Name: coffee cup calorimeter heat changes
Uploaded: 2020-09-03T13:38:27.000Z
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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

W przypadku reakcji chemicznej zachodzącej pod stałym ciśnieniem, takim jak ciśnienie atmosferyczne, ciepło wymieniane podczas procesu mierzy się jako zmianę entalpii ΔH. Zmiana entalpii reakcji objawia się zmianą temperatury, która jest mierzona za pomocą techniki zwanej kalorymetrią.
W kalorymetrii reakcja odbywa się w szczelnie zamkniętym i skalibrowanym pojemniku zwanym kalorymetrem. Kalorymetr jest dobrze izolowany i zapobiega jakiemukolwiek przepływowi ciepła między sobą a otoczeniem.
W ten sposób ciepło wymieniane między reagentami i produktami (które składają się na układ) a kalorymetrem (którym jest otoczenie), można dokładnie obliczyć, monitorując późniejsze zmiany temperatury w kalorymetrze.
Jeśli reakcja jest egzotermiczna, ciepło przepływa z układu do otoczenia, a temperatura wzrasta. I odwrotnie, jeśli reakcja jest endotermiczna, ciepło przepływa z otoczenia do układu, powodując spadek temperatury kalorymetru.
Prosty kalorymetr filiżanki kawy mierzy zmianę entalpii reakcji zachodzącej w roztworze w warunkach stałego ciśnienia.
Kalorymetr składa się z dwóch styropianowych filiżanek do kawy zagnieżdżonych razem i wyposażonych w termometr i mieszadło. Kalorymetr jest zamknięty luźno dopasowaną pokrywką z korka, aby utrzymać warunki stałego ciśnienia otwartego na atmosferę.
Załóżmy, że po 50,0 mililitrów 1,0 molowego wodnego roztworu kwasu solnego i 1,0 molowego wodnego roztworu potasu znajduje się reakcja w kalorymetrze, aby podnieść temperaturę roztworu o 6,9 °C.
Ciepło pochłonięte przez roztwór, roztwór q, jest równe jego ciepłu właściwemu, Cs, (4,18 J/g·°C) - tuż poniżej ciepła wody - pomnożonemu przez jego masę całkowitą, m (100,0 g) i zmianę temperatury.
Ciepło roztworu wynosi 2,9 × 103 dżuli lub 2,9 kilodżuli. Ciepło reakcji, reakcja q, ma tę samą wartość, ale z przeciwnym znakiem. Ponieważ ciśnienie jest stałe, zmiana entalpii jest taka sama jak ciepło reakcji.
Aby znaleźć zmianę entalpii reakcji na mol, entalpię dzieli się przez liczbę moli kwasu solnego. Mole kwasu solnego znajduje się przez pomnożenie objętości w litrach (0,05 l) przez molowość (1 molowiec). Dlatego minus 2,9 kilodżuli podzielone przez 0,050 mola daje minus 58 kilodżuli na mol.

<ol>
	<li>Banna, M. Salim. "Grzałka do kalorymetrii stałociśnieniowej." Journal of Chemical Education 63, nr 11 (1986): 997.</li>
	<li>Ruekberg, Ben. "Ekonomiczny, bezpieczny i wytrzymały kalorymetr studencki." Journal of Chemical Education 71, nr 4 (1994): 333.</li>
	<li>Stankus, John J. i Jennifer D. Caraway. "Zastąpienie kalorymetrów filiżankowych kawą kalorymetrami zlewkowymi." Journal of Chemical Education 88, nr 12 (2011): 1730-1731. 
	 </li>
</ol>

kalorymetria stałociśnieniowa

Kalorymetria to technika stosowana do pomiaru ilości ciepła zaangażowanego w proces chemiczny lub fizyczny lub do pomiaru ciepła przekazywanego do lub z substancji. Wymiana ciepła odbywa się za pomocą skalibrowanego i izolowanego urządzenia zwanego kalorymetrem. Eksperymenty kalorymetryczne opierają się na założeniu, że pomiędzy izolowanym kalorymetrem a otoczeniem zewnętrznym nie zachodzi wymiana ciepła. Dobrze izolowane kalorymetry zapobiegają przenoszeniu ciepła pomiędzy kalorymetrem a jego środowiskiem zewnętrznym, co skutecznie ogranicza „otoczenie” niesystemowych elementów kalorymetru (i samego kalorymetru). Umożliwia to dokładne określenie ciepła towarzyszącego procesom chemicznym, np. zawartości energetycznej żywności.

Zmiana temperatury mierzona przez kalorymetr służy do obliczenia ilości ciepła przekazanego w badanym procesie. W kalorymetrze układ definiuje się jako substancję lub substancje podlegające przemianie chemicznej lub fizycznej, czyli innymi słowy, reakcji, a otoczenie to cała inna materia, w tym roztwór i wszelkie inne składniki kalorymetru, które albo dostarczają ciepło do systemu lub pochłaniają ciepło z systemu.

Zanim omówimy kalorymetrię reakcji chemicznych, rozważmy prostszy przykład, który ilustruje podstawową ideę kalorymetrii. Załóżmy, że gorący kawałek metalu o wysokiej temperaturze umieszcza się w substancji o niskiej temperaturze, takiej jak zimna woda. Ciepło będzie przepływać od gorącego metalu do wody. Temperatura metalu będzie spadać, a temperatura wody będzie rosła, aż obie substancje osiągną tę samą temperaturę – to znaczy osiągną równowagę termiczną. Jeżeli ma to miejsce w kalorymetrze, całe ciepło jest przenoszone pomiędzy dwiema substancjami, bez utraty ciepła przez środowisko zewnętrzne. W tych idealnych okolicznościach zmiana ciepła netto wynosi zero:

<img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-01.png" style="height: 40px;">

Zależność tę można przekształcić tak, aby pokazać, że ciepło uzyskane przez metal jest równe ciepłu utraconemu przez substancję, czyli wodę:

<img alt="Eq2" src="https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-02.png" style="height: 40px;">

Wielkość ciepła (zmiany ciepła) jest zatem taka sama dla obu substancji. Znak ujemny pokazuje jedynie, że qmetal i qwoda mają przeciwny kierunek przepływu ciepła (zysk lub strata), ale nie wskazuje znaku arytmetycznego żadnej wartości q (która jest określona przez to, czy dana materia zyskuje, czy traci ciepło, zgodnie z definicja). W opisanej konkretnej sytuacji qmetal jest wartością ujemną, a qwoda jest wartością dodatnią, ponieważ ciepło jest przenoszone z metalu do wody.

W przypadku stosowania kalorymetrii do określenia ciepła biorącego udział w reakcji chemicznej obowiązują te same zasady. Ilość ciepła pochłonięta przez kalorymetr jest często na tyle mała, że najczęściej można ją pominąć, a kalorymetr minimalizuje wymianę energii z otoczeniem zewnętrznym. Kiedy w roztworze kalorymetru zachodzi reakcja egzotermiczna, ciepło wytworzone w wyniku reakcji jest absorbowane przez roztwór, co zwiększa jego temperaturę. Kiedy zachodzi reakcja endotermiczna, wymagane ciepło jest pochłaniane z energii cieplnej roztworu, co powoduje obniżenie jego temperatury. Zmiana temperatury (ΔT) wraz z ciepłem właściwym (csoln) i masą roztworu (msoln) można następnie wykorzystać do obliczenia ilości ciepła (qsoln) zaangażowanego w obu przypadkach.

<img alt="Eq3" src="https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-03.png" style="height: 40px;">

Prosty kalorymetr – zwany kalorymetrem kubkowym – zbudowany jest z dwóch zagnieżdżonych kubków polistyrenowych zamkniętych luźną pokrywką. Kalorymetry kubkowe służą do pomiaru ciepła reakcji zachodzących w roztworach (głównie roztworach wodnych), przy których nie zachodzi żadna zmiana objętości lub jest ona bardzo niewielka. Ponieważ energia nie jest wytwarzana ani niszczona podczas reakcji chemicznej, ciepło wytworzone lub zużyte w reakcji („system”), qrxn, plus ciepło pochłonięte lub utracone przez roztwór („otoczenie”), qsoln, musi się sumować do zera:

<img alt="Eq4" src="https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-04.png" style="height: 40px;">

Oznacza to, że ilość ciepła wytworzonego lub zużytego w reakcji jest równa ilości ciepła pobranego lub utraconego przez roztwór:

<img alt="Eq5" src="https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-05.png" style="height: 40px;">

Kalorymetr filiżankowy do kawy jest kalorymetrem stałociśnieniowym, a zmierzone ciepło reakcji jest równoważne zmianie entalpii.

<img alt="Eq6" src="https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-06.png" style="height: 40px;">

Kalorymetria stałociśnieniowa

Kalorymetria to technika stosowana do pomiaru ilości ciepła zaangażowanego w proces chemiczny lub fizyczny lub do pomiaru ciepła przenoszonego do lub z ...

Education

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Kluczowe terminy i pojęcia

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...

constant pressure calorimetry

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...

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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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Coffee Cup Calorimeter Heat Changes

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