Number of results: 36,448
Chemistry
What quantity of heat is necessary to convert 50.0 g of ice at 0.0 C into steam 100,0 C? The heat of fusion is 80.0 cal/g, the heat of vaporization is 540 cal/g, and the specific heat of water is 1.00 cal/gC.
Tuesday, March 27, 2012 at 6:08pm by Jill
chemistry
q = mass x specific heat x delta T. 6.1 = 1.50g x specific heat x 9 Solve for specific heat.
Monday, January 16, 2012 at 9:44pm by DrBob222
Chemistry
q at a phase change = mass x heat vaporization for liquid to gas or mass x heat fusion for solid to liquid. For example, to change water from liquid at 100 C to steam at 100 C is mass H2O x heat vaporization. q within a single phase is mass x specific heat in that phase x (...
Friday, April 20, 2012 at 8:11pm by DrBob222
Chemistery
200g of water (specific heat of 4.184 Jg-1'c-1) loses 2000 J of heat. Its starting temperature is 70'C. Calculate the temperature of the water.
Saturday, October 30, 2010 at 5:13pm by May
chemistry
q = mass water x specific heat water x delta T. I would convert heat to Joules and mass sample to grams to start.
Friday, February 5, 2010 at 4:22pm by DrBob222
chemistry
1. ice melts at zero C. q = mass ice x heat fusion 2. melted water at zero changes temperature to Tfinal. q = [mass melted ice x specific heat H2O x (Tfinal-Tinitial)] 3. Warm water at 100 C cools to Tfinal q = [mass warm water x specific heat H2O x (Tfinal-Tinitial)] Add 1 + ...
Thursday, October 4, 2012 at 8:32pm by DrBob222
Chemistry
How much heat is needed to heat the coffee? q = mass water x specific heat water x (Tfinal-Tintial) How much energy in 1 photon? E = hc/wavelength. Now set up a proportion. (1 photon/E) = (#photons/q) solve for # photons.
Wednesday, October 27, 2010 at 12:06am by DrBob222
Chemistry
What is a method for determining the specific heat for a metal like sodium which reacts with water? You could heat it and let it come to an equilibrium temperature inside a calorimeter. or you could put it in a liquid such as kerosene and observe the heat, temperature changes...
Wednesday, February 28, 2007 at 1:05am by Brown
College chemistry
q1 = heat to warm water from 10 to 100. q1 = mass x specific heat x (Tfinal-Tinitial) where Tf is 100 and Ti is 10 (or delta T = 90). q2 = heat to vaporize liquid water at 100 to vapor at 100 C. q2 = mass water x heat vaporization Total q = q1 + q2.
Friday, September 3, 2010 at 2:55pm by DrBob222
Chemistry (Thermo)
b. q = mass x heat fusion q about 32,723,000 J heat fusion about 334 J/g Solve for mass ice. You should confirm the 334 value. c. q = [mass ice x heat fusion ice] + [mass water x specific heat water x delta T] Let mass ice = mass water = x and solve for x. d. Same procedure ...
Friday, September 10, 2010 at 10:25am by DrBob222
chemistry
q = mass x specific heat x (Trinal-Tinitial) q = 550 x specific heat Al x (145-22) Look up the specific heat Al in your text or notes and punch the calculator.
Monday, April 11, 2011 at 7:16pm by DrBob222
physics
.250 kg * specific heat of water * 25 = heat of fusion of water * mass of ice in kg
Thursday, January 12, 2012 at 10:09am by Damon
chemistry
the specific heat of water is 4.184 j/g-c(celcius). how much heat is required to raise the temperature of 5.0 g of water by 3.0 c(celcius)?
Sunday, April 4, 2010 at 7:17pm by demond
Chemistry
If 1.22 grams of magnesium reacts with 100 ml of 6.02 M HCl solution. How much heat is evolved? Density of the HCl solution is 1.10 g/ml. Assume the specific heat of water 4.184 J/gC is the specific heat of the solution. Mg + 2 HCl à MgCl2&...
Tuesday, July 17, 2012 at 12:33am by Anonymous
Science (Chemistry)
Islands in the middle of the oceans (for example, Great Britain, Hawaii, Bermuda) tend to have more stable climates with smaller temperature fluctuations than regions of the same mass surrounded by land (for example, continents). Explain these facts by referring to heat energy...
Tuesday, April 10, 2012 at 4:22pm by Ricardo
Physics Help Please!
The change in temperature is 12 deg C if it rises from 15 to 27 degrees. 1. Find the mass of water from volume of water times its density. 2. Find the heat in Joule needed from Q=mct where m is mass of water, c is specific heat capacity and t is rise in temperature. Then the ...
Tuesday, April 6, 2010 at 2:51pm by Chris
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...
Friday, April 27, 2012 at 8:06pm by Anonymous
CHEM
A 5.00 g sample of Al pellets (specific heat = .89 J/g degrees c) and a 10.00 g sample of Fe pellets (specific heat = .45 J/g degrees c) are heated to 100.0 degrees C. The mixture of hot Fe and Al is then dropped into 97.3 g of water at 22.0 degrees C. Calculate the final temp...
Monday, October 1, 2007 at 6:16pm by Charlie
chemistry
This is best done in stages. There are just two formulas involved. Remember them. q1 = heat released on the phase change from vapor (steam) at 100 C to liquid water at 100 C. q1 = mass steam x heat vaporization. (formula 1) q2 = heat released on cooling liquid water at 100 C ...
Tuesday, April 12, 2011 at 5:28pm by DrBob222
Science
q1 = heat removed to condense steam at 100 to liquid at 100 C. q1 = mass x heat vaporization q2 = heat removed to cool from liquid water at 100 C to body temperature of 37 C. q2 = mass water x specific heat water x (Tfinal-Tinitial). Tf = 37, Ti = 100. Total heat absorbed by ...
Wednesday, July 13, 2011 at 5:40pm by DrBob222
chemistry
heat lost by Zn + heat gained by water = 0 [mass Zn x specific heat Zn x (Tfinal-Tinitial)] + [mass H2O x specific heat H2O x (Tfinal-Tinitial)] = 0 Substitute and solve for the one unknown.
Thursday, April 25, 2013 at 1:33pm by DrBob222
Chemistry
Since the T of the acid and base are not the same I would do it in two steps. qHCl = mass water x specific heat x (Tfinal-Tinitial). qNaOH = mass water x specific heat x (Tfinal-Tinitial). Then add qHCl + qNaOH = total q.
Tuesday, May 4, 2010 at 8:19pm by DrBob222
Physics
(mass flow rate)*C*(delta T) = 1.5*10^8 W C is the specific heat of the cooling water. "delta T" is the change in temperature of the water (3.0 C) Solve for the mass flow rate. It will be in kg/s if you use the specific heat, temperature and power units above.
Friday, January 1, 2010 at 2:30am by drwls
Chemistry
If 22 g of water is heated so that the water temperature rises from 18.1°C to 21.5°C, how many calories have been absorbed by the water? The specific heat of water = 1.00 cal / (g · °C)
Monday, October 25, 2010 at 12:55am by Cassie
chem
How much energy (in Joules) is required to heat 13.48 g of water from 10.5 oC to 46.2 oC ? Use 4.184 J/goC as the specific heat capacity of water.
Monday, March 26, 2012 at 4:06pm by emily
chemistry
If a 5.26-g sample of copper at 258 °C is placed in 125 mL of water at 21.0 °C, how hot will the water get? Assume no heat loss to the surroundings. The specific heat of copper is 0.385 J/g °C.
Thursday, October 23, 2008 at 5:11pm by Lilit***
chemistry
How many calories must be supplied to 59 g of ice at −6 C to melt it and raise the temperature of the water to 61 C? The specific heat of ice is 0.49 kcal/kg · K and of water is 1 kcal/kg · K; the heat of fusion of water is 79.7 kcal/kg, and its heat of...
Thursday, March 1, 2012 at 6:33pm by anonymous
chemistry
[mass Pb x specific heat lead x (Tfinal-Tinitial)] + [mass water x specific heat water x (Tfinal-Tinitial)] = 0.
Tuesday, August 3, 2010 at 5:21pm by DrBob222
Chemistry
I didn't include the water and should have done so. (mass water x specific heat water x (Tfinal-Tinitial)) + (mass alloy x specific heat alloy x (Tfinal-Tinitial)) + Ccal(Tfinal-Tinitial) = 0
Friday, October 22, 2010 at 7:13pm by DrBob222
chemistry
How many grams of water can be cooled from 35^\circ {\rm C} to 16^\circ {\rm C} by the evaporation of 57{\rm g} of water? (The heat of vaporization of water in this temperature range is 2.4 {\rm kJ}/{\rm g}. The specific heat of water is 4.18 {\rm J}/{\rm g}\cdot {\rm K}.)
Thursday, April 4, 2013 at 12:24pm by Anonymous
Chemistry
The temperature of 100.0 mL of water was raised from 26.7 degrees C to 62.3 degrees C. How much heat in calories was added to the water? (The specific heat of water is 1.000 cal/g degrees C and the density of water at 26.7 degrees C is 0.996626 g/mL)
Thursday, April 1, 2010 at 12:44am by Ally
Chemistry
qH2O + qmetal = 0 qH2O = mass H2O x specific heat water x (Tfinal-Tinitial). qmetal = mass metal x specific heat metal x(Tfinal-Tinitial). Just plug in the numbers and solve for specific heat metal.
Tuesday, July 15, 2008 at 11:13pm by DrBob 222
Physics
At thermal equilibrium, when everythng is 14 C, the temperature change of the copper is -86 C, and +4C for the water. The heat energy lost by the copper equals the energy gained by the water. Writing that equation with the water specific heat and masses will let you solve for ...
Thursday, May 7, 2009 at 3:26pm by drwls
Chemistry
q1 = heat needed to raise T of ice at -34C to zero C. q1 = mass ice x specific heat ice x (Tfinal-Tintial) q2 = heat needed to melt ice at zero C to liquid water at zero C. q2 = mass ice x heat fusion q3 = heat needed to raise T of liquid water at zero C to liquid water at 100...
Thursday, January 10, 2013 at 3:29am by DrBob222
chemistry
1) [mass metal x specific heat metal x Tfinal-Tinitial)] + [mass H2O x speicif heat water x (Tfinal-Tinitial) = 0 Only one unknown, specific heat metal. Solve for that. 2)Use the Law of Dulong and Petit
Thursday, November 13, 2008 at 12:37pm by DrBob222
Chemistry
q1 = heat released in steam moving from 130 C to 100 C. q1 = mass steam x specific heat steam x (Tfinal-Tinitial). q2 = heat released in condensing steam at 100 C to liquid water at 100 C. q2 = mass steam x heat vaporization. q3 = heat released in moving liquid water from 100 ...
Monday, January 24, 2011 at 10:24pm by DrBob222
Chemistry
A. q = mass water x specific heat water x delta T = heat evolved by the neutralization of HCl with NaOH. B. The above is q for how many moles? moles = L x M = 0.035L x 1.43 M = xx Then q/xxmoles = joules/mole
Friday, March 19, 2010 at 9:32pm by DrBob222
chem-calorimetry
If a 5.26-g sample of copper at 258C is placed in 125mL of water at 21.0C, how hot will the water get? Assume no heat loss to the surroundings. The specific heat of copper is .385 J/g C
Monday, March 31, 2008 at 9:11pm by natash
Chemistry
mass metal x specific heat metal x (Tfinal-Tinitial) + mass water x specific heat water x (Tfinal-Tinitial) = 0 The above will solve any of these problems. Just plug in the numbers and solve for the one unknown.
Wednesday, September 23, 2009 at 8:18pm by DrBob222
Physics 11
The heat lost by the hot water equals the heat gained by the tap water. The hot water cools 59 C and the tap water warms up by 14 C. 79*59*C =M*14*C The specific heat C cancels out. M = (59/14)*79 grams = 333 g = 0.333 kg I agree with your answer.
Monday, November 16, 2009 at 7:40pm by drwls
ap chemistry
q1 = heat to melt ice at zero C to water at zero C. q1 = mass ice x heat fusion. q2 = heat to move from zero C to 25 C. q2 = mass water x specific heat water x delta T. q total = q1 + q2 I don't see the right answer listed. Perhaps you made a typo in answer c.
Friday, September 24, 2010 at 8:22pm by DrBob222
Chemistry
A 5.00 gram sample of aluminum pellets (specific heat capacity = 0.89 J/g*C) and a 10.00 gram sample of iron pellets (specific heat capacity = 0.45 J/g*C) are heated to 100.0 *C. The mixture of hot iron and aluminum is then dropped into 97.3 gram of water at 22.0*C. Calculate ...
Tuesday, October 12, 2010 at 9:15pm by Anonymous
chem 101
heat lost by Fe + heat gained by water = 0 [mass Fe x specific heat Fe x (Tfinal-Tinitial)] + [mass H2O x specific heat H2O x (Tfinal-Tinitial)] = 0 Solve for Tf.
Wednesday, April 11, 2012 at 3:39pm by DrBob222
chemistry
3. Based on your answer in question 2, determine the percent error of your calculated specific heat capacity value of your unknown metal using the specific heat capacities of known metals below. Metal Specific Heat Capacity Nickel 0.440 Tin 0.210 Silver 0.237 Magnesium 0.140 ...
Thursday, April 4, 2013 at 2:35pm by lex
Chemistry
[mass ice x heat fusion ice] + [mass ice water x specific heat water x (Tfinal-Tinitial)] + [mass 1.5 L water x specific heat x (Tfinal-Tinitial) = 0 Solve for Tfinal.
Tuesday, July 27, 2010 at 4:58pm by DrBob222
Chemistry
This is how I solved it. M (water) = 250g T (initial water) = 25 + 273 = 298K M (metal) = 41.6g T (initial metal) = 100 + 273 = 373K T (final water & metal) = 26.4 + 273 = 299.4 C (water) = 4.184 (specific heat of water) C (metal) = x [4.184 * 250g (299.4 - 298)] + [x * 41...
Sunday, January 22, 2012 at 7:18pm by Rick
Chemistry
There are two formulas you use. If you are within the same phase, use q = mass x specific heat in that phase x (Tfinal-Tinitial). Example. q for 25g H2O from 5 C to 95 C is q = mass x specific heat x (95-5) = ? The other is at a phase change; i.e., ice melting or water boiling...
Sunday, April 22, 2012 at 3:03pm by DrBob222
chemistry
Calculate the energy in the form of heat, in kJ, required to convert 225 grams of liquid water at 21.0 °C to steam at 115 °C. Heat of fusion = 0.333 kJ/g; heat of vaporization = 2.26 kJ/g; specific heat capacities: liquid water = 4.18 J/g·°C., steam = 1.92 J...
Sunday, October 2, 2011 at 2:55am by Ninaya
Physics
A 0.260-kg piece of aluminum that has a temperature of -165 °C is added to 1.4 kg of water that has a temperature of 3.0 °C. At equilibrium the temperature is 0 °C. Ignoring the container and assuming that the heat exchanged with the surroundings is negligible, ...
Friday, November 17, 2006 at 7:54pm by Sara
Physics
heattoheatwater=masswater*specific*(45-20) figure mass water from volume and denstity, look up specific heat. if eff is .98, then energy=heat/.98 power=heateneryg/timeinseconds R=V^2/energy
Sunday, December 5, 2010 at 6:33pm by bobpursley
chemistry
Heat lost by nickel + heat gained by water = 0 [mass Ni x specific heat Ni x (Tfinal-Tinitial)] + [mass H2O x specific heat H2O x (Tfinal-Tinitial)] = 0
Tuesday, November 30, 2010 at 2:01pm 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
Chemistry
q1 = heat needed to melt ice at zero C to liquid water at zero C. q1 = mass ice x heat fusion q2 = heat needed to raise T from zero C to 100 C. q2 = mass melted ice x specific heat water x (Tfinal-Tinitial) q3 = heat needed to vaporize water at 100 to steam at 100. q3 = mass ...
Tuesday, March 27, 2012 at 6:08pm by DrBob222
Lauren
The specific heat of water is at 4.184J/g * degree C. How much heat is evolved, or absorbed, when the temperature of 9.00 mol of liquid water cools from 38 degrees C to 28 degrees C? How do I start this problem
Friday, November 16, 2007 at 6:37pm by Chemistry
Chemistry
An insulated beaker contains 250g of water at 25 degrees celsius. Exactly 41.6g of a metal at 100 degrees celsius was dropped in the beaker. The final temperature of the water was 26.4 degrees celsius. Assuming that no heat is lost in any other way, calculate the specific heat...
Sunday, January 22, 2012 at 7:18pm by Hannah
chemistry
heat needed was q = mass water x specific heat water x (100-0) = ?? delta T = 100 C.
Monday, May 2, 2011 at 2:46pm by DrBob222
Chemistry
1. heat lost piece of lead + heat gained by wter = 0 heat lost by lead = mass x specific heat lead x (Tf-Ti) where Tf is final T (in this case the unknown) and Ti is the initial T of the lead. heat gained by wter = mass x specific heat water x (Tf - Ti). Solve for Tf. Post ...
Monday, January 7, 2008 at 10:29pm by DrBob222
ap chemisty
Thank you. there is also a second part. B.) assuming that all the heat evolved in burning 30 g of butane is transferred to 8 kg of water at 22.2 degrees celsius (specific heat=4.184 J/gxK), calculate the final temperature of the water.
Friday, September 24, 2010 at 5:30pm by Sarah
Chemistry
[masss Al x specific heat Al x (Tfinal-Tinitial)] + [mass water x specific heat water x (Tfinal-Tinitial)] = 0 Solve for Tfinal.
Friday, September 10, 2010 at 1:44am by DrBob222
chemistry
q1 = heat evolved in moving steam from 145 to 100. q1 = mass steam x specific heat steam x (Tfinal-Tinital) where Tfinal is 100 and Tinitial is 145. q2 = heat evolved when steam at 100 C condenses to liquid at 100 C. q2 = mass x heat vaporization q3 = heat evolved in moving ...
Wednesday, June 23, 2010 at 12:40pm by DrBob222
Chemistry
75 g ice is melted to produce 75 g water at zero C and that is mixed with 1.5 L water at 75 C. (75g x heat fusion ice) + [mass water from ice x specific heat water x (Tfinal-Tinitial)] = 0 Solve for Tfinal.
Monday, November 22, 2010 at 5:22pm by DrBob222
science
The answer still is the same. Calcualte the heat stored in the 1 kg water and 1 kg gold and you will know which can produce the most heat to the bed. q = mass x specific heat x T
Saturday, September 8, 2007 at 6:27pm by DrBob222
chemistry
q1 = heat to move H2O from 55 to 100 C. q1 = mass x specific heat liqud water x (Tfinal-Tinial). Tfinal = 100; Tinitial = 55. q2 = heat to vaporize liquid water to steam @ 100 C. q2 = mass water x heat vaporization. total q = q1 + q2.
Thursday, April 22, 2010 at 1:16am by DrBob222
physics
A combination of .403 kg of water at 45.1 C, .471 kg of aluminum at 41.1 C, and .307 kg of copper at 50.4 C is mixed in an insulated container and allowed to come to thermal equilibrium. Determine the final temperature of the mixture. Neglect any energy transfer to or from the...
Sunday, February 13, 2011 at 11:06pm by brandon
chemistry
mass cold water x specific heat x (Tfinal-Tinitial) + mass hot water x specific heat x (Tfinal-Tinitial) = 0 Solve for mass hot water.
Wednesday, November 10, 2010 at 11:49pm by DrBob222
Physics
Assume all of the ice melts. (If it doesn't you will find out later when you compute the final temperature). Look up the specific heat of aluminum. It is 0.22 cal/C gm Assume the heat lost by the water and aluminum when being lowered to final temperature T equals the heat ...
Saturday, August 20, 2011 at 1:36pm by drwls
Chemistry
Need help with my lab report for specific heat of unknown metal! I need to Find the Specific Heat of Al! I know its Q= M x Cs x Change in Temp I am getting a such a high number am just confused if its right. Here is what I got in Lab: Aluminum Mass of Metal (Mm): 6.128g Mass ...
Friday, June 24, 2011 at 12:14am by Tc
physics
You must do the (a) part in stages. q1 = heat required to move the ice from a T of -5 to zero. mass x specific heat ice x (Tfinal-Tinitial). You have mass, look up specific heat ice and delta T = 5. q2 = heat to melt the ice. q2 = mass x heat fusion. You have mass. Look up ...
Saturday, November 22, 2008 at 10:06pm by DrBob222
Honors chemistry
You need to boil 307 g of water (specific heat = 4.184) so you can make a cup of your favorite drink. If room temperature is 20.15 oC, how much heat is needed to boil the water?
Sunday, September 23, 2012 at 8:52pm by Claire
Chemistry
Since these are the same masses, you can simply take the average of 90 and 10. (90+10)/2 = 50. If they are not the same mass it is a little more complicated than that but all of these can be solved the same way. heat gained by cool water + heat lost by warm water = 0 [mass ...
Sunday, November 13, 2011 at 8:47pm by DrBob222
CHEM
A 5.00 g sample of Al pellets (specific heat = .89 J/g degrees c) and a 10.00 g sample of Fe pellets (specific heat = .45 J/g degrees c) are heated to 100.0 degrees C. The mixture of hot Fe and Al is then dropped into 97.3 g of water at 22.0 degrees C. Calculate the final temp...
Monday, October 1, 2007 at 8:09am by Charlie
Chemistry Help!
calculate the specific heat of a metallic element if 314 joules of energy are needed to raise the teperature of a 50.0g sample from 25C to 50C. i'm not sure if you use the Q=(s)(m)(delta t) equation or not since it asks for the specific heat not the specific heat capacity...
Sunday, June 6, 2010 at 7:45pm by Ashley
physics
What amount of heat is required to increase the temperature of 75.0 g of water from 22.3C to 36.1C? The specific heat of water is 4186 J/KgC.
Monday, March 5, 2012 at 10:36pm by Anonymous
Chemistry
To heat water: mass H2O x specific heat H2O x (Tfinal-Tinital) T melt ice: q = mass ice x heat fusion water
Thursday, April 12, 2012 at 3:43pm by DrBob222
Chemistry
q = mass water x specific heat water x delta T water. Note the correct spelling of celsius.
Saturday, December 4, 2010 at 10:10pm by DrBob222
Science-Chemistry
A 5.00 g sample of Al pellets (specific heat = .89 J/g degrees c) and a 10.00 g sample of Fe pellets (specific heat = .45 J/g degrees c) are heated to 100.0 degrees C. The mixture of hot Fe and Al is then dropped into 97.3 g of water at 22.0 degrees C. Calculate the final temp...
Monday, October 1, 2007 at 12:40am by Niclas
Physics
How much energy would your body need to provide for the following : a)sweating and evaporation of 1kg of water from your skin. b)heat loss by radiation at the rate of 100 wats for 12 hours. (the specific latent heat of vaporisation of water is 2.3MJkg-1)
Thursday, June 2, 2011 at 5:31pm by Nelly
Physics
How much energy would your body need to provide for the following : a)sweating and evaporation of 1kg of water from your skin. b)heat loss by radiation at the rate of 100 wats for 12 hours. (the specific latent heat of vaporisation of water is 2.3MJkg-1)
Wednesday, June 1, 2011 at 6:19pm by Nelly
physics
The specific heat of mercury is .03cal/g*C, and it's boiling point is 357*C. The specific heat of water is 1 cal/g*C. It takes 65 calories of energy to vaporize one gram of mercury and 540 calories to vaporize one gram of water. If both substances begin at about 22*C does ...
Wednesday, January 25, 2012 at 8:31pm by Angel
Physics
An ice chest at a beach party contains 12 cans of soda at 2.45 °C. Each can of soda has a mass of 0.35 kg and a specific heat capacity of 3800 J/(kg C°). Someone adds a 9.60-kg watermelon at 25.3 °C to the chest. The specific heat capacity of watermelon is nearly ...
Sunday, May 5, 2013 at 12:47pm by Tim
Chemistry
An 850 gram chunk of ice at 0 degrees Celsius is dropped into a container holding 1.7 kg of water at an initial temperature of 35 degrees Celsius. Due to the presence of the ice, the temperature of the water eventually drops to 0 degrees Celsius. Show a mathematical solution ...
Sunday, January 29, 2012 at 4:52pm by Selena
Chemistry
A sample of silver with a mass of 63.3g is heated to a temperature of 384.4 K and placed in a container water at 290.0K The final temperature of the silver and water is 292.4K assuming no heat loss, what mass of water was in the container? the specific heat of water is 4.184J...
Sunday, February 21, 2010 at 7:35pm by Anonymous
chemistry
How much heat must be added to the water to move the T from Iinitial = 10 C to Tfinal = 16.4 C. That will be q = massH2O x specific heat water x (Tfinal-Tinitial) = ?? Knowing that 1 mol CaCl2 dissolving in water will produce 82.8 kJ, how many mols CaCl2 are required. Then ...
Monday, November 17, 2008 at 7:29pm by DrBob222
Chemistry
q1 = heat needed to raise T of solid ice from -20 to 0. q1 = mass ice x specific heat ice x (Tfinal-Tinitial). q2 = heat needed to melt the solid ice at zero to liquid at zero. q2 = mass ice x heat fusion. q3 = heat needed to raise T of liquid water from zero C to 100 C. q3 = ...
Monday, February 6, 2012 at 7:32pm by DrBob222
Physics
A 43 g ice cube at 0 C is placed in 882 g of water at 81 C. What is the final temperature of the mixture? The specific heat of water is 4186 J/kg · C and its latent heat of fusion is 3.33 × 105 J/kg . Answer in units of C
Tuesday, April 23, 2013 at 8:38pm by dallas
chemistry
q1 = heat to melt ice. q1 = mass ice x heat fusion. q2 = heat to raise T of liquid H2O from zero C to 100 C. q2 = mass H2O x specific heat H2O x (Tfinal-Tinitial) q3 = heat to vaporize the water q3 = mass water x heat vaporization. Total Q = q1 + q2 + q3
Thursday, April 26, 2012 at 11:56pm by DrBob222
Chemistry
It appears that ALL of the bath water is frozen and not just a part of it. heat lost by rocks + heat absorbed by ice melting + heat absorbed by liquid water to raise T to final T = 0 heat lost by rocks is mass rocks x specific heat rocks x (Tfinal-Tinitial) heat absorbed by ...
Friday, February 17, 2012 at 1:58pm by DrBob222
Lauren
The amount of heat required to raise temperature of 55.85 g of iron 1 degrees C is called its A. Change of energy B. Enthalpy C. Molar heat capacity D. Specific heat capacity E. Specific Heat.
Friday, November 16, 2007 at 4:42pm by Chemistry
chemistry
1.how do you calculate the specific heat of a metallic element if 314 joules of energy are needed to raise the temperature of a 50.0 g sample from 25.0 degrees c to 50.0 degrees c. 2. how do you propose a method for determining the specific heat for a metal like sodium which ...
Tuesday, October 2, 2007 at 7:11pm by S
Chemistry
You need to use Tfinal-Tinitial for delta T. heat lost by Al + heat gained by water=0 [mass Al x specific heat Al x (Tfinal-Tinitial)] + [mass H2O x specific heat H2O x (Tfinal-Tinitial)] = 0 Substitute and solve for Tf.
Sunday, April 24, 2011 at 5:50pm by DrBob222
AP Chemistry
energy in J = hc/wavelength.That is E in J for 1 photon. Multiply by 6.022E23 to find moles. How many seconds will it take to at 900 watts. Multiply by 60 seconds/min. Energy needed to heat water is mass water x specific heat water x (Tfinal-Tinitial) = q.
Tuesday, November 16, 2010 at 11:21pm by DrBob222
chemistry
q = mass H2O x specific heat water x delta T. Watch the units. It doesn't matter which "water" one uses, the change in T is 40 C. Heat flows from the warmer one to the cooler one. .
Thursday, June 16, 2011 at 7:44pm by DrBob222
AP Chemistry
Do you have specific heat water? ice? heat fusion?
Wednesday, January 23, 2013 at 5:01pm by DrBob222
Chemistry HEAT OF FUSION
#1. mass ice x deltaHfusion = ? #2. q = mass x specific heat x (Tfinal-Tinitial) = ? #3. You can put the pieces together. heat to melt ice + heat to raise T of melt from zero C to final T + heat lost by hot water going to lower final T.
Thursday, October 6, 2011 at 8:34pm by DrBob222
science
Specific heat of water: 4.187 kJ/kg-K Specific heat of steam: 1.996 kJ/-kgK Heat of vaporization = 540 kcal/kg heat removed per kg: 20*1.996 + 10*4.187 + 540 = 622 kcal/kg
Thursday, October 13, 2011 at 1:03am by drwls
chemistry
q = mass water x specific heat water x (Tfinal-Tinitial). You probably assume the density of water is 1.00 g/mL.
Sunday, September 11, 2011 at 8:43pm by DrBob222
physics
They need to tell you: (1) if water is flowing through, and at what rate (2) convective heat loss to the air. (3) radiative heat loss They probably expect you to assume no flow and neglect the loss terms. This will lead to a high prediction of the temperature rise. This is a ...
Saturday, March 3, 2012 at 11:18pm by drwls
chemistry
Compounds like CCl2F2 are known as chlorofluorocarbons, or CFCs. These compounds were once widely used as refrigerants but are now being replaced by compounds that are believed to be less harmful to the environment. The heat of vaporization of CCl2F2 is 289 J/g. What mass of ...
Wednesday, January 9, 2013 at 5:23pm by Samantha
uah
Writeacher is correct. I never would have clicked on uah. How much heat was gained by the cold water? mass x specific heat x (Tfinal-Tinitial) = ?? How much was lost by the hot water? mass x specific heat x (Tfinal-Tinitial) = ?? What's the difference? The difference is ...
Monday, March 8, 2010 at 11:12am by DrBob222
physics
What would be the final temp when 100 kg of 0 degrees Celcius cold water is mixed with 60 kg of 35 degrees warm water? Ans is in degrees Celcius. The sum of the heats gained is zero (remember one will lose heat, so have a negative heat gained). Heatgained by cold water + heat ...
Thursday, March 29, 2007 at 12:38am by Kristina
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