Calorimeter - Revision history

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	is kept constant. This time linearity requires good design and good (computerized) temperature control. Of course, controlled cooling and isothermal experiments are also possible.		is kept constant. This time linearity requires good design and good (computerized) temperature control. Of course, controlled cooling and isothermal experiments are also possible.

	Heat flows into the two pans by conduction. The flow of heat into the sample is larger because of its heat capacity ''C<sub>p</sub>''. The difference in flow ''dq''/''dt'' induces a small temperature difference Δ''T'' across the slab. This temperature difference is measured using a thermocouple.<ref name="~~CCRConPresCalor~~">{{cite book \|url=http://books.google.com/books?id=tRt-Z5Duz7QC&pg=PA1 \|title=Differential Scanning Calorimetry \|author=Höhne, Günther; Hemminger, W.F.; Flammersheim, H.J. \|publisher=Springer \|year=2003 \|page=1–7 \|isbn=354000467X \|accessdate=11 May 2013}}</ref> The heat capacity can in principle be determined from this signal:		Heat flows into the two pans by conduction. The flow of heat into the sample is larger because of its heat capacity ''C<sub>p</sub>''. The difference in flow ''dq''/''dt'' induces a small temperature difference Δ''T'' across the slab. This temperature difference is measured using a thermocouple.<ref name="HöhneDiff03">{{cite book \|url=http://books.google.com/books?id=tRt-Z5Duz7QC&pg=PA1 \|title=Differential Scanning Calorimetry \|author=Höhne, Günther; Hemminger, W.F.; Flammersheim, H.J. \|publisher=Springer \|year=2003 \|page=1–7 \|isbn=354000467X \|accessdate=11 May 2013}}</ref> The heat capacity can in principle be determined from this signal:

	<math>\Delta T = K {dq\over dt} = K C_p\, \beta</math>		<math>\Delta T = K {dq\over dt} = K C_p\, \beta</math>

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	<references />		<references />

			<!---Place all category tags here-->
	[[Category:Laboratory equipment]]		[[Category:Laboratory equipment]]

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	The technique is gaining in importance, particularly in the field of biochemistry, because it facilitates determination of substrate binding to enzymes. The technique is commonly used in the pharmaceutical industry to characterize potential drug candidates.<ref name="PLIIso">{{cite book \|url=http://books.google.com/books?id=0Jqe2I5SwbkC&pg=PA32 \|title=Peptide-Lipid Interactions \|author=Simon, Sidney A.; McIntosh, Thomas J. \|publisher=Academic Press \|year=2002 \|page=32–33 \|isbn=0080925855 \|accessdate=11 May 2013}}</ref>		The technique is gaining in importance, particularly in the field of biochemistry, because it facilitates determination of substrate binding to enzymes. The technique is commonly used in the pharmaceutical industry to characterize potential drug candidates.<ref name="PLIIso">{{cite book \|url=http://books.google.com/books?id=0Jqe2I5SwbkC&pg=PA32 \|title=Peptide-Lipid Interactions \|author=Simon, Sidney A.; McIntosh, Thomas J. \|publisher=Academic Press \|year=2002 \|page=32–33 \|isbn=0080925855 \|accessdate=11 May 2013}}</ref>

	~~==See also==~~
	~~{{commons category\|Calorimeters}}~~
	~~[[Differential scanning calorimetry]]~~

	==References==		==References==

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	[[Image:Ice-calorimeter.jpg\|150px\|right\|thumb\|The world’s first '''ice-calorimeter''', used in the winter of 1782-83, by Antoine Lavoisier and Pierre-Simon Laplace, to determine the heat evolved in various chemical changes; calculations which were based on Joseph Black's prior discovery of latent heat. These experiments mark the foundation of [[thermochemistry]].]]		[[Image:Ice-calorimeter.jpg\|150px\|right\|thumb\|The world’s first '''ice-calorimeter''', used in the winter of 1782-83, by Antoine Lavoisier and Pierre-Simon Laplace, to determine the heat evolved in various chemical changes; calculations which were based on Joseph Black's prior discovery of latent heat. These experiments mark the foundation of [[thermochemistry]].]]
	A '''calorimeter''' (from Latin ''calor'', meaning heat) is an object used for [[calorimetry]], or the process of measuring the heat of chemical reactions or physical changes as well as heat capacity. ~~Differential scanning calorimeters~~, ~~isothermal microcalorimeters~~, ~~titration calorimeters and accelerated rate calorimeters are among the most common types~~. A simple calorimeter just consists of a thermometer attached to a metal container full of water suspended above a combustion chamber.		A '''calorimeter''' (from Latin ''calor'', meaning heat) is an object used for [[calorimetry]], or the process of measuring the heat of chemical reactions or physical changes as well as heat capacity. More specifically, a calorimeter handles the [[enthalpy]] changes of chemical reactions by thermally isolating the reaction system from its surroundings.<ref name="AdvChemCalo">{{cite book \|url=http://books.google.com/books?id=qciCdSFpFPkC&pg=PA149 \|title=Advanced Chemistry \|author=Clugston, Michael J.; Flemming, Rosalind \|publisher=Oxford University Press \|year=2000 \|page=148 \|isbn=0199146330}}</ref> A simple calorimeter just consists of a thermometer attached to a metal container full of water suspended above a combustion chamber and is sometimes referred to as a "coffee cup" calorimeter, whereas more sophisticated forms like "flame" and "bomb" calorimeters involve combustion of the substance in a burner or pressurized vessel.

	To find the enthalpy change per mole of a substance A in a reaction between two substances A and B, the substances are added to a calorimeter and the initial and final temperatures (before the reaction started and after it has finished) are noted. Multiplying the temperature change by the mass and specific heat capacities of the substances gives a value for the energy given off or absorbed during the reaction. Dividing the energy change by how many moles of A were present gives its enthalpy change of reaction. This method is used primarily in academic teaching as it describes the theory of calorimetry. It does not account for the heat loss through the container or the heat capacity of the thermometer and container itself. In addition, the object placed inside the calorimeter shows that the objects transferred their heat to the calorimeter and into the liquid, and the heat absorbed by the calorimeter and the liquid is equal to the heat given off by the metals.		To find the enthalpy change per mole of a substance A in a reaction between two substances A and B, the substances are added to a calorimeter and the initial and final temperatures (before the reaction started and after it has finished) are noted. Multiplying the temperature change by the mass and specific heat capacities of the substances gives a value for the energy given off or absorbed during the reaction. Dividing the energy change by how many moles of A were present gives its enthalpy change of reaction. This method is used primarily in academic teaching as it describes the theory of calorimetry.<ref name="AdvChemCalo" /> It does not account for the heat loss through the container or the heat capacity of the thermometer and container itself. In addition, the object placed inside the calorimeter shows that the objects transferred their heat to the calorimeter and into the liquid, and the heat absorbed by the calorimeter and the liquid is equal to the heat given off by the metals.<ref name="ChemPrinCalo">{{cite book \|url=http://books.google.com/books?id=2OxrDtDaSqIC&pg=PA378 \|title=Chemical Principles \|author=Zumdahl, Steven S. \|publisher=Cengage Learning \|year=2009 \|page=378–87 \|isbn=061894690X}}</ref>

	==History==		==History==
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	==Adiabatic calorimeters==		==Adiabatic calorimeters==
	An adiabatic calorimeter is a calorimeter used to examine a runaway reaction. Since the calorimeter runs in an adiabatic environment, any heat generated by the material sample under test causes the sample to increase in temperature, thus fueling the reaction.		An adiabatic calorimeter is a calorimeter used to examine a runaway reaction. Since the calorimeter runs in an adiabatic environment, any heat generated by the material sample under test causes the sample to increase in temperature, thus fueling the reaction.

	No adiabatic calorimeter is adiabatic — some heat will be lost by the sample to the sample holder. A mathematical correction factor, known as the phi-factor, can be used to adjust the calorimetric result to account for these heat losses. The phi-factor is the ratio of the thermal mass of the sample and sample holder to the thermal mass of the sample alone.		No adiabatic calorimeter is adiabatic — some heat will be lost by the sample to the sample holder. A mathematical correction factor, known as the phi-factor, can be used to adjust the calorimetric result to account for these heat losses. The phi-factor is the ratio of the thermal mass of the sample and sample holder to the thermal mass of the sample alone.<ref name="SHMMM83">{{cite book \|url=http://books.google.com/books?id=8lANaR-Pqi4C&pg=PA410 \|title=Springer Handbook of Materials Measurement Methods \|editor=Czichos, Horst ; Saito, Tetsuya; Smith, Leslie R. \|publisher=Springer \|year=2006 \|page=410–414 \|isbn=3540303006 \|accessdate=08 May 2013}}</ref>

	==Reaction calorimeters==		==Reaction calorimeters==

	~~{{Main\|Reaction calorimeters}}~~		A reaction calorimeter is a calorimeter in which a chemical reaction is initiated within a closed insulated container. Reaction heats are measured and the total heat is obtained by integrating heat flow versus time. This is the standard used in industry to measure heats since industrial processes are engineered to run at constant temperatures. Reaction calorimetry can also be used to determine maximum heat release rate for chemical process engineering and for tracking the global kinetics of reactions.<ref name="IORCalor">{{cite book \|url=http://books.google.com/books?id=NgV9yqD-sOYC&pg=PA200 \|title=The Investigation of Organic Reactions and Their Mechanisms \|editor=Maskill, Howard \|publisher=John Wiley & Sons \|year=2008 \|page=200–202 \|isbn=0470994169 \|accessdate=08 May 2013}}</ref> There are four main methods for measuring the heat in reaction calorimeter:
	A reaction calorimeter is a calorimeter in which a chemical reaction is initiated within a closed insulated container. Reaction heats are measured and the total heat is obtained by integrating heat flow versus time. This is the standard used in industry to measure heats since industrial processes are engineered to run at constant temperatures. Reaction calorimetry can also be used to determine maximum heat release rate for chemical process engineering and for tracking the global kinetics of reactions. There are four main methods for measuring the heat in reaction calorimeter:

	===Heat flow calorimetry===		===Heat flow calorimetry===

	The cooling/heating jacket controls either the temperature of the process or the temperature of the jacket. Heat is measured by monitoring the temperature difference between heat transfer fluid and the process fluid. In addition fill volumes (i.e. wetted area), specific heat, heat transfer coefficient have to be determined to arrive at a correct value. It is possible with this type of calorimeter to do reactions at reflux, although the accuracy is not as good.		The cooling/heating jacket controls either the temperature of the process or the temperature of the jacket. Heat is measured by monitoring the temperature difference between heat transfer fluid and the process fluid. In addition fill volumes (i.e. wetted area), specific heat, heat transfer coefficient have to be determined to arrive at a correct value. It is possible with this type of calorimeter to do reactions at reflux, although the accuracy is not as good.<ref name="IORCalor" />

	===Heat balance calorimeter===		===Heat balance calorimeter===

	The cooling/heating jacket controls the temperature of the process. Heat is measured by monitoring the heat gained or lost by the heat transfer fluid.		The cooling/heating jacket controls the temperature of the process. Heat is measured by monitoring the heat gained or lost by the heat transfer fluid.<ref name="IORCalor" />

	===Power compensation===		===Power compensation===
	Power compensation uses a heater placed within the vessel to maintain a constant temperature. The energy supplied to this heater can be varied as reactions require and the calorimetry signal is purely derived from this electrical power.		Power compensation uses a heater placed within the vessel to maintain a constant temperature. The energy supplied to this heater can be varied as reactions require and the calorimetry signal is purely derived from this electrical power.<ref name="IORCalor" />

	===Constant flux===		===Constant flux===
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	[[File:Bomb Calorimeter.png\|thumb\|Bomb calorimeter]]		[[File:Bomb Calorimeter.png\|thumb\|Bomb calorimeter]]

	A bomb calorimeter is a type of constant-volume calorimeter used in measuring the heat of combustion of a particular reaction. Bomb calorimeters have to withstand the large pressure within the calorimeter as the reaction is being measured. Electrical energy is used to ignite the fuel; as the fuel is burning, it will heat up the surrounding air, which expands and escapes through a tube that leads the air out of the calorimeter. When the air is escaping through the copper tube it will also heat up the water outside the tube. The temperature of the water allows for calculating calorie content of the fuel.		A bomb calorimeter is a type of constant-volume calorimeter used in measuring the heat of combustion of a particular reaction. Bomb calorimeters have to withstand the large pressure within the calorimeter as the reaction is being measured. Electrical energy is used to ignite the fuel; as the fuel is burning, it will heat up the surrounding air, which expands and escapes through a tube that leads the air out of the calorimeter. When the air is escaping through the copper tube it will also heat up the water outside the tube. The temperature of the water allows for calculating calorie content of the fuel.<ref name="SHMMM83" /><ref name="AdvChemCalo" />

	In more recent calorimeter designs, the whole bomb, pressurized with excess pure oxygen (typically at 30atm) and containing a weighed mass of a sample (typically 1-1.5 g) and a small fixed amount of water (to saturate the internal atmosphere, thus ensuring that all water produced is liquid, and removing the need to include enthalpy of vaporization in calculations), is submerged under a known volume of water (ca. 2000 ml) before the charge is electrically ignited. The bomb, with the known mass of the sample and oxygen, form a closed system - no gases escape during the reaction. The weighted reactant put inside the steel container is then ignited. Energy is released by the combustion and heat flow from this crosses the stainless steel wall, thus raising the temperature of the steel bomb, its contents, and the surrounding water jacket. The temperature change in the water is then accurately measured with a thermometer. This reading, along with a bomb factor (which is dependent on the heat capacity of the metal bomb parts), is used to calculate the energy given out by the sample burn. A small correction is made to account for the electrical energy input, the burning fuse, and acid production (by titration of the residual liquid). After the temperature rise has been measured, the excess pressure in the bomb is released.		In more recent calorimeter designs, the whole bomb, pressurized with excess pure oxygen (typically at 30atm) and containing a weighed mass of a sample (typically 1-1.5 g) and a small fixed amount of water (to saturate the internal atmosphere, thus ensuring that all water produced is liquid, and removing the need to include enthalpy of vaporization in calculations), is submerged under a known volume of water (ca. 2000 ml) before the charge is electrically ignited. The bomb, with the known mass of the sample and oxygen, form a closed system - no gases escape during the reaction. The weighted reactant put inside the steel container is then ignited. Energy is released by the combustion and heat flow from this crosses the stainless steel wall, thus raising the temperature of the steel bomb, its contents, and the surrounding water jacket. The temperature change in the water is then accurately measured with a thermometer. This reading, along with a bomb factor (which is dependent on the heat capacity of the metal bomb parts), is used to calculate the energy given out by the sample burn. A small correction is made to account for the electrical energy input, the burning fuse, and acid production (by titration of the residual liquid). After the temperature rise has been measured, the excess pressure in the bomb is released.
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	==Calvet-type calorimeters==		==Calvet-type calorimeters==

	The detection is based on a three-dimensional fluxmeter sensor. The fluxmeter element consists of a ring of several thermocouples in series. The corresponding thermopile of high thermal conductivity surrounds the experimental space within the calorimetric block. The radial arrangement of the thermopiles guarantees an almost complete integration of the heat. This is verified by the calculation of the efficiency ratio that indicates that an average value of 94% +/- 1% of heat is transmitted through the sensor on the full range of temperature of the Calvet-type calorimeter. In this setup, the sensitivity of the calorimeter is not affected by the crucible, the type of purge gas, or the flow rate. The main advantage of the setup is the increase of the experimental vessel's size and consequently the size of the sample, without affecting the accuracy of the calorimetric measurement.		The detection is based on a three-dimensional fluxmeter sensor. The fluxmeter element consists of a ring of several thermocouples in series. The corresponding thermopile of high thermal conductivity surrounds the experimental space within the calorimetric block. The radial arrangement of the thermopiles guarantees an almost complete integration of the heat. This is verified by the calculation of the efficiency ratio that indicates that an average value of 94% +/- 1% of heat is transmitted through the sensor on the full range of temperature of the Calvet-type calorimeter. In this setup, the sensitivity of the calorimeter is not affected by the crucible, the type of purge gas, or the flow rate. The main advantage of the setup is the increase of the experimental vessel's size and consequently the size of the sample, without affecting the accuracy of the calorimetric measurement.<ref name="HTACCalor">{{cite book \|url=http://books.google.com/books?id=33_3DBLGzMYC&pg=PR619 \|title=Handbook of Thermal Analysis and Calorimetry: Principles and Practice \|editor=Brown, Michael E. \|publisher=Elsevier \|year=1998 \|page=619–629 \|isbn=0080539599 \|accessdate=08 May 2013}}</ref>

	The calibration of the calorimetric detectors is a key parameter and has to be performed very carefully. For Calvet-type calorimeters, a specific calibration, so called Joule effect or electrical calibration, has been developed to overcome all the problems encountered by a calibration done with standard materials.		The calibration of the calorimetric detectors is a key parameter and has to be performed very carefully. For Calvet-type calorimeters, a specific calibration, so called Joule effect or electrical calibration, has been developed to overcome all the problems encountered by a calibration done with standard materials.

	The main advantages of this type of calibration are as follows:		The main advantages of this type of calibration are as follows:
	*It is an absolute calibration.		*It is an absolute calibration.

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	<span class="plainlinks">[http://en.wikipedia.org/wiki/Biochemistry?title=Biochemistry biochemistry]</span>, because it facilitates determination of substrate binding to		<span class="plainlinks">[http://en.wikipedia.org/wiki/Biochemistry?title=Biochemistry biochemistry]</span>, because it facilitates determination of substrate binding to
	<span class="plainlinks">[http://en.wikipedia.org/wiki/Enzyme?title=Enzyme enzyme]</span>s. The technique is commonly used in the pharmaceutical industry to characterize potential drug candidates.		<span class="plainlinks">[http://en.wikipedia.org/wiki/Enzyme?title=Enzyme enzyme]</span>s. The technique is commonly used in the pharmaceutical industry to characterize potential drug candidates.

			==Calorimeter vendors==
			See the [[Calorimeter vendor]] page for a list of LIMS vendors past and present.

	==See also==		==See also==
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	==References==		==References==
	~~<span class="plainlinks">~~[http://en.wikipedia.org/wiki/Calorimeter~~?title=WikipediaCalorimeter~~ Wikipedia]~~</span>~~		[http://en.wikipedia.org/wiki/Calorimeter Wikipedia]


	[[Category:Analytical]]		[[Category:Analytical]]

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	where		where

	:Cp = Specific heat at constant pressure		:Cp = Specific heat at constant pressure
	:\Delta H = Enthalpy of solution		:\Delta H = Enthalpy of solution
	:\Delta T = Change in temperature		:\Delta T = Change in temperature
	:W = mass of solute		:W = mass of solute
	:M = molecular mass of solute		:M = molecular mass of solute

	==Differential scanning calorimeter==		==Differential scanning calorimeter==
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	When suddenly heat is absorbed by the sample (e.g., when the sample melts), the signal will respond and exhibit a peak.		When suddenly heat is absorbed by the sample (e.g., when the sample melts), the signal will respond and exhibit a peak.

	~~<math>~~{dq\over dt} = C_p \beta + f(t,T)~~</math>~~		{dq\over dt} = C_p \beta + f(t,T)

	From the		From the

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			== Headline text ==
	''This article is about heat measuring devices. For particle detectors, see'' <span class="plainlinks">[http://en.wikipedia.org/wiki/Calorimeter_(particle_physics)?title=Calorimeter Calorimeter (particle physics)]</span>		''This article is about heat measuring devices. For particle detectors, see'' <span class="plainlinks">[http://en.wikipedia.org/wiki/Calorimeter_(particle_physics)?title=Calorimeter Calorimeter (particle physics)]</span>

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	<span class="plainlinks">[http://en.wikipedia.org/wiki/Styrofoam?title=Styrofoam Styrofoam]</span> cups having holes through which a		<span class="plainlinks">[http://en.wikipedia.org/wiki/Styrofoam?title=Styrofoam Styrofoam]</span> cups having holes through which a
	<span class="plainlinks">[http://en.wikipedia.org/wiki/Thermometer?title=Thermometer thermometer]</span> and a stirring rod can be inserted. The inner cup holds the solution in which of the reaction occurs, and the outer cup provides		<span class="plainlinks">[http://en.wikipedia.org/wiki/Thermometer?title=Thermometer thermometer]</span> and a stirring rod can be inserted. The inner cup holds the solution in which of the reaction occurs, and the outer cup provides
	<span class="plainlinks">[http://en.wikipedia.org/wiki/Thermal_insulation?title=Insulation insulation]</span>. ~~Then~~		<span class="plainlinks">[http://en.wikipedia.org/wiki/Thermal_insulation?title=Insulation insulation]</span>.

	~~<math>~~Cp = \frac {W\Delta H}{M\Delta T}~~</math>~~		Then Cp = \frac {W\Delta H}{M\Delta T}

	where		where

	:~~<math>~~Cp~~</math>~~ = Specific heat at constant pressure		:Cp = Specific heat at constant pressure
	:~~<math>~~\Delta H~~</math>~~ = Enthalpy of solution		:\Delta H = Enthalpy of solution
	:~~<math>~~\Delta T~~</math>~~ = Change in temperature		:\Delta T = Change in temperature
	:~~<math>~~W~~</math>~~ = mass of solute		:W = mass of solute
	:~~<math>~~M~~</math>~~ = molecular mass of solute		:M = molecular mass of solute

	==Differential scanning calorimeter==		==Differential scanning calorimeter==
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	<span class="plainlinks">[http://en.wikipedia.org/wiki/Thermocouple?title=Thermocouple thermocouple]</span>. The heat capacity can in principle be determined from this signal:		<span class="plainlinks">[http://en.wikipedia.org/wiki/Thermocouple?title=Thermocouple thermocouple]</span>. The heat capacity can in principle be determined from this signal:

	~~<math>\~~Delta T = K {dq\over dt} = K C_p\, \beta~~</math>~~		Delta T = K {dq\over dt} = K C_p\, \beta

	Note that this formula (equivalent to		Note that this formula (equivalent to
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	When suddenly heat is absorbed by the sample (e.g., when the sample melts), the signal will respond and exhibit a peak.		When suddenly heat is absorbed by the sample (e.g., when the sample melts), the signal will respond and exhibit a peak.

	<math>{dq\over dt} = C_p \beta + f(t,T) </math>		<math>{dq\over dt} = C_p \beta + f(t,T)</math>

	From the		From the

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	==Isothermal titration calorimeter==<!-- This section is linked from [[Titration]] -->		==Isothermal titration calorimeter==<!-- This section is linked from [[Titration]] -->
	''Main article:''<span class="plainlinks">[http://en.wikipedia.org/wiki/Isothermal_Titration_Calorimetry?title=ISC Isothermal Titration Calorimetry]</span>		''Main article:''<span class="plainlinks">[http://en.wikipedia.org/wiki/Isothermal_Titration_Calorimetry?title=ISC Isothermal Titration Calorimetry]</span>
	In an '''isothermal		In an '''isothermal.

	<span class="plainlinks">[http://en.wikipedia.org/wiki/Titration?title=Titration titration]</span> calorimeter''', the heat of reaction is used to follow a titration experiment. This permits determination of the mid point (		<span class="plainlinks">[http://en.wikipedia.org/wiki/Titration?title=Titration titration]</span> calorimeter''', the heat of reaction is used to follow a titration experiment. This permits determination of the mid point (
	<span class="plainlinks">[http://en.wikipedia.org/wiki/Stoichiometry?title=Stoichiometry stoichiometry]</span>) (N) of a reaction as well as its enthalpy (delta H), entropy (delta S) and of primary concern the binding affinity (Ka)		<span class="plainlinks">[http://en.wikipedia.org/wiki/Stoichiometry?title=Stoichiometry stoichiometry]</span>) (N) of a reaction as well as its enthalpy (delta H), entropy (delta S) and of primary concern the binding affinity (Ka)
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	==See also==		==See also==
	~~{{commons category\|Calorimeters}}~~
	*<span class="plainlinks">[http://en.wikipedia.org/wiki/Enthalpy?title=Enthalpy Enthalpy]</span>		*<span class="plainlinks">[http://en.wikipedia.org/wiki/Enthalpy?title=Enthalpy Enthalpy]</span>
	*<span class="plainlinks">[http://en.wikipedia.org/wiki/Heat?title=Heat Heat]</span>		*<span class="plainlinks">[http://en.wikipedia.org/wiki/Heat?title=Heat Heat]</span>
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	<span class="plainlinks">[http://en.wikipedia.org/wiki/Calorimeter?title=WikipediaCalorimeter Wikipedia]</span>		<span class="plainlinks">[http://en.wikipedia.org/wiki/Calorimeter?title=WikipediaCalorimeter Wikipedia]</span>


	~~{{Laboratory equipment}}~~

	~~[[Category:Measuring instruments]]~~
	~~[[Category:Laboratory equipment]]~~

	~~[[ar:مسعر]]~~
	~~[[be-x-old:Калярымэтры]]~~
	~~[[bg:Калориметър]]~~
	~~[[ca:Calorímetre]]~~
	~~[[cs:Kalorimetr]]~~
	~~[[da:Kalorimeter]]~~
	~~[[de:Kalorimeter]]~~
	~~[[es:Calorímetro]]~~
	~~[[fr:Calorimètre]]~~
	~~[[hi:कैलोरीमीटर]]~~
	~~[[io:Kalorimetro]]~~
	~~[[id:Kalorimeter]]~~
	~~[[it:Calorimetro]]~~
	~~[[he:קלורימטר]]~~
	~~[[ht:Kalorimèt]]~~
	~~[[nl:Calorimeter]]~~
	~~[[ja:熱#熱量計]]~~
	~~[[pl:Kalorymetr]]~~
	~~[[pt:Calorímetro]]~~
	~~[[ru:Калориметр]]~~
	~~[[simple:Calorimeter]]~~
	~~[[sk:Kalorimeter]]~~
	~~[[sl:Kalorimeter]]~~
	~~[[sr:Kalorimetar]]~~
	~~[[fi:Kalorimetri]]~~
	~~[[sv:Kalorimeter]]~~
	~~[[th:แคลอรีมิเตอร์]]~~
	~~[[tr:Kalorimetre]]~~
	~~[[uk:Калориметр]]~~

	[[Category:Analytical]]		[[Category:Analytical]]