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July 29, 2014

Search: the specific heat of water is 4190 J/kg times degrees Celsius. what is the change in thermal energy when 500g of water cools from 45 degrees Celsius to 35 degrees Celsius

Number of results: 42,258

physical science
How much heat is required to raise the temperature of a 10.0 kg of aluminum by 80 degrees Celsius? Look up the specific heat of aluminum. The units will be Calories/kg*degC or Joules/kg*degC. Multiply that number by the temperature change (80 C) and the mass (10.0 kg). See ...
June 22, 2007 by jan

chemistry
If 7.24 kJ of heat is applied to a 952 g block of metal, the temperature increases by 10.7 degrees Celsius. Calculate the specific heat capacity of the metal in J/g degrees Celsius.
March 29, 2010 by Jack

CHEMISTRY
HOW MANY GRAMS OF ICE AT -5.2 DEGREES CELSIUS CAN BE COMPLETELY CONVERTED TO LIQUID AT 6.4 CELSIUS DEGREES IF THE AVAILABLE HEAT FOR THE PROCESS IS 441800kj,FOR ICE SPECIFIC HEAT IS 2.01
April 1, 2010 by LEBOHANG

Chemistry - General, Hess's Law
In an experiment, 11.6g of a salt was dissolved in 100.0ml of water contained in the above calorimeter, all at an initial tmperature of 24.5 degrees Celsius. After dissolution was complete, the temperatur was 31.8C. The specific heat of the solution is 3.63J/gxC and the ...
July 24, 2009 by Sahar

Chemistry
1. How much heat is absorbed when 63.7g H(small 2)O [water](l) at 100 degrees C and 101.3 kPa is converted to steam at 100 degrees C? Express your answer in kJ. Is there an equation? 2.How much heat (in kJ) is released when 0.677 mol NaOH(s) is dissolved in water? (Steps?) ...
May 12, 2010 by Anonymous

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 ...
June 24, 2011 by Tc

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 ...
October 12, 2010 by Anonymous

chemistry
When 45 grams of an alloy is dropped into 100.0 grams of water at 25 degrees celcius, the final temperature is 37 degrees celcius. what is the specific heat of the alloy? the alloys Temperature is 100 degrees celsius
June 11, 2008 by sdfsgfsf

chemistry
What will be the final temperature of the water in an insulated container as the result of passing 5.00 g of steam [H2O(g)] at 100.0C into 195.0 g of water at 20.0C? (?Hvap = 40.6 kJ/mol H2O) The best way to do these problems is to make the heat gained + heat lost = 0. q1...
October 12, 2006 by hal

Physic II
A person tries to heat up her bath water by adding 5.0 L of water at 80 degrees celcious to 60 L of water at 30 degrees celcious. What is the final temperature of the water? Show work please !
April 7, 2014 by hulune2

Chemistry Help!!!
1) When hydrazine (N2H4) is burned in a 253-g brick container, the temperature of the brick increases by 5.13 degrees Celsius. Calculate the quantity of heat released in this raection. The specific heat of brick is 0.840 J/(gC). 2) A sample of coal is burned in a bomb ...
November 14, 2010 by Sarah

Chem. Find specific heat capacity.
A piece of lead with a mass of 27.3 g was heated to 98.90oC and then dropped into 15,0 g of water at 22.50oC. The final temperature was 26.32oC. Calculate the specific heat capacity of lead from these data. THANK YOU FOR ANY HELP!
November 30, 2008 by Sarah

Physics
Please Help! I am having difficulties grasping these concepts. Explain please! 1. How much heat energy is required to change 500 grams of water at 100 degrees Celsius to steam at 100 degrees Celsius? 2. How much energy is lost if 7kg of water is cooled from 46 degrees Celsius ...
June 8, 2014 by Tamai

Chemistry
1) When hydrazine (N2H4) is burned in a 253-g brick container, the temperature of the brick increases by 5.13 degrees Celsius. Calculate the quantity of heat released in this raection. The specific heat of brick is 0.840 J/(gC). 2) A sample of coal is burned in a bomb ...
November 14, 2010 by Sarah

Chemistry
1) When hydrazine (N2H4) is burned in a 253-g brick container, the temperature of the brick increases by 5.13 degrees Celsius. Calculate the quantity of heat released in this raection. The specific heat of brick is 0.840 J/(gC). 2) A sample of coal is burned in a bomb ...
November 14, 2010 by Sarah

science
A heat exchanger is used to warm apple cider using steam as the heat source. The cider is heated from an initial temperature of 4 degrees celcius to a final temperature of 65 degree celcius. The steam enters the heat exchanger as 50% quality steam and exits as water condensate...
March 4, 2013 by Bev

Chemistry
A portable electric water heater transfers 255 watts (W) of power to 5.5 L of water, where 1 W = 1 J/s. How much time (in minutes) will it take for the water heater to heat the 5.5 L of water from 25 degrees celsius to 42 degrees celsius? (Assume that the water has a density ...
February 9, 2012 by Elle

Food Chemestry
A heat exchanger is used to warm apple cider using steam as the heat source. The cider is heated from an initial temperature of 4 degrees celcius to a final temperature of 65 degree celcius. The steam enters the heat exchanger as 50% quality steam and exits as water condensate...
March 4, 2013 by Bev

chemistry
Propane gas is used to heat a tank of water. If the tank contains 200 L of water, what mass of propane will be required to raise its temperature from 20 degrees C to 65 degrees C. The heat of combustion for propane is -2220 kJ/mol.
November 4, 2010 by Ray

Heat and Molar Mass
An aqueous solution containing 34.6 g of an unknown molecular nonelectrolyte compound in 142.0 g of water was found to have a freezing point of 1.2 degrees C. Calculate the molar mass. A sample of steam with a mass of 0.553 g and at a temperature of 100 degrees C condenses ...
January 15, 2013 by Amy

physic-heat
please list all the formulas for calculating the specific heat of a substance please. thanks specific heat = (heat added)/[(mass)(delta T)] That is the equation that defines specific heat. It should be the only equation you need. "delta T" is the increase in temperature. For ...
April 8, 2007 by Pauline

Chemistry
Steam at 100C was passed into a flask containing 250 g of water at 21C, where the steam condensed. How many grams of steam must have condensed if the temperature of the water in the flask was raised to 76C? The heat of vaporization of water at 100C is 40.7 kJ/mol and the ...
October 8, 2008 by Ryan

chemistry
calculate the heat energy required to raise the temperature of a 500. gram iron pipe from 25 degress celcius to 100 degrees celcius. the specific heat for iron is .45 J/g degrees celcius
May 12, 2013 by andrea

Energy multiple choice question
Which of the following samples has the highest specific heat capacity? a) A 100 kg sample of lead requires 13 000 J to increase its temperature by 1 K b) A 50 g sample of water releases 1050 J as it cools by 5 degree Celsius c) A 2 kg sample of copper receives 2340 J of ...
April 12, 2014 by Liz

Chemistry
An unknown substance has a mass of 16.3 g. The temperature of the substance increases by 20.1 degrees Celsius when 126 J of heat is added to the substance. What is the most likely identity of the substance? The table lists the specific heat capacities of select substances. ...
October 9, 2012 by Anonymous

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...
February 28, 2007 by Brown

physics
a banana with a temperature of 17 degrees C (specific heat of banana= 3520j/kgK) and a a mass of 250g is placed in a bowl of milk with a temperature of 8 degrees C and a mass of 350g (specific heat of milk= 4200 J/kgK). no heat is lost to the bowl or the air as the banana and ...
November 18, 2010 by Brittany

chemistry
85.0 of is initially at room temperature (22.0). A chilled steel rod at 2.0 is placed in the water. If the final temperature of the system is 21.2, what is the mass of the steel bar? Specific heat of water = 4.18 Specific heat of steel = 0.452 My answer was 32.752. I rounded ...
March 26, 2013 by Joshua

chemistry
85.0 of is initially at room temperature (22.0). A chilled steel rod at 2.0 is placed in the water. If the final temperature of the system is 21.2, what is the mass of the steel bar? Specific heat of water = 4.18 Specific heat of steel = 0.452 My answer was 32.752. I rounded ...
March 26, 2013 by Joshua

Chemistry
A piece of copper metal is initially at 100.0C. It is dropped into a coffee cup calorimeter containing 50.0 g of water at a temperature of 20.0C. After stirring, the final temperature of both copper and water is 25.0C. Assuming no heat losses, and that the specific heat (...
May 5, 2014 by Chris

chemistry
3.) A 5.00 x 10^2 g block of metal absorbs 5016 joules of heat when its temperature changed from 20 degrees C to 30 degrees C. Calculate the specific heat of the metal. I used the formula and came with two answers 100.32 joules and 10.01 joules. Which is correct?
February 9, 2008 by mhaidar9108

Chemistry
What is the specific heat of Gold if 15.3 J of heat changes 12 grams by 8 degrees Celsius? I got 7.834, would this be correct do you think? Thanks Jiskha.
June 9, 2009 by Jay

Chemistry
The amount of heat required to raise 200 g of aluminum by 10 degrees celsius if its specific heat is 0.897 J/gC ? I need help. This is all confusing.
May 20, 2014 by Katherina Ramos

Chemistry
HELP!!! An unknown metal having a mass of 14.00g is dropped into 11.00mL of water at 20.0 degrees Celcius. The starting temperature of the chunk of metal is 100.0C. The final temperature of the water and metal is 32.5C. What is the specific heat of the metal?
April 6, 2011 by Marie

physics
A 75.00-g sample of an unknown metal is heated to 52.00C. It is then placed in a coffee cup calorimeter filled with water. The calorimeter and the water inside have a combined mass of 225.0 g and an overall specific heat of 2.045 J/(giC). The initial temperature of the ...
June 27, 2014 by adam

Chemistry
If 22 g of water is heated so that the water temperature rises from 18.1C to 21.5C, how many calories have been absorbed by the water? The specific heat of water = 1.00 cal / (g C)
October 25, 2010 by Cassie

Chemistry
A 300 Calorie donut is used to heat 5.0 kg of water. If the initial temperature of the water is 20 degrees C what will the final temperature of the water be? Assume no heat loss to the surroundings
March 11, 2009 by Kayla

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.
October 23, 2008 by Lilit***

physics
The specific heat capacity of steel is 445 Jkg K. How much energy is required to raise the temperature of a 0.410g of kettle which contains 1.2L of water from 20 degrees Celsius to boiling point?
July 23, 2010 by Anonymous

physics
A snake is sunning itself on a rock. (a) If the snake is 0.3 m long, what is the approximate amount of radiation it absorbs from the sun in 10 minutes? (b) If no heat flows out of the snake via conduction or by evaporative cooling, how much does its temperature increase during...
April 12, 2011 by Sandhya

Physic II
A person tries to heat up her bath water by adding 5.0 L of water at 80 degrees celcious to 60 L of water at 30 degrees celcious. What is the final temperature of the water?
April 7, 2014 by hulune2

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
March 31, 2008 by natash

physics
1 kg of ice at 0 C is mixed with 9 kg of water at 50 C (The latent heat of ice is 3.34x105 J/kg and the specific heat capacity of water is 4160 J/kg). What is the resulting temperature?
January 23, 2011 by calous --- HELP PLEASEE!!!

ThermoChemistry
When 19 mL of water at 22 C is combined with 18 mL of water at 64 C, what is the final temperature of the water?. The specific heat of water is 4.184 J/g/K and its density is 1.0 g/mL.
December 2, 2011 by LaurenB

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...
February 27, 2012 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 ...
February 27, 2012 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 ...
February 27, 2012 by Abby

Chemistry
Calculate the final temperature when 20.0 g at 60 *C iron is put into 50.0 ml of 20 *C water. The specific heat of iron is 0.449 J/g*C and that of water is 4.184*C. (Assume no heat is lost to the container or the surrounndings.)
November 29, 2010 by Stacy

chemistry
How much heat flows from 20kg of 90 degrees water placed in contact with 20kg of 10 degrees water, producing a final temperature of 50 degrees? c=4186j/kgC
June 16, 2011 by jessica

physics
In lab, Will burns a 0.6 g peanut beneath 48 g of water, which increases in temperature from 22 degree C to 55 degree C. The amount of heat absorbed by the water can be found with the equation Q =cm \Delta T, where Q is the amount of heat, c the specific heat of water, m the ...
April 3, 2012 by christy

chemistry
Calculate the enthalpy change for converting 10.0g of ice at -25 degrees Celsius to water at 80 degrees Celsius. The specific heats of ice, water, and steam are 2.09j/g degrees Celsius, 4.18j/g degrees Celsius, and 1.85j/g degrees Celsius. The enthalpy of fusion for water is 6...
March 28, 2012 by Brittany

Chemistry
A calorimeter contains 50.0 mL of water; both are at 21.2 degrees C. Then the 50.0 mL of water at 57.6 degrees C is added to the calorimeter. At equilibrium, the final temperature of the water and the calorimeter is 33.3 degrees C. Calculate the heat capacity, C, of the ...
October 22, 2013 by Jay

Chemistry
How would I calculate these? I have the answers because there from a previous test. 1) How much heat is required to raise the temperature of a 5.52-g sample of iron ( specific heat = 0.450 J/g C) from 25.0 degrees C to 79.8 degrees C? 2) You mix 60. mL of 1.00 M silver nitrate...
June 30, 2013 by Mary

physics repost
How much heat must be removed from 0.15 kg of water to cool it from 95 d/C to 25 d/C? The specific heat capasity of water is 4182 J/kg-k. mC(T1-T2) 0.15(4182)(70) = 4.4 x 10^4 J
April 4, 2008 by Jon

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.
October 30, 2010 by May

science grade 5
how is heat related to temperature? Temperature tells us the DEGREE of heat; i.e., how hot is something. A temperature of 98.6 F is normal body temperature. A hot day is when the temperature is 95 degrees F. A cold day is when it is freezing outside. But the heat something ...
November 15, 2006 by kathy

chem
What would happen to the specific heat if some of the warm metal shot were lost during the transfer to the calorimeter? Answer a. It would not affect the calculated value of specific heat b. It would cause the calculated value of specific heat to be artificially high c. It ...
October 24, 2010 by kellie

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?
September 23, 2012 by Claire

physics
A flow calorimeter is used to measure the specific heat of a liquid. Heat is added at a known rate to a stream of the liquid as it passes through the calorimeter at a known rate. Then a measurement of the resulting temperature difference between the inflow and the outflow ...
September 23, 2013 by Chip

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?
September 26, 2011 by D

Chemistry
When 100 mL of Ba(NO3)2 solution at 25 degrees Celsius is mixed with 100 mL solution CaSO4 solution at 25 degrees Celsius in calorimeter, the white solid BaSO4 forms and the temperature of the mixture increases to 28.1 degrees Celsius. Assuming that the calorimeter absorbs ...
December 9, 2012 by Megan

AP Chemistry
A 2.75 g sample of the hydrocarbon acetone, CH3COCH3, is burned in a bomb calorimeter with 975 mL of water, initially at 23.50 degrees celsius. The bomb is constructed of 285.0 g of nickel metal having a specific heat capacity of Cp = 0.826 J/ g degrees C. The final ...
September 30, 2007 by Kate

AP CHEMISTRY
A 2.75 g sample of the hydrocarbon acetone, CH3COCH3, is burned in a bomb calorimeter with 975 mL of water, initially at 23.50 degrees celsius. The bomb is constructed of 285.0 g of nickel metal having a specific heat capacity of Cp = 0.826 J/ g degrees C. The final ...
September 30, 2007 by Kate

CHEMISTRY
A 2.75 g sample of the hydrocarbon acetone, CH3COCH3, is burned in a bomb calorimeter with 975 mL of water, initially at 23.50 degrees celsius. The bomb is constructed of 285.0 g of nickel metal having a specific heat capacity of Cp = 0.826 J/ g degrees C. The final ...
September 30, 2007 by Jake

chemistry
calculate the specific heat (j/g C ) for each of the following: -an 18.5-g sample of tin that absorbs 183 J when its temperature inceases from 35.0 degrees C to 78.6 degrees C
September 14, 2010 by kelly

Chemistry
What is the specific heat of an unknown substance if a 2.45g samples releases 12.9 cal as its temperature changes from 25.1 degrees C to 20.1 degrees C?
April 27, 2014 by Ashley

Chemistry
Calories of heat absorbed by water = (Mass undergoing change)(Change in temp.)How much heat is needed to warm 125 g. of water from 25 degrees Celsius to 100 degrees Celsius. Thank you very much!
January 30, 2013 by Larissa Jenkinson III

Chemistry
What is the total heat evolved when a saturated solution of boric acid (H3BO3) in water is cooled from 100C to 20C? Note the specific heat capacity of the saturated solution is approximately that of water in that temperature range (4.20 J/g.K) and the specific heat capacity of...
March 23, 2014 by Marlee

physics
How much heat must be removed from 0.15 kg of water to cool it from 95 d/C to 25 d/C? The specific heat capasity of water is 4182 J/kg-k. mC(T1-T2) 0.15(4182)(70) = 4.4 x 10^4 J
April 3, 2008 by Jon

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)?
April 4, 2010 by demond

Science
"a glass of water is at 60 degrees C if the temperature of water drops to 40 degrees C its specific volume will?
November 7, 2011 by John Wilson

Physics
How do I find out how much heat it takes to raise the temperature of 100 grams of aluminum from 50 degrees celcius to 80 degrees celsius. The specific heat is 900j/kg First I did 100*30*900 and it equalled 2,700,000. that seems to high, is it? I then multiplied 100*30*.9 and ...
June 27, 2010 by Carissa

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 it ...
January 25, 2012 by Angel

Chemistry
could someone help me with this question? A quantity of 400 mL of .6 M HNO3 is mixed with 400 mL of .3 M Ba(OH)2 in a constant pressure calorimeter of negligible heat capacity. The initial temperature of both solutions is the same at 18.46 degrees Celsius. What is the final ...
April 25, 2010 by Tokey

physics
At a fabrication plant, a hot metal forging has a mass of 78.5 kg and a specific heat capacity of 426 J/(kg C). To harden it, the forging is quenched by immersion in 788 kg of oil that has a temperature of 30.3 C and a specific heat capacity of 2770 J/(kg C). The final ...
May 5, 2011 by shaknocka

physics
At a fabrication plant, a hot metal forging has a mass of 66.8 kg and a specific heat capacity of 437 J/(kg C). To harden it, the forging is quenched by immersion in 785 kg of oil that has a temperature of 25.0 C and a specific heat capacity of 2770 J/(kg C). The final ...
April 28, 2012 by RC

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)
June 1, 2011 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)
June 2, 2011 by Nelly

Chemistry/Calorimetry
You buy coffee (200.0 ml) served in a styrofoam cup. You are up late working in a chemistry lab, and want to drink the coffee right away, but at 95.0 degrees C, it is too hot to drink. You like the temperature of your coffee to be 79.0 1.0 degrees C. You decide that the ...
February 23, 2012 by Jen

Chemistry
A piece of Copper alloy with a mass of 89.0 g is heated at 30.0 degrees C to 50.0 degrees C. In the process, it absorbs 517 J of energy as heat. What is the specific heat of this copper alloy? and Please do a step by step, I really want to see where I keep going wrong.
January 16, 2012 by Anonymous

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
January 28, 2012 by jessica

Chemistry Urgent
95.0mL of H2O is initially at room temperature (22.0∘C ). A chilled steel rod at 2.0∘C is placed in the water. If the final temperature of the system is 21.3∘C , what is the mass of the steel bar? Specific heat of water = 4.18 J/g⋅∘C Specific heat...
March 11, 2014 by Anna

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

chemistry
How much energy (in kJ) is released when 16.4 g of steam at 121.5 degrees C is condensed to give liquid water at 60.5 degrees C? The heat of vaporization of liquid water is 40.67 kJ/mol and the molar heat capacity is 75.3 J/(K*mol) for the liquid and 33.6 J?(K*mol) for the vapor.
January 24, 2012 by Becca

Chemistry - Heat of Fusion of Ice
Conclusion question(s) from a lab we did to find the heat of fusion of ice: Does the value obtained for the molar heat of fusion depend on the volume of water used? Does it depend on the mass of ice melted? Does it depend on the final temperature of the mixture? The heat of ...
October 1, 2006 by J.M.

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

Chemistry
If 50.00mL of 1.10M NaOH is added to 25.00mL of 1.86M HCl, with both solutions originally at 24.70 degrees Celsius, what will be the final solution temperature? (Assume that no heat is lost to the surrounding air and that the solution produced in the neutralization reaction ...
October 5, 2012 by Tasnim

chemistry
A 100.0 ml sample of 0.300 M NaOH is mixed with a 100.0 ml sample of 0.300 M HNO3 in a coffee cup calorimeter. Both solutions were initially at 35.0 degrees celcius; the temperature of the resulting solution was recorded at 37.0 degrees celcius. Determine the delta H (in units...
July 12, 2012 by jen

College Chemistry
What is the final temperature, in oC, after a 26.5 g piece of ice, at 0oC, is placed in a styrofoam cup with 122 g of water initially at 73.8oC the specific heat of water = 4.184 JK-1g-1 The heat of fusion of ice = 333 Jg-1
October 7, 2011 by John

Chemistry
A 2.75 g sample of the hydrocarbon acetone, CH3COCH3, is burned in a bomb calorimeter with 975 mL of water, initially at 23.50 degrees celsius. The bomb is constructed of 285.0 g of nickel metal having a specific heat capacity of Cp = 0.826 J/ g degrees C. The final ...
September 30, 2007 by Kate

Chemistry
A 2.75 g sample of the hydrocarbon acetone, CH3COCH3, is burned in a bomb calorimeter with 975 mL of water, initially at 23.50 degrees celsius. The bomb is constructed of 285.0 g of nickel metal having a specific heat capacity of Cp = 0.826 J/ g degrees C. The final ...
September 30, 2007 by Kate

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 ...
January 9, 2013 by Samantha

Chemistry
Calculate the amount of heat in joules required to heat 43 grams of water from 28 degrees celcius to the normal boiling point 100 degrees celcius
October 12, 2012 by Anonymous

chemistry
How much heat is required to warm 1.30 L of water from 30.0 degrees C to 100.0 degrees C? (Assume a density of 1.0 g/mL for the water.)
October 18, 2010 by Mely

physics
A transfer of heat occurs with a pot of 8.0 kg of water that changes from 400 degrees kelvin to 320 degrees kelvin. How much heat is absorbed or given off?
October 19, 2008 by sammi

chemistry
When a 28.8mL of .500M H2SO4 is added to 28.8mL of 1.00M KOH in a coffee-cup calorimeter at 23.50 degrees Celsius, teh temperature rises to 30.17 degrees Celsius. Calculate the ^H(change in enthalpy)of this reaction. (assume total volume is the sum of individual volumes and ...
October 12, 2008 by Kelsie

Chemistry
Assume that 57.0 cal of heat is applied to a 28g sample of sulfur at 27 degrees C. What is the final temperature of the sample if the specific heat of sulfur is 0.175 cal/g degrees C?
December 9, 2012 by Marie

chemsitry
A sample consisting of 0.025 mol of a solid compound is placed inside a metal cylinder. The cylinder was immersed in a water bath consisting of 10.00 kg of water at an original temperature of 25.00 C. When the compound decomposes, the temperature of the water rises to 29.52 ...
October 23, 2010 by Nora

physics
134 g of water at 7C is added to ice at 0C. If the final temperature of the system (which you can assume is isolated) is 0C, determine HOW MUCH ICE MELTED. The specific heat of water is 4186 J/kgC. The latent heat of fusion for H2O is 335,000 J/kg.
November 14, 2012 by Joseph

Chemistry
A person falls in water at 0 degrees C. After 20 minutes of exposure, they are suffering acute hypothermia, as their core body temperature has dropped to 30.0 degrees C. Assume that a persons heat capacity can be approximated by the heat capacity of water, 4.18 J/g/oC. The ...
November 20, 2007 by Raj

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