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Bomb calorimeter is used to determine the heat of reaction at (1) constant pressure (2) constant volume (3) \(298 \mathrm{~K}\) (4) \(373 \mathrm{~K}\)

Short Answer

Expert verified
The bomb calorimeter determines the heat of reaction at constant volume.

Step by step solution

01

Identify the features of a bomb calorimeter

A bomb calorimeter is a type of constant-volume calorimeter used in measuring the heat of combustion of a particular reaction. The key feature to remember is its constant volume.
02

Analyze provided options

Given the options: (1) constant pressure, (2) constant volume, (3) 298 K, and (4) 373 K. Recall that a bomb calorimeter operates at constant volume.
03

Choose the correct answer

Since the bomb calorimeter works at constant volume, the correct option is (2) constant volume.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Heat of Reaction
In thermodynamics, a heat of reaction is the heat change that occurs when a specified chemical reaction takes place. It can either be exothermic (releasing heat) or endothermic (absorbing heat). The heat of reaction is a crucial concept because it tells us about the energy change during a chemical process.
Understanding this helps in predicting reaction behavior and calculating energy requirements or releases in industrial processes.
The heat of reaction is typically measured in Joules (J) or calories (cal), and is often determined using a calorimeter.
  • In an exothermic reaction, the surroundings get warmer.
  • In an endothermic reaction, the surroundings get cooler.

The specific value of the heat of reaction for a process can be determined using devices such as a bomb calorimeter, which measures the heat at constant volume.
Constant Volume
A key feature of a bomb calorimeter is that it operates at constant volume.
This means that no work is done by or on the system in terms of expansion or compression since the volume does not change.
  • No volume change leads to precise measurement of the heat involved.
  • It makes the calculations simpler because the only concern is the internal energy change.
During the reaction, the calorimeter absorbs the heat released or supplies the heat absorbed, ensuring the measurement is accurate by maintaining a constant volume.
Chemical Thermodynamics
Chemical thermodynamics explores the energy changes during chemical reactions and how these changes affect system properties.
It provides a framework to understand how energy is transferred and transformed.
In the context of a bomb calorimeter:
  • The system remains isolated from its surroundings.
  • The energy changes are confined to the chemical reaction inside the apparatus.
Basic principles such as the first law of thermodynamics (energy conservation) apply. This principle asserts that the total energy of an isolated system is constant, providing foundational knowledge for calculating reaction heats and understanding how energy is conserved in chemical processes.

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Most popular questions from this chapter

\(C_{\text {(dianemd) }}+\mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{CO}_{2}(\mathrm{~g}) ; \Delta H=395 \mathrm{~kJ}\) \(C_{\text {(Braphite) }}+\mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{CO}_{2}(\mathrm{~g}) ; \Delta / I=-393.5 \mathrm{~kJ}\) The \(\Delta / /\) when diamond is formed from graphite (1) \(-1.5 \mathrm{~kJ}\) \((2)+1.5 \mathrm{~kJ}\) (3) \(+3.0 \mathrm{k} \mathrm{J}\) (4) \(-3.0 \mathrm{~kJ}\)

From the reaction \(P_{\text {white }} \longrightarrow P_{\text {red }} ; \Delta H=18.4 \mathrm{~kJ}\) follows that (1) Red \(\mathrm{P}\) is readily formed from white \(\mathrm{P}\). (2) White \(\mathrm{P}\) is readily formed from \(\mathrm{red} \mathrm{P}\). (3) White P cannot be converted to red \(P\). (4) Whitc P can be converted into red \(\mathrm{P}\) and red \(\mathrm{P}\) is more stable.

The temperature of \(5 \mathrm{~mL}\) of a strong acid increases by \(5^{\circ} \mathrm{C}\) when \(5 \mathrm{~mL}\) of a strong base is added to it. If \(10 \mathrm{~mL}\) of cach are mixed, temperature should increase by (1) \(5^{\circ} \mathrm{C}\) (2) \(10^{\circ} \mathrm{C}\) (3) \(15^{\circ} \mathrm{C}\) (4) cannot be known

The law of conscrvation of energy states that (1) the internal energy of a system is constant (2) the heat content of the system is constant (3) cnergy is neither created nor destroyed (4) there is an equivalence between energy and mass

The falsc statement among the following is (1) Vapourisation of liquid is accompaniod by incrcase in cnthalpy (2) The difference betwcen \(\Delta H\) and \(\Delta U\) is cqual to \(3 / 2 \mathrm{R}\). (3) It is the gcneral principle that the less encrgy a system contains, it is more stable. (4) The sum of the internal cnergy and work form of encrgy is called enthalpy.

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