
(a)
Interpretation:
An expression for the difference between the change in enthalpy and the change in internal energy for a gas phase process has to be determined assuming all the species behave as perfect gas.
Concept introduction:
Kirchhoff’s law:
This law states that the variation of change of enthalpy of a reaction with temperature at constant pressure is equal to the change in specific heat capacity at constant temperature of the system.
Internal energy:
Internal energy of a system is the total energy contained in the system. It keeps an account for the loss and gain of energy of the system due to changes in internal state. It is dependent on temperature and pressure.
It is denoted as
From 1st law of
Where,
Enthalpy:
Enthalpy is a property of a thermodynamic system that is equal to the sum of the internal energy of the system and the product of pressure and volume. For a closed system where transfer of matter between system and surroundings is prohibited, for the processes that occur at constant pressure, the heat absorbed or released equals to the change in enthalpy.
It is denoted as
From thermodynamics,
Where,
Specific heat capacity at constant pressure:
Specific heat capacity at constant pressure can be defined as the amount of energy required to increase the temperature of a substance by
It is denoted as
Heat capacity at constant volume:
Specific heat capacity at constant volume is defined as the amount of heat required to increase the temperature by
It is denoted as
(a)

Explanation of Solution
Given that for perfect gas
Applying the Kirchhoff’s law,
Thus by integration of both,
Thus the difference is,
The difference between the change in enthalpy and the change in internal energy for a gas phase process is
(b)
Interpretation:
For ionization
Concept introduction:
Ionization enthalpy:
Ionization enthalpy is the energy required to remove an electron from a gaseous atom or ion
Ionization energy:
Ionization energy is defined as the minimum amount of energy required to remove the most loosely bound valence electron of an isolated neutral gas molecule.
Kirchhoff’s law:
This law states that the variation of change of enthalpy of a reaction with temperature at constant pressure is equal to the change in specific heat capacity at constant temperature of the system.
(b)

Explanation of Solution
According to Kirchhoff’s law,
Applying integration,
Thus it has been established that,
(c)
Interpretation:
Difference between the standard enthalpy of ionization of
Concept introduction:
Ionization enthalpy:
Ionization enthalpy is the energy required to remove an electron from a gaseous atom or ion
(c)

Answer to Problem 2.10PR
The difference between the standard enthalpy of ionization of
Explanation of Solution
From part (b) it can be concluded that,
According to the question, difference between the standard enthalpy of ionization of
Given that,
Hence,
Hence the difference between the standard enthalpy of ionization of
(d)
Interpretation:
For electron gain
Concept introduction:
Electron gain enthalpy:
Electron gain enthalpy can be defined as the amount of energy released when an electron is added to an isolated gaseous atom for electron gain enthalpy the sign convention is negative.
Electron affinity can be defined as the change in energy of a neutral atom in the gaseous phase when an electron is added to the atom to form the negative ion.
Kirchhoff’s law:
This law states that the variation of change of enthalpy of a reaction with temperature at constant pressure is equal to the change in specific heat capacity at constant temperature of the system.
(d)

Explanation of Solution
According to Kirchhoff’s law,
Applying integration,
Thus it has been established that,
(e)
Interpretation:
Difference between the standard electron gain enthalpy of
Concept introduction:
Electron gain enthalpy:
Electron gain enthalpy can be defined as the amount of energy released when an electron is added to an isolated gaseous atom for electron gain enthalpy the sign convention is negative.
(e)

Answer to Problem 2.10PR
The difference between the standard electron gain enthalpy of
Explanation of Solution
From the part (d) it can be concluded that,
Now according to the question the difference between the standard electron gain enthalpy of
Given that,
Hence,
Hence the difference between the standard electron gain enthalpy of
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Chapter 2 Solutions
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