Heat Capacity

The warm capacity actions the amount of heat crucial to progressive the temperature of things or system by one degree Celsius.

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Key Takeaways

Key PointsHeat capacity is the measurable physical amount that characterizes the lot of heat forced to readjust a substance’s temperature by a given amount. That is measure up in joules every Kelvin and given by.The warm capacity is comprehensive property, scaling with the size of the system.The heat capacity of many systems is not constant (though it can often be treated together such). It depends on the temperature, pressure, and volume that the mechanism under consideration.Key Termsheat capacity: The amount of heat power needed come raise the temperature of things or unit of issue by one level Celsius; in systems of joules per kelvin (J/K).enthalpy: the total amount of power in a system, consisting of both the inner energy and also the power needed come displace that environment

Heat Capacity

Heat volume (usually denoted by a resources C, often with subscripts), or heat capacity, is the measurable physical amount that characterizes the lot of heat compelled to adjust a substance’s temperature by a given amount. In SI units, warm capacity is express in systems of joules per kelvin (J/K).

An object’s warm capacity (symbol C) is defined as the proportion of the lot of heat energy transferred to things to the resulting boost in temperature of the object.

\displaystyle\textC=\frac\textQ \Delta \textT.

Heat capacity is substantial property, so the scales with the dimension of the system. A sample containing double the quantity of problem as another sample requires the move of twice as much warmth (Q) to achieve the same adjust in temperature (ΔT). Because that example, if that takes 1,000 J to warmth a block the iron, it would certainly take 2,000 J to heat a second block of iron with twice the mass as the first.

The measurement of warm Capacity

The heat capacity of many systems is no a constant. Rather, it counts on the state variables that the thermodynamic system under study. In particular, the is dependency on temperature itself, and on the pressure and the volume of the system, and the ways in i beg your pardon pressures and volumes have actually been enabled to change while the system has actually passed from one temperature come another. The reason for this is the pressure-volume occupational done come the device raises the temperature by a system other than heating, when pressure-volume job-related done by the system absorbs warmth without raising the system’s temperature. (The temperature dependency is why the an interpretation a calorie is official the power needed to warm 1 g that water from 14.5 come 15.5 °C rather of normally by 1 °C. )

Different measurements of heat capacity can thus be performed, most generally at constant pressure and consistent volume. The values hence measured room usually subscripted (by p and V, respectively) to indicate the definition. Gases and liquids room typically likewise measured at constant volume. Dimensions under constant pressure create larger values than those at consistent volume because the consistent pressure values likewise include heat power that is offered to do job-related to expand the substance versus the continuous pressure as its temperature increases. This difference is specifically notable in gases where values under continuous pressure are commonly 30% to 66.7% higher than those at consistent volume.

Thermodynamic connections and meaning of heat Capacity

The internal power of a close up door system alters either by adding heat come the mechanism or through the device performing work. Recalling the very first law that thermodynamics,

\textdU=\delta \textQ-\delta \textW.

For job-related as a an outcome of an increase of the mechanism volume we might write,

\textdU=\delta \textQ-\textPdV.

If the heat is included at continuous volume, climate the 2nd term the this relationship vanishes and one conveniently obtains

\displaystyle\left( \frac\partial \textU\partial \textT\right) _\textV=\left( \frac\partial \textQ\partial \textT\right) _\textV=\textC_\textV.

This defines the heat volume at consistent volume, CV. An additional useful quantity is the heat capacity at consistent pressure, CP. V the enthalpy that the system provided by


our equation for dU transforms to

\textdH=\delta \textQ+\textVdP,

and therefore, at continuous pressure, us have

(\frac\partial \textH\partial \textT)_\textP=(\frac\partial \textQ\partial \textT)_\textP=\textC_\textP.

Specific Heat

The specific heat is an extensive property that explains how much heat must be included to a certain substance come raise its temperature.

Learning Objectives

Summarize the quantitative relationship in between heat transfer and also temperature change

Key Takeaways

Key PointsUnlike the complete heat capacity, the details heat volume is independent of mass or volume. It explains how much heat must be included to a unit of mass of a provided substance to raise that temperature by one degree Celsius. The units of details heat capacity room J/(kg °C) or equivalently J/(kg K).The warm capacity and the particular heat are related by C=cm or c=C/m.The fixed m, details heat c, readjust in temperature ΔT, and also heat included (or subtracted) Q are connected by the equation: Q=mcΔT.Values of particular heat room dependent top top the properties and phase that a offered substance. Due to the fact that they cannot be calculate easily, they room empirically measure up and obtainable for recommendation in tables.Key Termsspecific heat capacity: The quantity of warm that must be included (or removed) from a unit mass of a substance to change its temperature by one level Celsius. That is an intensive property.

Specific Heat

The warmth capacity is comprehensive property that describes how lot heat energy it takes come raise the temperature that a provided system. However, it would be quite inconvenient to measure up the warmth capacity the every unit that matter. What we desire is an intensive property that depends only on the kind and step of a substance and also can be applied to systems of arbitrarily size. This quantity is well-known as the particular heat capacity (or simply, the details heat), i beg your pardon is the warm capacity every unit massive of a material. Experiments show that the transferred warmth depends on three factors: (1) The change in temperature, (2) the massive of the system, and also (3) the substance and also phase that the substance. The last two determinants are encapsulated in the value of the specific heat.

Heat carry and specific Heat Capacity: The heat Q moved to reason a temperature adjust depends top top the magnitude of the temperature change, the mass of the system, and also the substance and also phase involved. (a) The quantity of heat transferred is directly proportional to the temperature change. To twin the temperature change of a mass m, you need to add twice the heat. (b) The lot of warm transferred is likewise directly proportional to the mass. To cause an tantamount temperature change in a double mass, you need to add twice the heat. (c) The amount of heat transferred counts on the substance and also its phase. If it takes an lot Q of heat to reason a temperature readjust ΔT in a provided mass of copper, it will take 10.8 times the amount of warm to reason the identical temperature change in the same mass of water presume no phase adjust in either substance.

The dependency on temperature readjust and massive are easily understood. Due to the fact that the (average) kinetic energy of an atom or molecule is proportional to the absolute temperature, the internal power of a device is proportional to the pure temperature and the variety of atoms or molecules. Due to the fact that the transferred warmth is same to the adjust in the inner energy, the warmth is proportional come the massive of the substance and the temperature change. The moved heat likewise depends on the problem so that, for example, the heat crucial to progressive the temperature is less for alcohol than for water. For the very same substance, the moved heat likewise depends on the step (gas, liquid, or solid).

The quantitative relationship in between heat transfer and also temperature readjust contains all 3 factors:

\textQ=\textmc\Delta \textT,

where Q is the price for warm transfer, m is the mass of the substance, and also ΔT is the adjust in temperature. The prize c stand for specific heat and also depends ~ above the material and also phase.

The certain heat is the lot of heat vital to adjust the temperature of 1.00 kg of massive by 1.00ºC. The certain heat c is a residential or commercial property of the substance; that is SI unit is J/(kg⋅K) or J/(kg⋅C). Recall that the temperature change (ΔT) is the very same in units of kelvin and degrees Celsius. Note that the full heat capacity C is simply the product the the specific heat capacity c and also the fixed of the problem m, i.e.,

\textC=\textmc or \textc=\frac\textC\textm=\frac\textC\rho \textV,

where ϱ is the density of the substance and also V is that is volume.

Values of certain heat must normally be looked increase in tables, since there is no simple method to calculate them. Instead, they are measured empirically. In general, the specific heat likewise depends ~ above the temperature. The table listed below lists representative worths of certain heat for miscellaneous substances. Except for gases, the temperature and also volume dependence of the particular heat of most substances is weak. The particular heat of water is five times the of glass and ten times the of iron, which means that the takes five times together much warmth to progressive the temperature the water the exact same amount together for glass and also ten times together much warmth to progressive the temperature of water together for iron. In fact, water has one the the largest certain heats of any material, i beg your pardon is important for sustaining life on Earth.

Specific Heats: noted are the certain heats of assorted substances. These values are similar in devices of cal/(g⋅C).3. Cv at constant volume and also at 20.0ºC, other than as noted, and also at 1.00 atm mean pressure. Values in parentheses space cp in ~ a continuous pressure the 1.00 atm.

Key Takeaways

Key PointsA calorimeter is offered to measure the heat created (or absorbed) by a physical adjust or chemistry reaction. The scientific research of measuring these changes is known as calorimetry.In stimulate to do calorimetry, the is an essential to know the particular heats that the substances being measured.Calorimetry have the right to be perform under continuous volume or constant pressure. The kind of calculation done counts on the problems of the experiment.Key Termsconstant-pressure calorimeter: an instrument offered to measure the heat created during changes that perform not involve changes in pressure.calorimeter: an apparatus for measuring the heat created or took in by one of two people a chemical reaction, change of step or some various other physical change.constant-volume calorimeter: one instrument supplied to measure the heat produced during changes that perform not involve changes in volume.



Calorimetry is the scientific research of measuring the heat of chemical reactions or physics changes. Calorimetry is performed with a calorimeter. A straightforward calorimeter just is composed of a thermometer attached to a metal container complete of water suspended above a combustion chamber. Words calorimetry is derived from the Latin word calor, meaning heat. Scottish physician and also scientist Joseph Black, who was the an initial to identify the distinction between heat and also temperature, is said to it is in the founder of calorimetry.

Calorimetry calls for that the material being heated have known thermal properties, i.e. Details heat capacities. The timeless rule, known by Clausius and also by Kelvin, is the the press exerted by the calorimetric material is totally and rapidly established solely by its temperature and volume; this ascendancy is for transforms that do not involve phase change, such as melting the ice. There are numerous materials that execute not comply through this rule, and also for them, more complex equations are required than those below.

Ice Calorimeter: The world’s very first ice-calorimeter, used in the winter the 1782-83, through Antoine Lavoisier and Pierre-Simon Laplace, to identify the heat progressed in variouschemical changes; calculations i beg your pardon were based on Joseph Black’s prior discovery of implicit heat. This experiments mark the structure of thermochemistry.

Basic Calorimetry at constant Value

Constant-volume calorimetry is calorimetry performed in ~ a continuous volume. This entails the use of a constant-volume calorimeter (one type is dubbed a Bomb calorimeter). Because that constant-volume calorimetry:

\delta \textQ=\textC_\textV\Delta \textT=\textmc_\textV\Delta \textT

where δQ is the increment that heat got by the sample, CV is the warmth capacity at consistent volume, cv is the specific heat at continuous volume, and ΔT is the adjust in temperature.

Measuring Enthalpy Change

To find the enthalpy change per fixed (or every mole) that a substance A in a reaction between two building materials A and also B, the building material are added to a calorimeter and the initial and also final temperatures (before the reaction started and also after it has actually finished) space noted. Multiply the temperature adjust by the massive and particular heat capacities that the substances provides a value for the energy given off or soaked up during the reaction:

\delta \textQ=\Delta \textT(\textm_\textA\textc_\textA+\textm_\textB\textc_\textB)

Dividing the energy readjust by how numerous grams (or moles) of A were present gives that enthalpy readjust of reaction. This an approach is used primarily in scholastic teaching together it defines the concept of calorimetry. That does not account for the warmth loss through the container or the heat capacity that the thermometer and container itself. In addition, the object put inside the calorimeter reflects that the objects transferred their warmth to the calorimeter and into the liquid, and the heat soaked up by the calorimeter and also the liquid is same to the heat offered off by the metals.

Constant-Pressure Calorimetry

A constant-pressure calorimeter procedures the adjust in enthalpy of a reaction arising in solution during which the atmospheric push remains constant. An example is a coffee-cup calorimeter, which is built from 2 nested Styrofoam cups and also a lid with two holes, permitting insertion of a thermometer and a stirring rod. The within cup stop a known amount the a solute, typically water, that absorbs the warm from the reaction. When the reaction occurs, the external cup provides insulation. Then

\textC_\textP=\frac\textW\Delta \textH\textM\Delta \textT

where Cp is the particular heat at continuous pressure, ΔH is the enthalpy of the solution, ΔT is the change in temperature, W is the fixed of the solute, and also M is the molecule mass the the solute. The measurement of warm using a simple calorimeter, prefer the coffee cup calorimeter, is an example of constant-pressure calorimetry, since the press (atmospheric pressure) remains consistent during the process. Constant-pressure calorimetry is offered in identify the alters in enthalpy occurring in solution. Under these conditions the adjust in enthalpy equals the warmth (Q=ΔH).

Specific warmth for an ideal Gas at constant Pressure and also Volume

An ideal gas has different specific heat capacities under consistent volume or consistent pressure conditions.

Key Takeaways

Key PointsThe certain heat at constant volume for a gas is provided as (\frac\partial \textU\partial \textT)_\textV=\textc_\textv.The certain heat at constant pressure for suitable gas is given as (\frac\partial \textH\partial \textT)_\textV=\textc_\textp=\textc_\textv+\textR.The heat capacity proportion (or adiabatic index ) is the ratio of the heat capacity at continuous pressure to warmth capacity at consistent volume.Key TermsFundamental Thermodynamic Relation: In thermodynamics, the fundamental thermodynamic relation expresses an infinitesimal readjust in internal power in terms of infinitesimal changes in entropy, and volume because that a closed mechanism in thermal equilibrium in the following way: dU=TdS-PdV. Here, U is interior energy, T is pure temperature, S is entropy, p is pressure and V is volume.adiabatic index: The proportion of the heat capacity at constant pressure to warmth capacity at consistent volume.specific heat: The proportion of the quantity of warm needed to raise the temperature of a unit mass of problem by a unit degree to the amount of heat needed come raise the of the same mass the water by the same amount.

Specific warmth for an ideal Gas at continuous Pressure and also Volume

The warm capacity at consistent volume of nR = 1 J·K−1 of any type of gas, including perfect gas is:

(\frac\partial \textU\partial \textT)_\textV=\textc_\textv

This represents the dimensionless heat capacity at constant volume; that is typically a function of temperature due to intermolecular forces. Because that moderate temperatures, the constant for a monoatomic gas is cv=3/2 while because that a diatomic gas that is cv=5/2 (see ). Macroscopic measurements on heat capacity carry out information ~ above the microscopic structure of the molecules.

Molecular inner vibrations: as soon as a gas is heated, translational kientic power of molecules in the gas will certainly increase. In addition, molecules in the gas might pick up many characteristic interior vibrations. Potential energy stored in these internal degrees of flexibility contributes to certain heat that the gas.

The warmth capacity at constant pressure the 1 J·K−1 ideal gas is:

(\frac\partial \textH\partial \textT)_\textV=\textc_\textp=\textc_\textv+\textR

where H=U+pV is the enthalpy that the gas.

Measuring the warm capacity at continuous volume deserve to be prohibitively complicated for liquids and solids. The is, small temperature changes typically require large pressures to keep a liquid or solid at consistent volume (this indicates the containing vessel need to be virtually rigid or at least an extremely strong). It is easier to measure up the warm capacity at continuous pressure (allowing the material to increase or contract freely) and solve because that the warm capacity at continuous volume making use of mathematical relationships obtained from the simple thermodynamic laws.

Utilizing the basic Thermodynamic relation we have the right to show:

\textC_\textp-\textC_\textV=\textT(\frac\partial \textP\partial \textT)_\textV,\textN(\frac\partial \textV\partial \textT)_\textp,\textN

where the partial derivatives are taken at: consistent volume and continuous number that particles, and at constant pressure and constant number the particles, respectively.

The heat capacity ratio or adiabatic index is the proportion of the heat capacity at consistent pressure to warm capacity at continuous volume. The is sometimes also known as the isentropic growth factor:

\gamma =\frac\textC_\textP\textC_\textV=\frac\textc_\textp\textc_\textv

For an ideal gas, examining the partial derivatives over according to the equation that state, wherein R is the gas consistent for suitable gas yields:

\textpV = \textRT

\textC_\textp-\textC_\textV=\textT(\frac\partial \textP\partial \textT)_\textV(\frac\partial \textV\partial \textT)_\textp

\textC_\textp-\textC_\textV=-\textT(\frac\partial \textP\partial \textV)_\textV(\frac\partial \textV\partial \textT)_\textp^2

\textP=\frac\textRT\textV\textn \to (\frac\partial \textP\partial \textV)_\textT=\frac-\textRT\textV^2=\frac-\textP\textV

\textV=\frac\textRT\textP\textn \to (\frac\partial \textV\partial \textT)^2_\textp=\frac\textR^2\textP^2


-\textT(\frac\partial \textP\partial \textV)_\textV(\frac\partial \textV\partial \textT)_\textp^2=-\textT\frac-\textP\textV\frac\textR^2\textP^2=\textR

This equation reduces simply to what is well-known as Mayer’s relation:

Julius Robert Mayer: Julius Robert von Mayer (November 25, 1814 – march 20, 1878), a German physician and also physicist, was one of the founders of thermodynamics. The is finest known because that his 1841 enunciation of among the initial statements that the preservation of power (or what is now well-known as one of the first versions of the first law of thermodynamics): “Energy can be neither produced nor destroyed. ” In 1842, Mayer explained the an important chemical procedure now referred to as oxidation together the primary source of power for any type of living creature. His achievements were overlooked and credit for the discovery of the mechanical tantamount of warmth was attributed to James Joule in the complying with year. Von Mayer likewise proposed the plants transform light into chemical energy.


It is a simple equation relating the warm capacities under continuous temperature and under constant pressure.

Solving troubles with Calorimetry

Calorimetry is provided to measure up the amount of heat created or consumed in a chemical reaction.

Learning Objectives

Explain a bomb calorimeter is supplied to measure up heat advanced in a combustion reaction

Key Takeaways

Key PointsCalorimetry is used to measure quantities of heat transferred to or native a substance.A calorimeter is a an equipment used to measure up the quantity of heat affiliated in a chemical or physical process.This means that the lot of heat developed or consumed in the reaction equates to the quantity of heat absorbed or lost by the solution.Key Termsheat that reaction: The enthalpy readjust in a chemistry reaction; the quantity of heat that a systems gives up come its next site so it can return to its initial temperature.combustion: A process where 2 chemicals are combined to produce heat.

Calorimeters space designed to minimize power exchange in between the mechanism being studied and also its surroundings. They variety from basic coffee cup calorimeters used by introductory chemistry student to advanced bomb calorimeters used to identify the energy content the food.

Calorimetry is supplied to measure quantities of warmth transferred to or indigenous a substance. To perform so, the heat is exchanged through a calibrated thing (calorimeter). The change in temperature of the measuring part of the calorimeter is converted right into the amount of warmth (since the vault calibration was used to develop its warm capacity ). The measure up of warm transfer making use of this method requires the definition of a device (the problem or substances experience the chemical or physical change) and its surroundings (the other materials of the measurement device that offer to either administer heat to the mechanism or absorb heat from the system). Understanding of the warm capacity the the surroundings, and careful dimensions of the masses the the system and also surroundings and also their temperature before and after the process allows one to calculate the warm transferred as explained in this section.

A calorimeter is a an equipment used to measure up the quantity of heat associated in a chemistry or physics process. Because that example, once an exothermic reaction occurs in solution in a calorimeter, the heat created by the reaction is took in by the solution, which increases its temperature. When an endothermic reaction occurs, the heat forced is absorbed from the thermal power of the solution, i m sorry decreases that is temperature. The temperature change, along with the specific heat and also mass that the solution, deserve to then be used to calculate the lot of heat affiliated in either case.

Coffee-Cup Calorimeters

General chemistry students often use straightforward calorimeters constructed from polystyrene cups. This easy-to-use “coffee cup” calorimeters allow an ext heat exchange through their surroundings, and also therefore produce less accurate energy values.

Structure the the continuous Volume (or “Bomb”) Calorimeter

Bomb Calorimeter: This is the snapshot of a common setup of bomb calorimeter.

A different type of calorimeter that operates at continuous volume, colloquially recognized as a bomb calorimeter, is provided to measure the energy developed by reactions the yield large amounts the heat and gaseous products, such as burning reactions. (The ax “bomb” comes from the monitoring that these reactions deserve to be vigorous enough to resemble explosions that would damage other calorimeters.) This form of calorimeter consists of a robust steel container (the “bomb”) that includes the reactants and also is itself submerged in water. The sample is inserted in the bomb, i m sorry is then filled through oxygen in ~ high pressure. A tiny electrical spark is offered to ignite the sample. The energy produced by the reaction is trapped in the stole bomb and also the surrounding water. The temperature boost is measure up and, in addition to the known heat capacity of the calorimeter, is provided to calculate the energy created by the reaction. Bomb calorimeters call for calibration to recognize the heat capacity of the calorimeter and ensure exact results. The calibration is achieved using a reaction v a known q, such together a measured amount of benzoic mountain ignited through a spark indigenous a nickel fuse wire the is weighed before and after the reaction. The temperature adjust produced by the recognized reaction is supplied to determine the warmth capacity the the calorimeter. The calibration is normally performed every time prior to the calorimeter is provided to gather research study data.

Example: identifying a steel by Measuring particular Heat

A 59.7 g item of steel that had actually been submerged in boiling water was easily transferred into 60.0 mL of water at first at 22.0 °C. The last temperature is 28.5 °C. Usage these data to determine the particular heat of the metal. Use this result to recognize the metal.

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Assuming perfect heat transfer, the heat offered off by steel is the negative of the warmth taken in by water, or:


In expanded form, this is:

\textc_\textmetal \times \textm_\textmetal \times \left( \textT_\textf,metal-\textT_\texti,metal \right) = \textc_\textwater \times \textm_\textwater \times \left( \textT_\textf,water-\textT_\texti,water \right)

Noting that since the steel was submerged in boiling water, its initial temperature was 100.0 °C; and also that because that water, 60.0 mL = 60.0 g; we have:

\left( \textc_\textmetal \right)\left( 59.7\text g \right)\left( 28.5^\texto \textC - 100.0^\texto \textC \right) = \left( 4.18 \text J/g^\texto \textC \right) \left( 60.0\text g \right)\left( 28.5^\texto \textC - 22.0^\texto \textC \right)

Solving this:

\textc_\textmetal = \dfrac- \left( 4.184 \text J/g^\texto \textC \right) \left( 60.0\text g \right)\left( 6.5^\texto \textC \right)\left( 59.7\text g \right)\left( -71.5^\texto \textC \right) = 0.38 \text J/g^\texto \textC

Our experimental details heat is closest come the value for copper (0.39 J/g °C), so we identify the steel as copper.