liquid water at 65.0C? The specific heat of water is 4186 J/kgK. The latent heat of fusion is 333 kJ/kg, and the latent heat of ...
Friday, April 12, 2013 at 5:44am by HELP

thermal physics
What mass (in grams) of steam at 100C must be mixed with 340 g of ice at its melting point, in a thermally insulated container, to produce liquid water at 12.0C? The specific heat of water is 4186 J/kgK. The latent heat of fusion is 333 kJ/kg, and the latent heat of ...
Monday, March 23, 2009 at 6:36pm by chirayu

thermal physics
What mass (in grams) of steam at 100C must be mixed with 340 g of ice at its melting point, in a thermally insulated container, to produce liquid water at 12.0C? The specific heat of water is 4186 J/kgK. The latent heat of fusion is 333 kJ/kg, and the latent heat of ...
Wednesday, March 25, 2009 at 7:15am by chirayu

physical mod
What mass (in grams) of steam at 100C must be mixed with 462 g of ice at its melting point, in a thermally insulated container, to produce liquid water at 40.0C? The specific heat of water is 4186 J/kgK. The latent heat of fusion is 333 kJ/kg, and the latent heat of ...
Friday, September 13, 2013 at 2:43am by adrian

physics
When a lead bullet hits a solid target at high speed, its entire kinetic energy is converted into heat. For simplicity, assume that all the heat is concentrated in the bullet rather than the target. If the bullet's initial temp. is 20` C, how fast should it be moving before ...
Friday, February 19, 2010 at 11:13pm by elisabeth

Physical Science
lead has specific heat of .028kcal/kgC, melting point of 328 degrees C and a heat fusion of 5.5 kcal/kg. how much heat must be provided to melt a 250kg sample of lead with a temperature of 20 degrees Celsius?
Friday, April 8, 2011 at 12:16am by yolanda

physics
Entropy of melting A block of a certain substance (m = 0.3 kg) sits in a cold room at its melting point 170 K. A lab demonstrator supplies heat at a rate of 200 W for 140 seconds by focusing light on the block to (just) completely melt the block. (a) What is the latent heat of...
Saturday, March 27, 2010 at 4:54am by michael

Chemistry
Dr. Bob, When I use the values that I have for latent heat of fusion and vaporization, I do not get the right answer. I have that latent heat of vaporization is 597.3 - 0.564T, and latent heat of fusion is 79.7 cal/gH2O.
Saturday, November 3, 2012 at 8:04pm by Paige

Physical Science
to get the heat released or absorbed, Q = mc(T2-T1) where m = mass of substance c = specific heat capacity T2 = final temperature T1 = initial temperature **note: if Q is (-), heat is released and if (+), heat is absorbed now we can only apply this to substances that did not ...
Friday, April 8, 2011 at 12:16am by Jai

Chemisty
LEAD IS A SOFT, DENSE METAL WITH A SPECIFIC HEAT OF 0.028KCAL/KGC, A MELTING POINT OF 328.0C, AND A HEAT FUSION OF5.5KCAL/KG. HOW MUCH HEAT MUST BE PROVIDED TO MELT A 250.0KG SAMPLE OF LEAD WITH A TEMPERATURE OF 20.0C?
Thursday, October 23, 2008 at 7:34pm by Jessica

physics
The latent heat of fusion for water is 33.5 104 J/kg, while the latent heat of vaporization is 22.6 105 J/kg. What mass m of water at 0 C must be frozen in order to release the amount of heat that 2.32 kg of steam at 100 C releases when it condenses?
Tuesday, July 30, 2013 at 10:22pm by damon

physics
How much heat must be added to 0.55 kg of aluminum to change it from a solid at 180C to a liquid at 660C (its melting point)? The latent heat of fusion for aluminum is 4.0x10^5 J/kg. I understand the Equation Q=mc times change it T would that be .55 times 4.0 x 10^5 times (...
Friday, December 10, 2010 at 6:24pm by maria

physical science
Lead is a soft, dense metal with a specific heat of 0.028 kcal/kgC, a melting point of 328.0C, and a heat of fusion of 5.5 kcal/kg. How much heat must be provided to melt a 202.2 kg sample of lead with a temperature of 20.0C?
Tuesday, October 12, 2010 at 10:56pm by Anonymous

physics
How much heat must be added to 0.55 kg of aluminum to change it from a solid at 180C to a liquid at 660C (its melting point)? The latent heat of fusion for aluminum is 4.0 105 J/kg.
Friday, December 10, 2010 at 4:00pm by maria

physics
How much heat in joules must be added to 0.348 kg of aluminum to change it from a solid at 138 C to a liquid at 660 C (its melting point)? The latent heat of fusion for aluminum is 4.0 x 105 J/kg.
Tuesday, May 15, 2012 at 4:29am by RM

Physics
It takes 1110 calories of energy to melt a 185 gram lump of lead. What is lead's latent heat of fusion?
Monday, March 5, 2012 at 9:21pm by Tracy

physics
bullet mass: M = 3.00g initial velocity: V0 = 640m/s initial temperature: T0 = 313.15K final velocity: V1 = 0m/s melting point of Lead: T2 = 600.61K specific heat of lead: C = 0.128J/g/K latent heat of melting: L = 22.4J/g (a)Find the available kinetic energy of the bullet.(J...
Friday, July 19, 2013 at 7:51pm by Graham

Physics
The latent heat of fusion of alcohol is 50 kcal/kg and its melting point is -54oC. It has a specific heat of 0.60 in its liquid state. Calculate the energy needed to melt 2.0 kg of solid alcohol at -54o and raise it to a temperature of -4C.
Tuesday, June 18, 2013 at 9:35am by Isis

Astronomy
The latent heat of melting is the amount of energy needed to convert a solid substance at its melting temper- ature to a liquid at the same temperature. For typical volcanic rocks, the latent heat of melting is around 5105 J/kg, which means it takes 5105 J to turn 1 kg of ...
Thursday, April 9, 2009 at 1:01am by Ashley

Will Someone please respond! Chem
q = mass ice x heat fusion = ? If you have others of a similar nature, they are At a phase change, mass x heat fusion at melting point OR mass x heat vaporization at boiling point.l WITHIN a phase, q = mass x specific heat in that hase x (Tfinal-Tinitial)
Friday, June 22, 2012 at 11:34am by DrBob222

Chem
From solid at the start to the melting point, heat required is q1 = mass x specific heat solid x (Tfinal-Tinitial) At the melting point, q for melting is q2 = mass solid x heat fusion From the melting point to the boiling point, q for heating the liquid phase is q3 = mass x ...
Friday, September 2, 2011 at 11:23am by DrBob222

Chemistry
heat lost by Ag turning to solid + heat lost by Ag in heating water + heat gained by water = 0 I don't think you can work this problem unless your are given the melting point of silver. You must know WHERE the initial T is. Perhaps you are to look it up. I did that on the web...
Wednesday, February 24, 2010 at 10:49pm by DrBob222

Chemistry
to get the heat released or absorbed, Q = mc(T2-T1) where m = mass of substance (units in g) c = specific heat capacity (units in J/g-K) T2 = final temperature T1 = initial temperature **note: if Q is (-), heat is released and if (+), heat is absorbed now we can only apply ...
Thursday, March 31, 2011 at 1:49am by Jai

chemistry
Use two formulas. Within a phase: q=mass x specific heat x (Tfinal-Tinitial) phase change: mass x heat vap at boiling point mass x heat fusion at melting point For example: at melting point of ice. To change solid ice at zero C to liquid at zero C. q = 59 g ice x heat fusion...
Thursday, March 1, 2012 at 6:33pm by DrBob222

Physics
What is latent heat of vaporisation and latent heat of fusion?
Sunday, June 5, 2011 at 4:40am by Shruthi

College Physics
For each incremental heat loss dQ, there is an entropy loss of the lead that is equal to dQ/T, where T must be in Kelvin. Compute the total entropy loss in three steps: (1) liquid lead cooling from 873 to 600 C (2) molten lead turning to solid at a contant temperature of 600 K...
Sunday, June 12, 2011 at 4:38am by drwls

Chemistry
when it is solid, liquid, or gas, the heat involved is m*c*deltaTemp At the transition pointss, melting, and again at boiling, there is a heat L*mass where L, the latent heat per mass, is either Lv (vaporiation heat/gram) or Lf(melting heat/gram) We will be happy to critique ...
Sunday, September 30, 2007 at 9:21am by bobpursley

Chem II
Here is how you do this. I suggest you make a table showing T in one column and the transition in the other; i.e. solid to liquid, melting point, liquid to gas, boiling point, etc. Then as long as you are in one phase, th3 formula is q = mass x specific heat x (Tfinal-Tinitial...
Wednesday, January 18, 2012 at 4:54pm by DrBob222

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

chemisty
calculate the heat energy released when 25.8 g of liquid mercury at 25 C is converted to solid mercury at its melting point. Constants for mercury at 1 atm: heat capacity of Hg-->28.0 melting point-->234.32 K enthalpy of fusion-->2.29 kj/mol
Thursday, June 27, 2013 at 5:53pm by Jill

Chemistry
The specific heat capacity of solid lead is 0.159J/gC, the molar enthalpy of fusion is 5.0kJ/mol, and the melting point of lead is 328C. Calculate the total energy required to change 100g of lead at 25C to molten lead at it's melting point. I will be happy to critique your ...
Saturday, September 23, 2006 at 3:02pm by J.M.

Chemistry
I'm not usre of your use of the terms heat of solid and heat of liquid. The heat required to move the temperature of a solid from Tinitial to Tfinal, is q = mass x specific heat solid x (Tfinal-Tinitial) and Tfinal can't be greater than the melting point. The heat required to ...
Thursday, June 10, 2010 at 5:28pm by DrBob222

Chemistry
to get the heat released or absorbed, Q = mc(T2-T1) where m = mass of substance (units in g) c = specific heat capacity (units in J/g-K) T2 = final temperature T1 = initial temperature **note: if Q is (-), heat is released and if (+), heat is absorbed now we can only apply ...
Saturday, May 14, 2011 at 8:53pm by Jai

Chemistry
I would think that melting point and crystallization point would be the same. q = heat needed = mass Cu x heat fusion
Wednesday, August 15, 2012 at 9:50pm by DrBob222

Physics: Capacitance of Capacitor
Capacitor A and capacitor B both have the same voltage across their plates. However, the energy of capacitor A can melt m kilograms of ice at 0 C, while the energy of capacitor B can boil away the same amount of water at 100 C. The capacitance of capacitor A is 8.4 μF. ...
Friday, May 10, 2013 at 2:37pm by Phil-- HELP NEEDED ASAP

chem
im working on a lab in chemistry called measuring energy changes :Calorimetry how to you determine the molar latent heat of fusion of ice using q=mcT ?? why was the ice driedbefore it was placed in water? why is hot warer ysed rather than room temp? in which dirextion would ...
Thursday, February 11, 2010 at 10:20am by jess

Physical Science
20 grams times the latent heat of fusion, which is 80 calories per gram for water.
Monday, July 12, 2010 at 8:35pm by drwls

Physics
This is a three part question. First part is to calculate the amount of energy necessary to turn -10 C ice into 0 C water. Next is calculating the energy to convert 0 C water into 100 C steam. Then calculating the amount of energy to raise the steam 10 C to 110 C. Use Q=mc&#...
Sunday, January 12, 2014 at 9:46pm by Eschew Obfuscate

Physics
You need to raise the temperature of the lead from 27.3 degrees C to 327.3 degrees C heat required = mass * specific heat of lead * (327.3-27.3) then melt the lead heat to melt = mass * heat of fusion of lead You know everything here but the specific heat of lead which you ...
Tuesday, March 30, 2010 at 10:15pm by Damon

physcial science
When 1 kg of ice at 0 degrees Celsius absorbs 80 kilocalories of heat, the ice undergoes a) a change of state b) a loss of energy c) a rise in temperature d) an increase in volulme The heat of fusion of water is 80 kcal/kg. That means that 1 kg of ice will melt if it absorbs ...
Friday, June 22, 2007 at 8:12pm by daniel

ap chemistry
An easy but long problem. You have two formulas to use for this. Within a phase (all gas, all liquid, all solid), q = mass x specific heat x (Tfinal-Tinitial) At a transition point: At the boiling point is is q = mass x heat vaporization At the melting point it is q = mass x ...
Tuesday, October 22, 2013 at 6:23pm by DrBob222

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
Compute the amount of heat necessary to be removed from the Al and liquid H2O to reduce both to 0 C. If that heat can be absorbed by the melting of less than 150g or less of ice, then the equilibrium temperature is 0 C. If not, you will have to do some algebra to get the ...
Friday, January 13, 2012 at 1:46am by drwls

Physics
5) An insulated Thermos contains 190 cm3 of hot coffee at 79.0C. You put in a 11.0 g ice cube at its melting point to cool the coffee. By how many degrees (in Celsius) has your coffee cooled once the ice has melted and equilibrium is reached? Treat the coffee as though it ...
Sunday, November 14, 2010 at 3:21am by john

physics
An insulated Thermos contains 140 cm3 of hot coffee at 89.0C. You put in a 11.0 g ice cube at its melting point to cool the coffee. By how many degrees (in Celsius) has your coffee cooled once the ice has melted and equilibrium is reached? Treat the coffee as though it were ...
Sunday, December 4, 2011 at 7:58am by mar13

physics
An insulated Thermos contains 140 cm3 of hot coffee at 89.0C. You put in a 11.0 g ice cube at its melting point to cool the coffee. By how many degrees (in Celsius) has your coffee cooled once the ice has melted and equilibrium is reached? Treat the coffee as though it were ...
Sunday, December 4, 2011 at 8:00am by mar13

Chemistry
You must calculate the heat evolved in stages, then add all of the heats together to obtain the sum. Here is the way you go about it. q1 = heat lost in moving the vapor from the starting point to the boiling point. q1 = mass vapor x specific heat vapor x (Tfinal-Tinitial) ...
Saturday, June 12, 2010 at 2:20pm by DrBob222

Nsuk
(1)calculate the heat energy datas temperatures 100degree celciuse and 4degree celciuse,mass 0.5kg take latent heat of vapourisation 2.02times10raised to the power of minus6.(2)calculate the specific latent heat of fusion mass of calorimeter 0.01kg and mass of ice 0.09kg and 0...
Friday, February 22, 2013 at 6:34am by Saen

science
When you freeze water, 80 calories of heat are released into the surroundings for every gram of water that freezes. This is known as the "latent heat of fusion" of water, which is 80 cal/g. Heat of fusion is a characteristic property. Theoretically, if you could "capture" all ...
Monday, January 31, 2011 at 12:14am by Elizabeth

science
im doing exactly the same thing. Chechimal change : Chemical Change: Light and Heat is produced. It will make the atoms move around with the energy. The Hydrocarbon vapours burn to give a Combustion reaction with Oxygen of the air which converts the vapour into CO2, CO, C (...
Saturday, October 21, 2006 at 10:00am by Me bruv

Chemistry
DrBob222, HELP! Calculate the heat energy released when 29.7 g of liquid mercury at 25.00 C is converted to solid mercury at its melting point. Constants for mercury at 1 atm: Heat capacity of Hg (l) 28.0 J/Mol*K, Melting pt 234.32 k, and enthalpy of fusion 2.29 kg/mol
Tuesday, September 11, 2012 at 12:31am by Jordan

CHEM HELP ASAP!
Calculate the heat energy released when 29.7 g of liquid mercury at 25.00 C is converted to solid mercury at its melting point. Constants for mercury at 1 atm: Heat capacity of Hg (l) 28.0 J/Mol*K, Melting pt 234.32 k, and enthalpy of fusion 2.29 kg/mol
Tuesday, September 11, 2012 at 8:18am by Jordan

Physics
How much heat is required to melt 50 g of mercury at -45 degrees celsius to 425 degrees celsius. (melting point=-38.degree-c, specific heat=0.03325 cal/g-degree c for solid mercury, .2988 cal/g-c degree c for liquid mercury and .2486 cal/g-c degree for gaseous mercury, heat of...
Monday, February 27, 2012 at 6:32pm by Abby

Physics
How much heat is required to melt 50 g of mercury at -45 degrees celsius to 425 degrees celsius. (melting point=-38.degree-c, specific heat=0.03325 cal/g-degree c for solid mercury, .2988 cal/g-c degree c for liquid mercury and .2486 cal/g-c degree for gaseous mercury, heat ...
Monday, February 27, 2012 at 8:06pm by Abby

Physics
How much heat is required to melt 50 g of mercury at -45 degrees celsius to 425 degrees celsius. (melting point=-38.degree-c, specific heat=0.03325 cal/g-degree c for solid mercury, .2988 cal/g-c degree c for liquid mercury and .2486 cal/g-c degree for gaseous mercury, heat ...
Monday, February 27, 2012 at 8:13pm by Abby

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

Physics B
The overall equation is Q=mL (m is mass; L is the latent heat of fusion for water) *we are trying to find mass (m) *rearranging the equation m=Q/L To find Q: the heat that caused the ice to melt was produced by the friction...we can find the amount of energy (in Joules) by ...
Thursday, January 15, 2009 at 4:38pm by Ashley

math
Problem The latent heat of fusion (solid become liquid) for ice is 79.8 cal/gram. How much ice can we melt with 1000 calories of heat? Problem Which would require more heat, melting 500 g of 0 C ice or turning 500 g of 100 C water into steam? Problem A 500 g sample of an ...
Monday, October 6, 2008 at 6:39pm by sherri

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

Chemistry
Search: How much energy (in Kj) is relased when 25.0g of ethanol vapor at 93, is cooled to -10? Ethanol has a melting point of -114.5, bp of 78.4, specific heat= 2.10J/g, heat of fusion =4.60Kj/mol, specicic heat= 1.9j/g, heat of vaporization = 38.56Kj/mol
Tuesday, September 27, 2011 at 9:49pm by Oscar

chemistry
You need the latent heat of fusion. You may have been given it with the question. http://en.wikipedia.org/wiki/Diethyl_ether_(data_page) has 7.19 kJ mol-1 so calculate the number of moles of diethyl ether relative molecular mass = 74.14 then multiply the number of moles by the...
Tuesday, May 4, 2010 at 11:06am by Dr Russ

Chemistry
38.0kg mass of copper is melted to be cast into a graphite mold at a copper pipe foundtry. If the solid copper starts off at the normal melting temperature of copper and the liquid copper is put into the mold at the crystallization point of copper, how much heat is added to ...
Wednesday, August 15, 2012 at 9:50pm by Jacob

chem
The specific heat of silver is 0.237 J/goC Its melting point is 961oC . Its heat of fusion is 11 J/g. How much heat (in J) is needed to change 17.5 g of silver from solid at 25oC to liquid at 961oC ? Add the heat required to warm the silver from room temp to the mp. Then add ...
Tuesday, October 31, 2006 at 7:59pm by mary

chemistry
When no phase change is involved, use this equation. q = mass x specific heat x (Tfinal-Tinitial). When a phase change is involved (at the melting point or boiling point) use this one. q = mass x heat fusion or heat vap Total q = sum of individual qs.
Thursday, November 10, 2011 at 8:04pm by DrBob222

chem
The normal melting point of copper is 1357 K and heat of fusion of Cu is 13.05 KJ. How much heat, in kilojoules, is evolved when a 3.70 kg sample of of molten Cu freezes?
Thursday, February 11, 2010 at 1:17am by Joseph

Chemistry
Lithium metal is a highly reactive metal that oxidizes instantly in water or air. Given the data below, calculate the energy required to heat 10.0 g of Li from 150.0 C to 200.0 C. Molar heat capacity (solid) = 3.58 J/C mol Molar heat capacity (liquid) = 4.379 J/C mol ...
Thursday, April 25, 2013 at 11:53pm by Johnny

Physics B
Since the surface is horizontal, all of the loss of kinetic energy is due to frictional heating. The loss of kinetic energy is (1/2)M(Vfinal^2 - Vinitial^2) = 538 Joules = 129 calories If all that heat went into melting the ice, the amount that melted is 129 calories divided ...
Thursday, January 15, 2009 at 4:38pm by drwls

chemistry
Tungsten has been used to make light bulb filaments since 1908. The melting point of tungsten is 3422 C and the heat of fusion is 35 kJ/mole. Calculate the entropy change associated with the melting of one mole of tungsten.
Wednesday, October 24, 2007 at 10:14pm by dan

Chemistry
Here is how you do it. For temperature changes in the same phase( all solid, all liquid, all gas), q = mass x specific heat in that phase x (Tfinal-Tinitial). For changing phases (from solid to liquid of liquid to gas), q = mass x heat fusion (at melting point) q = mass x heat...
Monday, December 5, 2011 at 1:29pm by DrBob222

Physics
lead melts at 328 degrees C. lead has a heat of fusion of 2.04X10^4 J/kg and a specific heat of 130 J/kgK. how much heat must be removed from 0.50 kg of molten lead (liquid) at 328 degrees C to make it all a solid chunk at 300 degrees C?
Thursday, November 18, 2010 at 8:35pm by Brittany

Chemistry
q1 = heat to raise T from 23.0C to 327 C. q1 = mass Pb x specific heat Pb x (Tfinal-Tinitial) q2 = heat to melt Pb q2 = mass Pb x heat fusion. Total = q1 + q2 I note you have mass in grams in specific heat (not listed) in J/g*C so that's ok. However, when you go to the melting...
Sunday, November 4, 2012 at 10:30pm by DrBob222

Chemistry
There are only two equations to remember in this heat transfer business with specific heat. 1. q= heat absorbed/releassed by phase change (melting/condensing) = mass x heat fusion for melting/freezing or heat vaporization for vaporization/condensing. 2. heat change by moving T...
Saturday, July 9, 2011 at 3:05pm by DrBob222

Science
the latent heat of fusion
Friday, December 8, 2006 at 11:25am by Anonymous

physics
A 1.3 Kg block of ice is initially at a temp of -5 degrees celsius. If 7.5 *10^5 J of heat are added to the ice, what is the final temperature of the system? I multiplied 1.3 Kg of ice by the specific heat of ice (2090), then I divided by the amount of heat added. I came up ...
Friday, June 22, 2007 at 2:30pm by tasha

physics
An unknown material has a normal melting/freezing point of -20.4 C, and the liquid phase has a specific heat capacity of 179 J/(kg C). One-tenth of a kilogram of the solid at -20.4 C is put into a 0.130-kg aluminum calorimeter cup that contains 0.198 kg of glycerin. The ...
Wednesday, December 4, 2013 at 10:32pm by tiana

Entropy
Tungsten has been used to make light bulb filaments since 1908. The melting point of tungsten is 3422C and the heat of fusion is 35 kJ/mole. Calculate the entropy change associated with the melting of one mole of tungsten.
Wednesday, October 24, 2007 at 11:29pm by Matt

Chemistry
I don't think the question is worded right. if you want just the heat removed by melting Ga all you need is q = 5grams x heat fusion = ?. If you want, and I don't know why the specific heat is given if you don't want it, is the heat removed before melting at 29.76 when ...
Thursday, February 7, 2013 at 11:20pm by DrBob222

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

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
Ethanol (C2H5OH) has been produced since antiquity by the fermentation of fruits and vegetables. Given the following data, if 5.87 kJ of energy are transferred to 13.3 g of frozen ethanol at -130.0 C, what is the final temperature of the sample? Heat capacity (solid) = 0.97 J...
Thursday, April 25, 2013 at 11:52pm by Johnny

Physics
you need to first look for the latent heat of fusion (Lf) --- this is a constant, then use the formula: Q = m(Lf) where Q = heat in Joules, m = mass in grams *since it melted, it definitely absorbed/gained heat, thus Q is (+) so there,, :)
Thursday, October 28, 2010 at 8:54am by jai

Physics
You have left your bicycle outside in the backyard for three hours on a very cold day. Now you decide to go for a ride. The metal handlebars feel colder than the plastic hand-grips because: Question 4 options: A) The latent heat of fusion of the plastic is bigger than the ...
Monday, August 15, 2011 at 7:07pm by Skylar

chemistry
Say you have two substances, A and B. A has a melting point of 300 degrees Celcius, while B has a melting point of 200 degrees Celcius. If you took a mixed melting point where the ratio of A is higher than B, what would the melting range look like? Would the melting point be ...
Saturday, January 25, 2014 at 8:45pm by Louis

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