Name: coffee cup calorimeter heat changes
Uploaded: 2020-09-03T13:38:27.000Z
Duration: 3 min 2 s
Channel: JoVE

K12 Standards

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North Carolina K-12 Science Standard Course of Study

9-12

Chemistry

Energy

PS.Chm.7.2

Constant Pressure Calorimetry

For a chemical reaction carried out under constant pressure, such as atmospheric pressure, the heat exchanged during the process is measured as the change in enthalpy &#916;H. The enthalpy change for the reaction is manifested as a change in temperature, which is measured using a technique called calorimetry.
In calorimetry, the reaction is executed in a sealed and calibrated container called a calorimeter. The calorimeter is well insulated and prevents any heat flow between itself and its environment.
Thus, heat exchanged between the reactants and products (which constitute the system) and the calorimeter (which is the surroundings), can be accurately calculated by monitoring the subsequent changes in the temperature in the calorimeter.
If the reaction is exothermic, heat flows from the system into the surroundings, and the temperature rises. Conversely, if the reaction is endothermic, heat flows from the surroundings into the system, causing the temperature of the calorimeter to fall.
A simple coffee cup calorimeter measures change in enthalpy of a reaction occurring in a solution, under constant pressure conditions.
The calorimeter consists of two Styrofoam coffee cups nested together and equipped with a thermometer and a stirrer. The calorimeter is closed with a loose-fitting cork lid to maintain conditions of constant pressure that is open to the atmosphere.
Suppose 50.0 milliliters each of 1.0 molar aqueous hydrochloric acid and 1.0 molar aqueous potassium hydroxide, react within the calorimeter, to raise the temperature of the solution by 6.9 &#176;C.
The heat absorbed by the solution, qsolution, is equal to its specific heat, Cs, (4.18 J/g&#183;&#176;C) &#8212; just below that of water &#8212; multiplied by its total mass, m (100.0 g), and the change in temperature.
The heat of the solution is 2.9 &#215; 103 joules or 2.9 kilojoules. The heat of the reaction, qreaction, has the same value but with an opposite sign. Because the pressure is constant, the enthalpy change is the same as the heat of the reaction.
To find the enthalpy change of the reaction per mole, the enthalpy is divided by the number of moles of hydrochloric acid. The moles of hydrochloric acid are found by multiplying the volume in liters (0.05 L) with the molarity (1 molar). Therefore, negative 2.9 kilojoules divided by 0.050 moles gives negative 58 kilojoules per mole.

constant pressure calorimetry

Calorimetry is a technique used to measure the amount of heat involved in a chemical or physical process or to measure the heat transferred to or from a substance. The heat is exchanged with a calibrated and insulated device called the calorimeter. Calorimetry experiments are based on the assumption that there is no heat exchange between the insulated calorimeter and the external environment. The well-insulated calorimeters prevent the transfer of heat between the calorimeter and its external environment, which effectively limits the &#8220;surroundings&#8221; to the nonsystem components within the calorimeter (and the calorimeter itself). This enables the accurate determination of the heat involved in chemical processes, such as the energy content of foods. 
The temperature change measured by the calorimeter is used to derive the amount of heat transferred by the process under study. In a calorimeter, a system is defined as the substance or substances undergoing the chemical or physical change, or in other words, the reaction, and the surroundings are all other matter, including the solution and any other components in the calorimeter that either provide heat to the system or absorb heat from the system.
Before discussing the calorimetry of chemical reactions, consider a simpler example that illustrates the core idea behind calorimetry. Suppose a hot piece of metal at a high-temperature is placed in a low-temperature substance, such as cool water. Heat will flow from the hot metal to the water. The temperature of the metal will decrease, and the temperature of the water will increase until the two substances have the same temperature&#8212;that is when they reach thermal equilibrium. If this occurs in a calorimeter, all of the heat is transferred between the two substances, with no heat gained or lost by its external environment. Under these ideal circumstances, the net heat change is zero:
<img alt="Heat transfer equation, \( q_{\text{metal}} + q_{\text{water}} = 0 \), thermodynamic process analysis." src="/files/core/CDNSource/lessons/798/798_Equations-01.png" style="height: 40px;" data-altupdatedat="1754904545000" data-alt="Heat equilibrium equation, q_metal + q_water = 0, formula for thermal exchange analysis." />
This relationship can be rearranged to show that the heat gained by the metal is equal to the heat lost by substance the water:
<img alt="Static equilibrium concept; q&#60;sub&#62;metal&#60;/sub&#62; = -q&#60;sub&#62;water&#60;/sub&#62;; equation illustrating heat transfer." src="/files/core/CDNSource/lessons/798/798_Equations-02.png" style="height: 40px;" data-altupdatedat="1754904545000" data-alt="Thermodynamics static equilibrium equation \(q_{\text{metal}} = -q_{\text{water}}\)." />
The magnitude of the heat (change) is, therefore, the same for both substances. The negative sign merely shows that qmetal and qwater are opposite in direction of heat flow (gain or loss), but it does not indicate the arithmetic sign of either q value (that is determined by whether the matter in question gains or loses heat, per definition). In the specific situation described, qmetal is a negative value and qwater is a positive value since heat is transferred from the metal to the water.
When using calorimetry to determine the heat involved in a chemical reaction, the same principles apply. The amount of heat absorbed by the calorimeter is often small enough that it can most often be neglected, and the calorimeter minimizes energy exchange with the outside environment. When an exothermic reaction occurs in solution in a calorimeter, the heat produced by the reaction is absorbed by the solution, which increases its temperature. When an endothermic reaction occurs, the heat required is absorbed from the thermal energy of the solution, which decreases its temperature. The temperature change (&#916;T), along with the specific heat (csoln) and mass of the solution (msoln), can then be used to calculate the amount of heat (qsoln) involved in either case.
<img alt="Calorimetry equation, \( q_{\text{soln}} = m_{\text{soln}} \times c_{\text{soln}} \times \Delta T \), formula." src="/files/core/CDNSource/lessons/798/798_Equations-03.png" style="height: 40px;" data-altupdatedat="1754904545000" data-alt="Calorimetry equation q=mc&#916;T, heat energy calculation formula for solution experiments." />
A simple calorimeter &#8212; called the coffee cup calorimeter &#8212; is constructed from two nested polystyrene cups closed with a loose-fitting lid. Coffee cup calorimeters are used to measure the heat of reactions that take place in solutions (mostly aqueous solutions) and involve no or very little volume change. Because energy is neither created nor destroyed during a chemical reaction, the heat produced or consumed in the reaction (the &#8220;system&#8221;), qrxn, plus the heat absorbed or lost by the solution (the &#8220;surroundings&#8221;), qsoln, must add up to zero:
<img alt="Thermochemistry equation q_rxn + q_soln = 0; heat transfer concept, enthalpy balance." src="/files/core/CDNSource/lessons/798/798_Equations-04.png" style="height: 40px;" data-altupdatedat="1754904545000" data-alt="Thermochemistry equation: q_rxn + q_soln = 0; static equilibrium concept; educational formula." />
This means that the amount of heat produced or consumed in the reaction equals the amount of heat absorbed or lost by the solution:
<img alt="Calorimetry principle with equation \( q_{rxn} = -q_{soln} \), thermodynamic analysis." src="/files/core/CDNSource/lessons/798/798_Equations-05.png" style="height: 40px;" data-altupdatedat="1754904545000" data-alt="Chemical thermodynamics, equation \( q_{\text{rxn}} = -q_{\text{soln}} \), heat exchange process." />
The coffee cup calorimeter is a constant-pressure calorimeter, and the measured heat of the reaction is equivalent to the change in enthalpy.
<img alt="Thermochemistry equation \(q_{\text{rxn}} = \Delta H_{\text{rxn}}\); heat and enthalpy relation." src="/files/core/CDNSource/lessons/798/798_Equations-06.png" style="height: 40px;" data-altupdatedat="1754904545000" data-alt="Chemical thermodynamics formula: q_rxn = &#916;H_rxn equation illustrated for reaction heat analysis." />
This text is adapted from <a href="https://openstax.org/books/chemistry-2e/pages/5-2-calorimetry">Openstax, Chemistry 2e, Section 5.2: Calorimetry</a>.

Calorimetry is a technique used to measure the amount of heat involved in a chemical or physical process or to measure the heat transferred to or from a ...

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KEY TERMS AND CONCEPTS

coffee cup calorimeter heat changes

Coffee cup calorimetry measures heat changes in reactions and physical changes using an insulated calorimeter. The calorimeter is calibrated and designed to limit heat exchange with the outside environment. That makes it possible to measure the heat taken in or released by a substance more accurately, including the energy content of foods.

In calorimetry, the system is the substance or substances undergoing change. The surroundings are everything else inside the calorimeter, including the solution and any other components that can give heat to the system or absorb heat from it. The measured temperature change is then used to calculate the heat transferred in the process under study.

A simple example helps show the idea. If a hot piece of metal is placed in cool water, heat flows from the metal to the water until both reach thermal equilibrium, or the same temperature. In an ideal calorimeter, no heat is gained or lost by the external environment, so the heat lost by the metal equals the heat gained by the water. The two heat values have the same magnitude, but they point in opposite directions of heat flow.

The same rules apply when a chemical reaction happens in solution. For an exothermic reaction, the reaction gives off heat, and the solution absorbs it, so the solution temperature rises. For an endothermic reaction, the reaction absorbs heat from the solution, so the solution temperature falls. The temperature change, along with the solution mass and specific heat, can be used to find the heat involved.

A coffee cup calorimeter is a simple constant-pressure calorimeter made from two nested polystyrene cups with a loose-fitting lid. It is used for reactions in solution, mostly aqueous solutions, when there is little or no volume change. In this setup, the heat of the reaction, q rxn, and the heat of the solution, q soln, add up to zero. That means the heat released or absorbed by the reaction matches the heat gained or lost by the solution. Because the pressure stays constant, the measured heat change is the enthalpy change.

Coffee Cup Calorimeter Heat Changes

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Heat changes in chemical equations show how much energy a reaction releases or absorbs. At constant pressure, the enthalpy of reaction, or ΔHrxn, is equal to the heat exchanged with the surroundings, qp. Because this value depends on how much reactant takes part, it is an extensive property. The size and sign of ΔHrxn also depend on the reaction itself and on the physical states of the substances involved. An exothermic reaction has a negative ΔHrxn value, while an endothermic reaction has a...

Coffee cup calorimetry measures heat changes in reactions and physical changes using an insulated calorimeter. The calorimeter is calibrated and designed to limit heat exchange with the outside environment. That makes it possible to measure the heat taken in or released by a substance more accurately, including the energy content of foods. In calorimetry, the system is the substance or substances undergoing change. The surroundings are everything else inside the calorimeter, including the...

constant volume calorimetry

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hess's law

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standard enthalpy of formation

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Enthalpy changes are often listed for reactions that start and end under the same conditions. Chemists use a standard state as a reference set of conditions for comparing properties. In IUPAC terms, the standard state means 1 bar of pressure and 1 M solutions, but it does not set a temperature. Many thermochemical tables still use 1 atm as the reference pressure. Because the difference between 1 bar and 1 atm is very small, enthalpy change usually stays almost the same. A superscripted o in...

enthalpies of reaction

Calculating reaction heat with Hess's law uses standard enthalpies of formation to find the enthalpy change of a reaction. When the formation values for the reactants and products are known, the overall reaction can be broken into simpler stepwise reactions. This approach helps show how the heat change for the full reaction is built from smaller parts. First, the reactants are thought of as being decomposed into their component elements. The enthalpy change for this step is proportional to the...

key terms and concepts

Explore how a coffee cup calorimeter measures heat changes in solutions, from thermal equilibrium to exothermic and endothermic reactions at constant pressure.

Coffee Cup Calorimeter Heat Changes | JoVE K12

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Matter and its Interactions

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Coffee Cup Calorimeter Heat Changes

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