Name: coffee cup calorimeter heat changes
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Constant Pressure Calorimetry

Для химической реакции, проводимой при постоянном давлении, таком как атмосферное давление, теплообмен во время процесса измеряется как изменение энтальпии дельта H.Изменение энтальпии для реакции проявляется как изменение температуры, которое измеряется с помощью калориметрии. При калориметрии реакция проводится в герметичном откалиброванном контейнере, называемом калориметром. Калориметр хорошо изолирован и предотвращает любую утечку тепла из содержимого в окружающую среду.Таким образом, теплообмен между исходными веществами и продуктами, которые составляют систему, и калориметром, который является окружающей средой, можно точно рассчитать, отслеживая последующие изменения температуры в калориметре. Если реакция экзотермическая, тепло перетекает из системы в окружающую среду, и температура повышается. И наоборот, если реакция эндотермическая, тепло перетекает из окружающей среды в систему, вызывая падение температуры калориметра.Простой маленький калориметр измеряет изменение энтальпии реакции, протекающей в растворе, в условиях постоянного давления. Калориметр состоит из двух чашек из пенопласта, установленных вместе и оснащенных термометром и мешалкой. Калориметр закрыт неплотно закрывающейся пробковой крышкой для поддержания постоянного давления и открыт в атмосферу.Предположим, что 50, 0 миллилитров 1, 0 молярного водного раствора соляной кислоты и 1, 0 молярного водного раствора гидроксида калия вступают в реакцию в калориметре, повышая температуру раствора на 6, 9 градусов Цельсия. Тепло, поглощаемое раствором q раствор равно его удельной теплоемкости, C s, 4, 18 джоулей на грамм градус Цельсия так же, как тепло воды, умноженное на ее общую массу, m 100, 0 грамм, и изменения в температуре. Теплота раствора равна 2, 9 умножить на десять в 3 степени джоулей или 2, 9 килоджоулей.Теплота реакции q реакция имеет то же значение, но с противоположным знаком. Поскольку давление постоянно, изменение энтальпии совпадает с теплотой реакции. Чтобы найти изменение энтальпии реакции на моль, энтальпию делят на количество молей соляной кислоты.Количество молей соляной кислоты определяется умножением объема в литрах 0, 05 литров на молярность 1 моль. Следовательно, отрицательные 2, 9 килоджоулей, разделенные на 0, 050 моль, дают отрицательные 58 килоджоулей на моль.

<ol>
	<li>Банна, М. Салим. "Нагреватель для калориметрии с постоянным давлением." Журнал химического образования 63, No11 (1986): 997.</li>
	<li>Рюкберг, Бен. "Экономичный, безопасный и прочный студенческий калориметр." Журнал химического образования 71, No4 (1994): 333.</li>
	<li>Станкус, Джон Дж., и Дженнифер Д. Каравей. "Замена калориметров в кофейных чашках на калориметры с изготовленным стаканом." Журнал химического образования 88, No12 (2011): 1730-1731. 
	 </li>
</ol>

Калориметрия постоянного давления

Калориметрия — это метод, используемый для измерения количества тепла, выделенного в химическом или физическом процессе, или для измерения температуры, передаваемой веществу или из него. Тепло обменивается калиброванным и изолированным устройством, называемым калориметром. Эксперименты с калориметрией основаны на предположении, что теплообмен между изолированным калориметром и внешней средой отсутствует. Хорошо изолированные калориметры предотвращают передачу тепла между калориметром и его внешней средой, что эффективно ограничивает «окружение» несистемными компонентами в пределах калориметра (и самого калориметра). Это позволяет точно определить температуру, которая используется в химических процессах, например, содержание энергии в продуктах.  
 
 Изменение температуры, измеренное калориметром, используется для получения количества тепла, передаваемого исследуемым процессом. В калориметре система определяется как вещество или вещества, претерпеющие химические или физические изменения, или, другими словами, реакция, а вокруг все остальные вопросы, включая раствор и любые другие компоненты в калориметре, которые либо обеспечивают тепло системе, либо поглощают тепло из системы. 
 
 Перед обсуждением калориметрии химических реакций рассмотрите более простой пример, иллюстрирующий основную идею калориметрии. Предположим, что горячий кусок металла при высокой температуре помещается в низкотемпературное вещество, например, в прохладную воду. Тепло будет поступать из горячего металла в воду. Температура металла снизится, а температура воды будет повышаться до тех пор, пока два вещества не нагреются до той же температуры, то есть, когда они достигнут теплового равновесия. Если это происходит в калориметре, все тепло переносится между двумя веществами, без нагрева, получаемого или теряемого его внешней средой. В этих идеальных условиях изменение температуры в сети равно нулю: 
 
 <img alt=""Eq1"" src=""https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-01.png"" style=""height: 40px;"" />
 
 Это отношение можно изменить, чтобы показать, что тепло, получаемое металлом, равно теренному веществом теренному воздействию воды: 
 
 <img alt=""Eq2"" src=""https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-02.png"" style=""height: 40px;"" />
 
 Таким образом, количество тепла (изменения) одинаково для обоих веществ. Отрицательный знак просто показывает, что qmetal и qwater противоположны в направлении потока тепла (усиление или потеря), но не указывает арифметический знак значения q (который определяется тем, получает ли рассматриваемое дело или теряет тепло, в соответствии с определением). В конкретной ситуации qmetal является отрицательным значением, и qwater является положительным значением, так как тепло переносится из металла в воду. 
 
 При использовании калориметрии для определения температуры, участвующей в химической реакции, применяются те же принципы. Количество тепла, поглощенного калориметром, часто достаточно мало, чтобы его чаще всего можно было игнорировать, а калориметр минимизирует обмен энергии с внешней средой. При экзотермической реакции в раствор в калориметре тепло, выделенное реакцией, поглощается раствор, что повышает его температуру. При возникновении эндотермической реакции необходимое тепло поглощается тепловой энергией раствор, что снижает его температуру. Изменение температуры (ΔT), а также удельным теплом (csoln) и массой раствор (msoln) могут затем использоваться для расчета количества тепла (qsoln), которое используется в любом случае. 
 
 <img alt=""Eq3"" src=""https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-03.png"" style=""height: 40px;"" />
 
  Простой калориметр, называемый калориметром чашки кофе, изготовлен из двух вложенных стаканов из полистирола, закрытых крышкой, свободной от подгонки. Калориметры чашек кофе используются для измерения температуры реакций, которые происходят в растворах (в основном водных растворах) и не требуют изменения объема. Поскольку энергия не создается и не уничтожается во время химической реакции, тепло, выделенное или потребное в реакции («система»), qrxn, плюс тепло, поглощенное или теренное раствор («окружающая среда»), qsoln, должно прибавляваться к нулю: 
 
 <img alt=""Eq4"" src=""https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-04.png"" style=""height: 40px;"" />
 
 Это означает, что количество тепла, выделенное или израсходованное в результате реакции, равно количеству тепла, поглощенного или теренного раствор: 
 
 <img alt="Eq5" src="https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-05.png" style="height: 40px;" />
 
 Калориметр чашки кофе представляет собой калориметр постоянного давления, а измеренная температура реакции эквивалентна изменению энтальпии. 
 
 <img alt="Eq6" src="https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-06.png" style="height: 40px;" />
 
 Этот текст адаптирован из <a href="https://openstax.org/books/chemistry-2e/pages/5-2-calorimetry">Openstax, Химия 2е изд., раздел 5.2: Калориметрия</a>.

Калориметрия - это метод, используемый для измерения количества тепла, задействованного в химическом или физическом процессе, или для измерения тепла, передаваемого в ...

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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

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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...

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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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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...

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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...

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

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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 ...

real-gases-effects-intermolecular-forces-molecular-volume-deriving

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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