Calorimetry

Key Questions

• What is the relationship between heat and calorimetry?

  Calorimetry is an experimental method that allows one to calculate the heat change in a chemical process.

  calorimeter is just a reaction vessel. It could be a foam cup, a soda can, or a commercially available bomb calorimeter like http://www.parrinst.com/products/oxygen-bomb-calorimeters/1341-plain-jacket-bomb-calorimeter/.

  Basically, you have a certain amount of water surrounding a reaction. You measure the temperature change in that water, and you use that to calculate the heat gained or released during a process. That equation usually takes a form:

  #-q_(rxn) = q_(cal) + q_(water)#

  Where q represents the heat change in the reaction, the calorimeter and the water. Since you are only measuring temperature, you will need to calculate the heat using it.

  The change in heat of the calorimeter is given by:
  #q_(cal) = CDeltaT# where C is the heat capacity of the calorimeter.

  The change in heat of the water is given by:
  #q_(water) = c_(p)mDeltaT# where #c_p# is the specific heat of water, which is 4.184 J/gC, m is the mass of water in the calorimeter in grams, and delta T is the change in temperature.

  The video discusses how to solve a sample calorimetry calculation.
  
  Video from: Noel Pauller

  See here for more sample calculations:
  http://www.chem.ufl.edu/~itl/2045/lectures/lec_9.html

  Another video on calorimetry:
  

  ChemGuy · 3 · Apr 13 2014
• How do you measure calorimetry?

  Calorimetry is the measurement of heat flow.

  Heat energy flows from a substance that has a higher temperature to a substance that has a lower temperature. The heat will continue to flow until both substances reach the same temperature, known as the final temperature.

  A device called a calorimeter is used to measure heat flow. It consists of nested styrofoam cups. In a high school chemistry class we generally study the heat exchange between hot metals and water or water samples at different temperatures. The nested styrofoam cups are insulators so that all the heat is transferred from the warm object to the cooler one.

  The equation for heat, q = m x #C_s# x #deltaT# is used for calorimetry. The heat lost by the warm object is equal to the heat gained by the cooler object:
  Q lost by the hot material = Q gained by the cold material
  We can set up the following equation to solve for any part of the heat calculations
  [ Mhot x #C_s#hot x (#T_f# - #T_bhot)] - [Mcold x C_s# cold x (#T_f# -#T_b#cold)] = 0

  #C_s# is the specific heat of the material. M is mass and T is temperature.

  The video discusses how to solve a sample calorimetry calculation.
  
  Video from: Noel Pauller

  Another video on calorimetry:
  

  Corinne F. · 1 · Feb 19 2014
• What is calorimetry?

  The process of measuring the heat released in any type of reactions like chemical and physical reactions.

  This is the definition of calorimetry.

  It is measured by calorimeter.

  Xenoz · 3 · Jul 5 2018

• How does differential scanning in calorimetry work?
• What information do you get from a differential scanning calorimetry plot?
• How do you measure calorimetry?
• Question #962a7
• Question #1dfc5
• Question #41af6
• What is calorimetry?
• What is a differential scanning calorimeter?
• How can a calorimeter measure energy?
• What are calorimeters made of?
• What are the principles of calorimetry?
• What is adiabatic calorimetry?
• How is calorimetry used in the industry?
• Why is bomb calorimetry important?
• When is indirect calorimetry necessary?
• What is the relationship between heat and calorimetry?
• Question #45e82
• Question #b6523
• Question #b6a86
• Question #5d3f9
• Question #1dda3
• Question #5efd7
• Question #d33b2
• How is Q= mCdeltaT used, what are the variables, what are the units, and how does it work?
• Question #56d6d
• Question #1c0c4
• A cup of tea containing 400.0 g of liquid at 20.0 degree C was heated. If 58.5 kJ of heat was added to the tea, what would be the final temperature? Assume that the specific heat is the same as that of water( 4.18 J g c)
• Question #fa6dc
• 11. 135 g of aluminum (initially at #"400"^("o")"C"#) are mixed with an unknown mass of water (initially at #"25"^("o")"C"#). When thermal equilibrium is reached, the system has a temperature of #"80"^("o")"C"#. Find the mass of the water?
• Question #37748
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• Question #62519
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• Question #c91cf
• The specific heat of liquid bromine is 0.226J/g-K and the density is 3.12g/mL, how much heat (J) is required to raise the temperature of 10.0mL of bromine from 25.00 C to 27.30 C?
• If 65.34g piece of tin were to lose 754 Joules of energy in a calorimeter while experiencing a temperature change from 23.9 degrees C to 22.0 degrees C, how would you find its specific heat?
• The specific heat capacity of liquid water is 4.18 kJ/g C, how would you calculate the quantity of energy required to heat 1.00 g of water from 26.5 C to 83.7 C?
• A 30-0 g sample of water at 280 K is mixed with 50.0 g of water at 330 K. How would you calculate the final temperature of the mixture assuming no heat is lost to the surroundings?
• #"1351 J"# of energy are required to heat a #"0.125 kg"# sample of a metal from #25.0^@"C"# to #112.1^@"C"#. What is the specific heat of the metal?
• If the specific heat of water is 4.18J/g°C, how many joules of heat are given off when 5.0 g of water cool from 45°C to 25°C?
• If 26.03 g of water showed a temperature increase of 102°C upon addition of hot metal, what is the heat change for the water?
• A substance has a molar mass of 40.0g/mol. If the decomposition of 1.00mole of this substance absorbs 60.0KJ of energy, how much energy would be absorbed by the decomposition of 20.0g of the substance?
• Question #eca79
• A 1.50-kg iron horseshoe initially at 600.0°C is dropped into a bucket containing 20.0 kg of water at 25.0°C. What is the final temperature?
• Question #bcfb3
• Question #8e0a7
• What is the final temperature of water if 380 grams of water at 36°C absorb 47880 joules of energy?
• Question #0e53e
• An unknown volume of water at 18.2°C is added to 33.5 mL of water at 35.0°C. If the final temperature is 23.5°C, what was the unknown volume?
• To calculate the heat absorbed by an object, what information is needed besides its specific heat?
• The temperature of 50.0 g of water was raised to 50.0°C by the addition of 1.0 kJ of heat energy. What was the initial temperature of the water?
• Question #df236
• Two identical cups of cocoa are sitting on a table. One has a metal spoon in it and one doe snot. After five minutes, which is cooler, and why?
• A 100.0g ice cube at 0.0°C is placed in 650g of water at 25°C . what is the final temperature of the mixture?
• When one object heats another, does the temperature increase of one object always equal the temperature decrease of the other object?
• What is the energy transfer when you touch a block of ice with your hand?
• Question #0e523
• What minimum mass of ice is needed so that a glass of water at #25^@ "C"# is cooled down to #0^@ "C"# before the ice completely melts?
• A serving of Cheez-Its releases 130 kcal (1 kcal = 4.18 kJ) when digested by your body. If this same amount of energy were transferred to 2.5 kg of water at 27°C ,what would the final temperature be?
• Question #da1ce
• 350g of 0.0°C ice cubes are placed in a glass of 700g of room temperature water (23.0°C) in an experiment. Later, the temperature of the water in the glass is measured at 13.0°C. Does all of the ice melt?
• If 200 grams of water is to be heated from 24°C to 100°C to make a cup of tea, how much heat must be added?
• How many calories are absorbed by a pot of water with a mass of 500 g in order to raise the temperature from 20° C to 30° C?
• How many joules are required to heat 15.2 g of water at 35.0°C to 70.0°C?
• Question #a6d1a
• How much energy is absorbed as heat by 21 g of gold when it is heated from 25°C to 35°C?
• How much heat is required to convert 5.88 g of ice at -12.0°C to water at 25.0°C, if the heat capacity of ice is 2.09 J/°C?
• Question #d5e47
• Question #fdbe9
• What are the steps to this basic thermodynamics equation?
• How many calories of energy must be added to a 1 gram of water to increase its temperature by 1 degree?
• How much heat (kJ) is needed to raise the temperature of 100.0 grams of water from 25.0°C to 50.0°C?
• If a sample of chloroform is initially at 25°C, what is its final temperature of 150.0 g of chloroform absorbs 1.0 kilojoules of heat, and the specific heat of chloroform is 0.96 J/g°C?
• To what temperature will a 50.0 g piece of glass raise if it absorbs 5275 joules of heat and its specific heat capacity is 0.50 J/g°C, if the initial temperature of the glass is 20.0°C?
• Question #086d5
• What would be the final temperature if #3.31 * 10^3# joules of heat were added to 18.5 grams of water at 22.0°C?
• Question #b29dc
• How much heat is released when 275 g of water cools from 85.2°C to 38.4 °C?
• What is the mass of a piece of copper when 3000 J of heat is applied, causing a 45 °C increase in temperature, if the #C_p# of copper is .38452 J/g °C?
• What would be the final temperature if you mixed a liter of 32°C water with 4 liters of 20°C water?
• How much heat is needed to raise the temperature of 5.58 kilograms of iron from 20.0°C to 1000.0°C?
• Question #f0003
• A 32 gram sample of vanadium was heated to 75°C, and placed in a calorimeter containing water at a temperature of 22.5°C. The final temperature of both the metal and the water was 26.3°C. What is the mass of the water in the calorimeter?
• How much heat is added to 10.0 g of ice at -200°C to convert it to steam at 120.00°C?
• Given a consistent source of heat, about how much longer would it take to boil 100 g of water at 100°C than to melt 100 g of ice at 0°C?
• How much energy is needed to change 1 g of ice at 0°C to water at 0°C?
• A sample of metal with a specific heat of .502 J/g°c is heated to 100.0°C and then placed a 50.0 g sample of water at 20.0°C. The final temperature of the system is 76.2°C. What is the mass of the metal used in process?
• What is the total energy required to bring 3 kg ice from -10°C to 110°C?
• How many kilojoules are released when 8.2 g of water condenses at 100°C and cools to 15°C?
• Question #acab0
• How much heat do you need to raise the temperature of 150 g of ice from -30°C to -15°C?
• If you combine 360.0 mL of water at 25.00°C and 120.0 mL of water at 95.00°C, what is the final temperature of the mixture?
• Question #3c141
• #1.2 xx 10^5# #J# of thermal energy are added to a sample of water and its temperature changes from #229# #K# to #243# #K#. What is the mass of the water?
• To what temperature will a 45.0 g piece of glass rise if it absorbs 6875 joules of heat and its specific heat capacity is 0.50 J/g°C? The initial temperature of the glass is 18.0°C.
• In a calorimeter, 20 g of ice absorbs heat with an enthalpy of fusion of 334 J/g. What is the heat absorbed?
• How does molecular shape affect polarity?
• Question #7c911
• Question #2e6dd
• Question #3d723
• What is the final temperature when 50 mL of water at 80°C are added to 25 mL of water at 25°C?
• Question #71e95
• A certain mass of water was heated with 41,840 Joules, raising its temperature from 22.0°C to 28.5°C. What is the mass of the water, in grams?
• How many grams of water would require #2.20 * 10^4# calories of heat to raise its temperature from #34.0°C# to #100.0°C#?
• An ancient copper coin was found to absorb 545.8 J of heat when the temperature increases 31.4 C°. The specific heat of copper is 0.387 J/g°C. What is the mass of the copper coin?
• Molten iron is extremely hot, averaging about 1,500°C The specific heat of iron is 0.46 J/g°C. How much heat is released to the atmosphere when 1 kg molten iron cools to room temperature (25°C)?
• Question #e1989
• Mass spectroscopy is an analytical technique which involves ? a. production of gaseous ions from a sample b. separation of the gaseous ions c. measurement of the relative abundance of the gaseous ions d. all of the above
• Question #2e81a
• How much energy is required to raise the temperature of a #300*g# mass of water by #75*K#?
• What would be the final temperature if you mixed a liter of 20°C water with 2 liters of 40°C water?
• What would be the final temperature when 100 g of 25° C water is mixed with 75 g of 40°C water?
• How will the temperature of a calorimeter solution change for an exothermic reaction?
• What is the final temperature of 400 g of water at 20°C after it absorbs 226 kJ of heat?
• Question #02750
• Question #d4a35
• The specific heat of silver is 0.24 J/g°C. How many joules of energy are needed to warm 7.37 g of silver from 25.0°C to 27.5°C?
• An average baked potato contains 164 calories. What is the energy value of the potato in joules?
• When #1.0# #g# of potassium chloride, #KCl#, is dissolved in #25# #mL# (=#25# #g#) of water, it causes the temperature to drop from #24.33^o# #C# to #22.12^o# #C#. What is the molar enthalpy of dissolution for #KCl#?
• Why is it necessary to stir the calorimeter in an experiment?
• Calorimetry is based on what basic concepts?
• What is the final temperature after 840 J is absorbed by 10.0 g of water at 25°C?
• How many calories are required to raise the temperature of 225 g of water from 42°C to 75°C?
• How many grams of water would require 22,000 of heat to raise its temperature from 100.0°C?
• How much heat is given off when a 24.7 kg iron ingot is cooled from 880°C to 13°C?
• A 4.0 g sample of iron was heated from 0°C to 20°C. It absorbed 35.2 J of energy as heat. What is the specific heat of this piece of iron?
• How much heat is needed to raise the temperature of 25 g of a substance by 15°C when the specific heat is .92 J/g-°C?
• How much heat is required to raise the temp of 654 g of water from 34.5°C to 89.7°C?
• How much heat is required to warm 1.60 L of water from 26.0°C to 100.0°C?
• What is the mass of liquid water required to absorb #4.32*10^5# #kJ# of heat energy upon boiling?
• How much heat is required to raise the temperature of a 50.0 g block of iron by #10.0^@"C"# ? Specific heat of iron: #"0.449 J/g"""^@"C"#
• How many joules of heat energy would be required to raise the temperature of 150.0 g of aluminum from 23°C to 150°C?
• How much heat is required to warm 1.60 kg of sand from 22°C to 100°C?
• A sample of #H_2O# with a mass of 46.0 grams has a temperature of -58.0°C. How many joules of energy are necessary to heat the ice to 0°C?
• If you combine 250.0 mL of water at 25°C and 120.0 mL of water at 95°C, what is the final temperature of the mixture?
• Question #0295b
• How much heat is needed to raise 26 g of iron from 25°C to 45°C?
• How many joules are required to heat 250 grams of liquid water from 0°C to 100°C?
• Question #84e43
• Question #d9771
• You have a 189 gram sample of ice at -20°C. What is the total energy required to convert this sample to steam at 115°C?
• A sample of drinking water severely contaminated with chloroform , CHCl3 ,is supposed to be carcinogenic in nature . The level of combination was 15 ppm (by mass) .What is the molality of chloroform in the water sample ?
• Question #fe40a
• Given the Following: heat of fusion of ice = 80.0 cal/g; specific heat of ice = 0.480 cal/g; and specific heat of water = 1.00 cal/g. Calculate the amount of heat required to melt 30.0 g of ice at 0 degrees celsius?
• Solid magnesium has a specific heat of 1.01 J/g°C. How much heat is given off by a 20.0 gram sample of magnesium when it cools from 70.0°C to 50.0°C?
• How much heat is released when 88.2 g of water cools from 33.8°C to 12.9°C?
• Question #8e7c8
• Question #b4cdf
• The specific heat of ice is 0.492 cal/(g × °C). How many calories of heat are required to raise 100.0 g of ice from -20.0 °C to -0.5 °C?
• A 1 kg bar of gold at 150°C was placed in 3 kg of water that was originally at 20°C. What happened to the water?
• Question #e69fc
• If you combine 300.0 mL of water at 25.00°C and 110.0 mL of water at 95.00°C, what is the final temperature of the mixture?
• Question #9b8be
• How much energy would it take to melt 1 aluminum soda can if the can starts out at 20°C, melts at 660°C, and has a mass of 14 g?
• Question #8ad50
• Question #0c3b6
• How much energy is needed to raise the temperature of 2.0 g of water 5.00°C?
• A silver block, initially at 58.5°C, is submerged into 100.0 of water at 24.8°C in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 26.2 °C. What is the mass of the silver block?
• What is the amount of heat liberated (in kJ) from 327 g of mercury when it cools from 77.8°C to 12.0°C?
• A 5.82-kg piece of copper metal is heated from 21.5°C to 328.3°C. What is the heat absorbed (in kJ) by the metal?
• How much heat is added when 22 grams of water are heated from 10°C to 15°C?
• How much heat is given off when 10 grams of water are cooled from 50°C to 40°C?
• Question #fc006
• The heat of fusion for water is 80. cal/g. How many calories of heat are needed to melt a 35 g ice cube that has a temperature of 0 C?
• 900 kg water have T1 = -40 C, T2 = 0C and T3 = 5 C, How much energy is needed to melt this mass of water in 2 hours? Thank you so much.
• Question #97a5e
• Suppose that 25 g of aluminum is initially at 27.0 C. What is the final temperature of aluminum upon absorbing 2,35 kJ of heat? (#c= 0.903 J/g. ^0C#)?
• Question #ade0c
• Question #64f37
• Question #8451f
• Question #a540a
• Water (2290 g) is heated until it just begins to boil. If the water absorbs #5.47xx10^5 J# of heat in the process what was the initial temperature of the water?
• Question #6493b
• Question #9a717
• Question #93a6f
• Question #29480
• Question #2f390
• Question #ef8fb
• In calorimetry, we often define #q_(sys) = 0#. What assumptions about the calorimeter make this possible?
• What is the final temperature if a metal at #75^@ "C"# is dropped into #"185 g"# of water starting at #25^@ "C"#? The heat capacity of the metal is #"55 J/g"*""^@ "C"#.
• Question #1c6ef
• Question #bfecf
• Two solutions, initially at 24.60 degrees celsius are mixed in a coffee cup calorimeter (Ccal = 15.5 J/ degree celsius). When a 100.0 mL volume of 0.100 M AgNO3 solution is mixed with a 100.0 mL sample of 0.200 M NaCl solution...?
• Question #6b9c1
• Question #23181
• Why do we often write the water product as a gas in complete combustion reactions?
• Question #93e81
• Question #8c237
• Question #f16a3
• The specific heat of a certain type of metal is 0.128 J/(g·°C). What is the final temperature if 305 J of heat is added to 83.0 g of this metal initially at 20.0 °C?
• How do I decide what mass and specific heat capacity to use to find the heat involved when I place a hot ionic solid into water? Do I use the mass of the solid or the water?
• What is the unit used to measure the amount of energy in food?
• Question #cf198
• What mass of water will change its temperature by 3 C when 525 J of heat is added to it? The specific heat of water is 4-.8 J/gC
• (full question below) "How much water would you expect to vaporize, assuming no water splashes out?"
• What mass of ethanol #C_2H_5OH(l)# must be burned to supply 500.0 kJ of heat?
• Question #6ad9d
• For the reaction: #2H_2O + 137 kcal -> 2H_2(g) + O_2(g)# how many kcal are needed to form 2.00 moles #O_2(g)#?
• How do you determine the mass of a water sample that is heated from an initial temperature of 25 deg C to a final temperature of 100 deg C following the addition of 1200 J of heat energy?
• Question #b5be7
• How did you get #9.5%# for the theoretical yield of the potato chips in the Food Calorimetry Lab? I get #11%#.
• How much heat is required to heat ethanol from #25^@ "C"# to a gas at #78.24^@ "C"#? #C_P = "2.460 J/g"^@ "C"#, #DeltaH_(vap)^@ = "38.56 kJ/mol"#, #T_b = 78.24^@ "C"#
• How much #NO(g)# would form if #513.4*J# were pumped into the reaction?
• Question #0b2c1
• A 2.2 g sample of quinone #C_6H_4O_2# was burned in a bomb calorimeter for which the total heat capacity is 7854 J/°C. The temperature of the calorimeter increased from 23.44 C to 30.57 °C. What is the molar heat of combustion of quinone (in kJ/mol)?
• Question #3c48f
• If #"85 mL"# of #"0.900 M"# #"HCl"# is combined with #"85 mL"# of #"0.900 M"# #"KOH"# in a coffee-cup calorimeter, and the heat capacity of the calorimeter is #"0.325 kJ/"^@ "C"#, what is the final temperature if the initial temperature was #18.24^@ "C"#?
• How do you calculate total calories of a protein?
• Question #69369
• A 36-gram sample of water has an initial temperature of 22°C. After the sample absorbs 1200 joules of heat energy, what is the final temperature of the sample?
• Question #a73fe
• How much heat is given off when 1.25 grams of silver is cooled from 100.0 C to 80.0 C?
• A piece of copper with a mass of 22.6 g initially at a temperature of 16.3 °C is heated to a temperature of 33.1 °C. Assuming the specific heat of copper is 0.386 J/(g°C), how much heat was needed for this temperature change to take place?
• A piece of gold initially at a temperature of 25.1 °C absorbs 675 J of heat, raising its temperature to 57.4 °C. Assuming the specific heat of gold is 0.126 J/(g°C), what is the mass of the sample?
• Calculate the heat required to raise the temperature of 0.75 kg of water from 5˚C to 90.˚C?
• Question #9b580
• Calculate the heat required to raise the temperature of 2.0 kg of ice at -25˚C to 70.˚C?
• What is the final temperature if you place 501 g of copper at 89.5 °C in a calorimeter containing 159 g of water at 22.8 °C?
• Question #4c66a
• Question #4af98
• Question #11e6e
• Question #38eda
• What is an equation that you can use to find the number of Calories in any number of grams of trail mix?
• Question #59f7f
• Question #779cf
• It takes 80 cal/g to change solid water at 0°C to liquid water. How many calories will it take to change 3 g of water at 0 °C to liquid water?
• A calorimeter contains 15 grams of water. The water's temperature increases by 10 C°. How much heat energy was added to the water? (Hint: water's specific heat is 1 cal/g°C)?
• Question #2c289
• Question #7cc47
• Question #7e831
• Question #6ad15
• Question #8b482
• Question #5012c
• If 213 J raises a sample of water 8.2°C, what is the mass of the water?
• How many joules are required for heating 65 g of water from 12 °C to 76 °C?
• Question #ef3fa
• Question #4719e
• How much energy is required to heat a #1*g# block of ice at #-10# #""^@C# to give a #1*g# mass of water at #+10# #""^@C#?
• Question #04da9
• Question #8f2db
• Question #b579a
• Question #e8e78
• Question #42dcd
• Question #05bc9
• A 1,200-watt heater is used for raising the temperature of 1 liter of water to boiling point. How long will it take for the water to boil if the initial temperature of water is 20 C? (1 cal = 4.19 joules?)
• If 335 g of water at 65.5°C loses 9750 J heat, what is the final temperature of the water?
• Question #509d0
• Question #0def0
• Question #0ce58
• Question #8899d
• Question #98fe4
• Question #d8b91
• If 5,100 joules of heat are given off when a sample of water freezes, what Is the mass of the water?
• How many joules of heat are necessary to melt 500 g of ice at its freezing point?
• The combustion of propane (#C_3H_8#) produces 248 of energy per mole of propane burned. How much heat energy will be released when 1 000 L of propane are burned at STP?
• Question #b5482
• Question #f631a
• How much heat would be needed to raise the temperature of 25.0 g of water by 18#"^@#C?
• Question #440b7
• How much heat is required to convert #10g# of ice at #-10^@C# into steam at #100^@C#?
• How much heat energy (Joules) is required to to raise the temperature of 120.0 g of water from -90 C to -5 C?
• Why would heat lost by warmer water not equal the heat gained by the colder water?
• How much heat energy (Joules) is required to raise the temperature of 120.0 g of wate from -90 C to -5 C?
• How many grams of silver are needed to absorb 1.00 kJ of energy changing the temperature from 33.0°C to 41.8°C?
• How many grams of silver are needed to absorb 1.00 kJ of energy changing the temperature 33.0 C to 41.8°C?
• How many joules are in 104 calories? (1 cal = 4.18J)?
• What is the amount of heat required to raise the temperature of 200.0 g of aluminum by 10°C? (Specific heat of aluminum = -0.21 cal/g*#"^@#C)?
• Question #01bc9
• How many kilojoules are required to warm 25.0 g of water from 75.0 C to 100.0 C and convert it to steam at 100.0 C? The heat of vaporization of water is 2260 joules/g, and the the specific heat of water is 4.184 joules/g?
• Question #99f0f
• Question #53c80
• 1. (a) A 300.0 g copper kettle contains 1.000 kg of water at 20.0 °C. How much energy must you supply to heat the kettle + water to 98.6 °C? (b) How much propane must you burn to provide this energy, if the transfer of the heat of combustion is 35 %?
• Question #84a81
• It takes 4.2 joules of energy to raise the temperature of 1 gram of water by 1°C. What heat of water is 4.2 joules/gram C?
• How much heat is required to raise 250.0 g of ice at a temperature -15.0°C to 105.0°C?
• If 980 kJ of energy are added to 6.2 L of water at 291 K, what wil the final temperature of the water be?
• #"6345 J"# of energy are required to raise the temperature of water from #22.6^@"C"# to #45.1^@"C"#. What is the mass of the water?
• How much heat is released when a 10.0 g sample of iron cools from 75.0 C to 25.5 C? The specific heat capacity of iron is 0.449 J/g?
• Question #70bc1
• Question #b9477
• If #"1500 g"# of water was heated by the combustion of #"1 g"# of sucrose to go from #25.0^@ "C"# to #28.3^@ "C"#, what is the enthalpy of combustion in #"kJ/mol"#?
• 150mL of water at 25oC is mixed 325mL of 80oC water in a sealed vacuum insulated vessel. Determine the final temp of the combined 475mL of water. The density of water is 1g/mL. What's the final temperature??
• Question #c0a79
• Question #618a1
• Question #e3249
• Question #91423
• Find the amount of heat energy needed to convert 150 grams of ice at -15°C to ice at -63°C?
• Find the amount of heat energy needed to convert 400 grams of ice at -38°C to steam at 160°C? 1284440 Joules 246840 Joules 331056 Joules 159984 Joules
• How much energy is required to heat a #20*g# mass of ice, to give a #20*g# mass of steam at #120# #""^@C#?
• If 24500 J is applied to 125g of water at 35 C, what will the final temperature of the water be?
• Why does water take so long to heat up or cool down?
• How much energy would it take to heat 10 g of water from 10 to 15 C?
• Question #503c5
• Question #087c4
• How much energy is required to heat #72# #g# of water by #75^o# #C#?
• Question #e71b7
• Is ΔH=mCΔT and q=mCΔT the same thing? If so, which is more scientific?
• Question #db7ad
• Im having trouble understanding what the question is asking?
• How many calories are absorbed when 500 grams of water (1 cal/g c) is heated from 50 to 100 degrees Celsius?
• Use this balanced equation #2C_2H_2 + 5O_2 -> 4CO_2 + 2H2_O + 2599 kJ#. How much energy is needed to produce 42.9 grams of carbon dioxide?
• Question #9a43b
• How many joules are required to increase the temperature of a 30.0 g block of gold from 25.0 ºC to 50.0 ºC? The specific heat of gold is 0.129 J/(g⋅°C) 4.184 J 96.8 J 193.5 J 3138 J
• Question #fb65f
• How do you calculate the amount of heat needed to increase the temperature of 250g of water from 20 C to 56 C? #C_g = 4.8 J/(C-g)#
• Question #897e7
• Question #7d7cc
• Question #b2438
• Question #7be8f
• Question #77db3
• How many calories are required to raise the temperature of a 35.0 g sample of iron from 25°C to 35°C? Iron has a specific heat of 0.108 cal/g°C?
• Question #95b88
• How much heat (in kJ) is released when 1.65 mol NaOH(s) is dissolved in water? (The molar heat of solution of NaOH is -445.1 kJ/mol)
• How much heat is required to heat a #10*g# mass of ice at #-10# #""^@C#, to give a #10*g# mass of water at #+10# #""^@C#?
• Question #926ff
• Question #22d95
• A sample of substance X that has a mass of 326.0 g releases 4325.8 cal when it freezes at its freezing point. If substance X has a molar mass of 58.45 g/mol, what is the molar heat of fusion for substance X?
• A sample of #H_2O# with a mass of 46.0 grams has a temperature of 100 °C. How many joules are necessary to boil the water? (use 2.0934 J/g for the heat of vaporization of water)
• A student conducting a calorimetry investigation determines a negative #DeltaH#. What does the negative value indicate about the reaction?
• The molar heat of fusion for water is 6.01 J/mol. How much energy must be added to a 75.0-g block of ice at 0°C to change it to a 75.0 g of liquid water at 0°C?
• Question #b0ecf
• Question #2afc8
• Suppose you have a #25xx45xx2.5# #"cm"# steel bar whose density is #"7.8 g/cm"^3# at #22^@ "C"#. If #"3.8 kJ"# was imparted into it by solar energy, and the bar's specific heat capacity is #"0.49 J/g"^@ "C"#, to what temperature does it rise?
• Question #816d2
• Question #3d744
• Question #ea8ea
• Question #35c00
• Question #2cc3c
• Question #fae70
• Question #e3133
• If #4.25 xx 10^3# #"g"# of gold was heated from #15.5^@ "C"# to #197.0^@ "C"#, how much heat was involved, and what is the molar enthalpy in #"kJ/mol"#? #C_P = "0.129 J/g"^@ "C"#?
• What is the molar heat of combustion when #"25000 g"# of methanol is combusted in a bomb calorimeter to raise the temperature of the surrounding water by #40^@ "C"# if the heat capacity of the calorimeter is #"10.4 kJ/"^@ "C"#?
• Calcium chloride dissolves in water to form calcium and chloride ions, producing 83kJ of heat per mole. Calculate final temp. when 0.02 moles of calcium chloride is dissolved into 150ml of water at a temperature initially of 19 degrees?
• Question #3269e
• Question #8af18
• If a #25.00g# piece of copper (#C_s = (0.385J)/(g*°C)#) at #115.0°C# is added to #50.00g# of water (#C_s = (4.184J)/(g*°C)#) at #25.00°C#, what is the final temperature once the object and water thermally equilibrate?
• Question #f51b9
• What energy is associated with the complete combustion of a #20*g# mass of ethane?
• Question #34abf
• Question #769b2
• What total amount of heat input is required to heat #"9 g"# of water from a liquid at #92^@ "C"# to steam at #103^@ "C"#?
• Adding nitric acid to water is quite exothermic. What is the temperature change of 100 mL of water (d = 1.00g/mL) at 20.0°C [cp = 75.3 J/(mol·°C)] after adding 10.0 mL of concentrated HNO3(14.0M , ΔH°soln = –33.3 kJ/mol) ?
• Question #48d66
• Question #16f9b
• Question #ca241
• Question #4113d
• What is the heat absorbed by #"27 g"# of water that increases in temperature by #58^@ "C"#? Assume #c = "4.184 J/g"^@ "C"# for water in this temperature range.
• Question #61aa8
• Question #21940
• Chemistry; Calorimetry; Calculating Heat Capacity; Help Please?!
• Question #de7a7
• How much energy is required to convert 429 g of water to steam at 156 °C?
• How do I find the change in temperature of #"199.0 g"# of water that loses #"2793 J"# of heat?
• Question #d1d51
• Question #21fd7
• Question #95ca2
• Question #d2b4f
• Question #da3fc
• Question #54a28
• Question #8f7d4
• A 29.80 g sample of liquid cadmium at 377.00°C is poured into a mold and allowed to cool to 24.00°C. How many kJ of energy are released in this process?
• Question #6033f
• Question #5141e
• How much boiling water would you need to raise the bath to body temperature (about 37 ∘C)? Assume that no heat is transferred to the surrounding environment. Express your answer to two significant figures and include the appropriate units.
• Question #53ce8
• A cube of gold is heated then submerged in water. What is the volume of the cube of gold (in mL)?