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

대기압과 같은 일정한 압력 조건에서 화학 반응이 수행되는 경우 공정 중에 교환되는 열은 엔탈피의 변화 델타 H로 측정됩니다. 반응에서 엔탈피 변화는 온도의 변화로 분명하게 나타나며 이 변화는 열량 측정법을 사용하여 측정됩니다. 열량 측정법에서는 열량계라고 하는 밀봉되고 교정된 용기에서 반응이 실행됩니다.

열량계는 절연이 잘 되어있어 환경과의 열 흐름을 방지합니다. 따라서 계를 구성하는 반응물 및 생성물과, 주위가 되는 열량계 사이에 교환되는 열은 열량계의 온도 변화를 모니터링하여 정확하게 계산할 수 있습니다. 반응이 발열성인 경우 열은 계에서 주위로 흐르며 온도가 상승합니다.

반대로 반응이 흡열성이면 열은 주위로부터 계로 흘러들어 열량계의 온도가 떨어지게 됩니다. 간단한 커피컵 열량계로 일정한 압력 조건에서 용액에서 발생하는 반응의 엔탈피 변화를 측정해 봅시다. 열량계는 온도계와 교반기가 장착된 두 개의 스티로폼 커피 컵으로 구성되어 있습니다.

열량계는 헐렁한 코르크 뚜껑으로 닫겨 있어 대기에 개방된 일정한 압력 상태를 유지합니다. 1.0몰의 염산 수용액과 1.0몰의 수산화칼륨 수용액 각각 50.0밀리리터가 열량계 내부에서 반응하여 용액의 온도를 섭씨 6.9도 상승시킨다고 가정합니다. 용액에 흡수된 열, q 용액은 물의 경우 전체 질량 m, 즉 100.0 그램에 온도 변화를 곱한 것처럼 그램 섭씨 1도당 4.18줄의 비열과 같습니다.

용액의 열은 2.9 곱하기 10의 3제곱 줄 또는 2.9 키로줄입니다. 반응열 q 반응 은 값은 같지만 부호는 반대입니다. 압력이 일정하기 때문에 엔탈피 변화는 반응의 열과 동일합니다.

몰당 반응의 엔탈피 변화를 찾기 위해 엔탈피를 염산의 몰수로 나눕니다. 염산의 몰은 리터 단위의 부피 0.05 리터에 몰농도 1을 곱하여 구할 수 있습니다. 따라서 마이너스 2.9 킬로 줄을 0.050 몰로 나누면 몰당 마이너스 58 킬로 줄이 됩니다.

<ol>
	<li>Banna, M. Salim. "정압 열량계용 히터." 화학 교육 저널 63, no. 11 (1986): 997.</li>
	<li>Ruekberg, Ben. "경제적이고 안전하며 견고한 학생 열량계." 화학 교육 저널 71, no. 4 (1994): 333.</li>
	<li>Stankus, John J. 및 Jennifer D. Caraway. "커피 컵 열량계를 제작된 비커 열량계로 교체." 화학 교육 저널 88, no. 12 (2011): 1730-1731. 
	 </li>
</ol>

일정압력 열량계

열량계는 화학적 또는 물리적 공정과 관련된 열의 양을 측정하거나 물질로 전달되거나 물질에서 전달되는 열을 측정하는 데 사용되는 기술입니다. 열은 열량계라고 불리는 보정되고 절연된 장치를 통해 교환됩니다. 열량측정 실험은 단열 열량계와 외부 환경 사이에 열 교환이 없다는 가정을 기반으로 합니다. 잘 절연된 열량계는 열량계와 외부 환경 사이의 열 전달을 방지하여 "주변"을 열량계(및 열량계 자체) 내의 비시스템 구성 요소로 효과적으로 제한합니다. 이를 통해 식품의 에너지 함량과 같은 화학 공정과 관련된 열을 정확하게 측정할 수 있습니다.

열량계로 측정된 온도 변화는 연구 중인 공정에 의해 전달된 열의 양을 도출하는 데 사용됩니다. 열량계에서 시스템은 화학적 또는 물리적 변화, 즉 반응을 겪는 물질로 정의되며, 주변은 열을 제공하는 열량계의 용액 및 기타 구성 요소를 포함하여 다른 모든 물질입니다. 시스템에 유입되거나 시스템에서 열을 흡수합니다.

화학 반응의 열량 측정법을 논의하기 전에 열량 측정의 핵심 아이디어를 설명하는 더 간단한 예를 고려하십시오. 고온의 뜨거운 금속 조각이 차가운 물과 같은 저온의 물질 속에 놓여 있다고 가정해 봅시다. 열은 뜨거운 금속에서 물로 흐릅니다. 두 물질의 온도가 같아질 때까지, 즉 열평형에 도달할 때까지 금속의 온도는 감소하고 물의 온도는 증가합니다. 열량계에서 이런 일이 발생하면 외부 환경에 의해 열을 얻거나 잃지 않고 모든 열이 두 물질 사이에 전달됩니다. 이러한 이상적인 상황에서 순 열 변화는 0입니다.

<img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-01.png" style="height: 40px;" />

이 관계는 금속이 얻은 열이 물이 잃은 열과 동일하다는 것을 보여주기 위해 재배열될 수 있습니다.

<img alt="Eq2" src="https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-02.png" style="height: 40px;" />

따라서 열(변화)의 크기는 두 물질 모두 동일합니다. 음의 부호는 q_metal과 q_water가 열 흐름 방향(증가 또는 손실)이 반대라는 것을 나타낼 뿐, q 값(즉, 문제의 물질이 열을 얻거나 잃느냐에 따라 결정되는지에 따라 결정됨)의 산술 부호를 나타내지는 않습니다. 정의). 설명된 특정 상황에서 q_metal은 음수 값이고 q_water는 열이 금속에서 물로 전달되므로 양수 값입니다.

화학 반응과 관련된 열을 측정하기 위해 열량계를 사용할 때도 동일한 원리가 적용됩니다. 열량계가 흡수하는 열의 양은 종종 무시할 수 있을 만큼 작으며, 열량계는 외부 환경과의 에너지 교환을 최소화합니다. 열량계의 용액에서 발열 반응이 일어날 때, 반응에 의해 생성된 열이 용액에 흡수되어 온도가 상승합니다. 흡열 반응이 일어날 때 필요한 열은 용액의 열 에너지로부터 흡수되어 온도가 감소합니다. 그런 다음 온도 변화(ΔT)를 비열(c_soln) 및 용액의 질량(m_soln)과 함께 사용하여 두 경우 모두에 관련된 열량(q_soln)을 계산할 수 있습니다.

<img alt="Eq3" src="https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-03.png" style="height: 40px;" />

커피 컵 열량계라고 불리는 간단한 열량계는 느슨한 뚜껑으로 닫힌 두 개의 폴리스티렌 컵으로 구성됩니다. 커피 컵 열량계는 용액(주로 수용액)에서 발생하고 부피 변화가 없거나 거의 없는 반응열을 측정하는 데 사용됩니다. 화학 반응 중에 에너지가 생성되거나 파괴되지 않기 때문에 반응("시스템")에서 생성되거나 소비되는 열인 q_rxn과 용액("주변")에 의해 흡수되거나 손실되는 열인 q_soln이 합해서 0이여야 합니다.

<img alt="Eq4" src="https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-04.png" style="height: 40px;" />

이는 반응에서 생성되거나 소비되는 열의 양이 용액에 의해 흡수되거나 손실되는 열의 양과 동일하다는 것을 의미합니다.

<img alt="Eq5" src="https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-05.png" style="height: 40px;" />

커피 컵 열량계는 정압 열량계이며, 측정된 반응열은 엔탈피 변화와 동일합니다.

<img alt="Eq6" src="https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-06.png" style="height: 40px;" />



이 문서는 에서 발췌되었습니다 <a href="https://openstax.org/books/chemistry-2e/pages/5-2-calorimetry">Openstax, Chemistry 2e, Section 5.2: Calorimetry</a>.

열량계는 화학적 또는 물리적 공정과 관련된 열의 양을 측정하거나 열량계로 전달되는 열을 측정하는 데 사용되는 기술입니다.

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화학

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Thermochemistry

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KEY TERMS AND CONCEPTS

주요 용어 및 개념

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

energy basics

How Energy Changes in Chemical Reactions

Chemical reactions change matter and energy at the same time. A match lighting is a simple example. These energy changes are part of everyday life and appear in food, fuels, and industry. Food provides energy through metabolic reactions. The macronutrients in food break down and help keep the body functioning. Fuels such as gasoline, natural gas, and coal are burned to produce energy for transportation, heating, and electricity generation. Industrial chemical reactions also use large amounts...

first law of thermodynamics

Energy Conservation and Internal Energy

Energy conservation describes how energy changes form during chemical and physical changes. Energy can be converted from one form into another, but the energy present before a change still exists in some form after the change is complete. This is the law of conservation of energy. It says energy can neither be created nor destroyed. The law of conservation of matter also applies during chemical change. In most chemical reactions, the total amount of matter does not show a detectable change.

internal energy

Internal Energy, Heat, and Work

Internal energy is the total of all possible kinds of energy in a substance. It is often written as U, and sometimes as E. For a system that changes energy, the important value is the change in internal energy, or ΔU. ΔU is the difference between the final internal energy and the initial internal energy. The exact values of U final and U initial are usually not known, but the first law of thermodynamics only requires ΔU. A positive ΔU means the system gained energy from the surroundings. A...

quantifying heat

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quantifying work

Pressure-Volume Work in Chemistry

Pressure-volume work shows how gas volume changes can transfer energy in chemistry. As a system changes, its internal energy may change too. Energy can move between the system and the surroundings through heat and work. Internal energy, heat, and work are related by an energy equation. Heat depends on a measured temperature change. Work depends on a measured change in volume called pressure-volume work. Work can be defined as a force acting through a distance. Pressure-volume work, also...

enthalpy

Enthalpy and Heat at Constant Pressure

Enthalpy describes heat changes in chemical and physical processes. Chemists use the symbol H for enthalpy. It is defined as a system’s internal energy, E, plus the product of pressure, P, and volume, V. Enthalpy is a state function, so only changes in enthalpy can be measured, not the enthalpy of a substance by itself. For many reactions, the pressure stays constant. Under those conditions, the enthalpy change, ΔH, can be written in a way that includes pressure-volume work. The term PΔV...

thermochemical equations

Heat Changes in Chemical Equations

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

Bomb Calorimeter Heat Measurement

Bomb calorimetry measures the heat released by reactions that produce a lot of energy, especially combustion reactions. A coffee cup calorimeter works at constant pressure and is useful for reactions in solution. A bomb calorimeter works at constant volume and is used for reactions that make large amounts of heat and gaseous products. The word "bomb" refers to the strong, explosive force some reactions can have. In a bomb calorimeter, the volume does not change, so 94V = 0. That means the...

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Calculating Reaction Heat with Hess's Law

Calculating reaction heat with Hess's law lets chemists find enthalpy changes without measuring every reaction directly. Some reactions are hard or impossible to test in the lab. Even when a reaction can be measured, it is often easier to calculate the heat change from other known enthalpy values. Hess's law says that if a process can be written as the sum of several stepwise processes, the enthalpy change for the total process equals the sum of the enthalpy changes for the steps. This works...

standard enthalpy of formation

Using Standard Enthalpy Values in Chemistry

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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Clausius-Clapeyron Equation

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Quantifying Work

As a system undergoes a change, its internal energy can change, and energy can be transferred from the system to the surroundings, or from the ...

Enthalpy

Chemists ordinarily use a property known as enthalpy (H) to describe the thermodynamics of chemical and physical processes. Enthalpy is defined as the sum ...

Thermochemical Equations

For a chemical reaction (the system) carried out at constant pressure &ndash; with the only work done caused by expansion or contraction &ndash; the ...

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 ...

Constant Volume Calorimetry

Calorimeters are useful to determine the heat released or absorbed by a chemical reaction. Coffee cup calorimeters are designed to operate at constant ...

using-differential-scanning-calorimetry-to-measure-changes-in-enthalpy

Using Differential Scanning Calorimetry to Measure Changes in Enthalpy

Source: Laboratory of Dr. Terry Tritt &#8212; Clemson University
Differential Scanning Calorimetry (DSC) is a method of thermodynamic analysis based on ...

Hess's Law

There are two ways to determine the amount of heat involved in a chemical change: measure it experimentally, or calculate it from other experimentally ...

Standard Enthalpy of Formation

Enthalpy changes are typically tabulated for reactions in which both the reactants and products are at the same conditions. A standard state is a commonly ...

Enthalpies of Reaction

Hess&rsquo;s law can be used to determine the enthalpy change of any reaction if the corresponding enthalpies of formation of the reactants and products ...

Use mathematics and computational thinking to execute simple calorimetric calculations based on the Law of Conservation of Energy.

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Definition and Measurement of Pressure: Atmospheric Pressure, Barometer, and Manometer

Gas pressure is caused by force exerted by gas molecules colliding with the surfaces of objects. Although the force of each collision is very small, any ...

gas-laws-boyle-s-gay-lussac-charles-avogadro-s-and-ideal-gas-law

Gas Laws: Boyle's, Gay-Lussac, Charles', Avogadro's, and Ideal Gas Law

Through experiments, scientists established the mathematical relationships between pairs of variables, such as pressure and temperature, pressure and ...

applications-of-the-ideal-gas-law-molar-mass-density-and-volume

Applications of the Ideal Gas Law: Molar Mass, Density, and Volume

The volume occupied by one mole of a substance is its molar volume. The ideal gas law, PV = nRT, &nbsp;suggests that the volume of a given quantity of gas ...

mixtures-of-gases-dalton-s-law-of-partial-pressures-and-mole-fractions

Mixtures of Gases: Dalton's Law of Partial Pressures and Mole Fractions

Unless individual gases chemically react with each other, the individual gases in a mixture of gases do not affect each other&rsquo;s pressure. Each gas ...

chemical-stoichiometry-gases-using-ideal-gas-law-to-determine

Chemical Stoichiometry and Gases: Using Ideal Gas Law to Determine Moles

Chemical stoichiometry describes the quantitative relationships between reactants and products in chemical reactions.

In addition to measuring quantities ...

basic-postulates-kinetic-molecular-theory-particle-size-energy

Basic Postulates of Kinetic Molecular Theory: Particle Size, Energy, and Collision

The ideal-gas equation, which is empirical, describes the behavior of gases by establishing relationships between their macroscopic properties. For ...

kinetic-molecular-theory-gas-laws-explain-properties-gas

Kinetic Molecular Theory and Gas Laws Explain Properties of Gas Molecules

The test of the kinetic molecular theory (KMT) and its postulates is its ability to explain and describe the behavior of a gas. The various gas laws ...

kinetic-molecular-theory-molecular-velocities-temperature-kinetic

Kinetic Molecular Theory: Molecular Velocities, Temperature, and Kinetic Energy

The kinetic molecular theory qualitatively explains the behaviors described by the various gas laws. The postulates of this theory may be applied in a ...

behavior-gas-molecules-molecular-diffusion-mean-free-path

Behavior of Gas Molecules: Molecular Diffusion, Mean Free Path, and Effusion

Although gaseous molecules travel at tremendous speeds (hundreds of meters per second), they collide with other gaseous molecules and travel in many ...

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Real Gases: Effects of Intermolecular Forces and Molecular Volume Deriving Van der Waals Equation

Thus far, the ideal gas law, PV = nRT, has been applied to a variety of different types of problems, ranging from reaction stoichiometry and empirical and ...

Ideal Gas Law

Source: Laboratory of Dr. Andreas Z&#252;ttel - Swiss Federal Laboratories for Materials Science and Technology
The ideal gas law describes the behavior ...

Derivation of the Ideal Gas Law
Gases are a fundamental state of matter. A gas is a collection of molecules that have a significant distance between their ...

Source: Smaa Koraym at Johns Hopkins University, MD, USA

	Preparation of the LaboratoryExpand
	Here, we show the laboratory preparation for 10 students ...

Source: Smaa Koraym at Johns Hopkins University, MD, USA

	Determining the Mass of the Unknown LiquidExpand
	According to the ideal gas law for a given ...

Use mathematics and computational thinking to explain the relationships among pressure, temperature, volume, and quantity of gas, both qualitatively and quantitatively.

PS.Chm.7.3

Understand the relationship among pressure, temperature, volume, and phase.

Coffee Cup Calorimeter Heat Changes

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