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N.K. Sharma
N.K. Sharma
Asked: May 5, 2024In: IGNOU Assignments

Define molecular partition functions. Derive an expression for the translational partition function for motion along x- direction in a system.

Define molecular partition functions. Derive an expression for the translational partition function for motion along x- direction in a system.

ChemistryGENERAL PHYSICAL CHEMISTRYIGNOUMCH-013MSCCHEM
  1. Abstract Classes Power Elite Author
    Added an answer on May 5, 2024 at 3:26 pm

    Definition of Molecular Partition Functions Molecular partition function is a fundamental concept in statistical mechanics that quantifies the number of available quantum states for a molecule at a given temperature. It plays a crucial role in linking the microscopic quantum states of a system to itRead more

    Definition of Molecular Partition Functions

    Molecular partition function is a fundamental concept in statistical mechanics that quantifies the number of available quantum states for a molecule at a given temperature. It plays a crucial role in linking the microscopic quantum states of a system to its macroscopic thermodynamic properties. The partition function is a sum over all possible energy states of a system, weighted by the Boltzmann factor, \( e^{-\beta E} \), where \( \beta = \frac{1}{k_BT} \) (with \( k_B \) being the Boltzmann constant and \( T \) the temperature), and \( E \) represents the energy levels of the system.

    Derivation of the Translational Partition Function for Motion Along the X-direction

    1. Setting the Framework

    The translational partition function quantifies the number of ways a particle can be distributed in space, considering its kinetic energy due to motion. For a single particle in a one-dimensional box (along the x-axis), the energy states can be described by the quantum mechanics of a particle in a box:

    \[
    E_n = \frac{n^2 \pi^2 \hbar^2}{2mL^2}
    \]

    where:

    • \( n \) is the quantum number,
    • \( \hbar \) is the reduced Planck’s constant,
    • \( m \) is the mass of the particle,
    • \( L \) is the length of the box.

    2. Expression for the Partition Function

    The translational partition function for a particle confined to move along the x-axis in a box of length \( L \) is given by:

    \[
    q_x = \sum_{n=1}^{\infty} e^{-\beta E_n}
    \]

    Substituting the expression for \( E_n \):

    \[
    q_x = \sum_{n=1}^{\infty} e^{-\beta \frac{n^2 \pi^2 \hbar^2}{2mL^2}}
    \]

    3. Approximating the Summation

    For high temperatures or large boxes, the energy levels are closely spaced, allowing the summation to be approximated by an integral:

    \[
    q_x \approx \int_{0}^{\infty} e^{-\beta \frac{\pi^2 \hbar^2 x^2}{2mL^2}} dx
    \]

    To solve the integral, we perform a change of variables \( u = \frac{\pi \hbar x}{\sqrt{2mL^2 \beta}} \), which simplifies the integral:

    \[
    q_x \approx \frac{\sqrt{2mL^2 \beta}}{\pi \hbar} \int_{0}^{\infty} e^{-u^2} du
    \]

    The integral of \( e^{-u^2} \) from 0 to \( \infty \) is \( \frac{\sqrt{\pi}}{2} \), thus:

    \[
    q_x \approx \frac{\sqrt{2mL^2 \beta}}{\pi \hbar} \cdot \frac{\sqrt{\pi}}{2} = \frac{\sqrt{2\pi mk_BT}}{h}L
    \]

    This result shows that the translational partition function for motion along the x-direction is proportional to the length of the box and depends on the mass of the particle, the temperature, and the Boltzmann constant.

    Conclusion

    The translational partition function for motion in one dimension provides insight into how quantum mechanical properties of particles contribute to macroscopic thermodynamic quantities. It illustrates the dependency of statistical properties on physical dimensions and conditions of the system, such as temperature and size. This concept is extensible to three dimensions and forms the foundation for understanding molecular behavior in gases and other phases.

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Ramakant Sharma
Ramakant SharmaInk Innovator
Asked: May 5, 2024In: IGNOU Assignments

Explain the difference between permutation and configuration. Calculate the number of permutations and configurations possible while selecting three days out of seven days in a week.

Explain the difference between permutation and configuration. Calculate the number of permutations and configurations possible while selecting three days out of seven days in a week.

ChemistryGENERAL PHYSICAL CHEMISTRYIGNOUMCH-013MSCCHEM
  1. Abstract Classes Power Elite Author
    Added an answer on May 5, 2024 at 3:24 pm

    Understanding Permutation and Configuration 1. Definition of Permutation Permutation refers to the arrangement of a subset of items where the order of arrangement is important. It calculates the number of ways to arrange a certain number of objects from a larger set, considering the sequence in whicRead more

    Understanding Permutation and Configuration

    1. Definition of Permutation

    Permutation refers to the arrangement of a subset of items where the order of arrangement is important. It calculates the number of ways to arrange a certain number of objects from a larger set, considering the sequence in which they appear. For instance, arranging the letters A, B, and C would yield different results such as ABC, ACB, BAC, BCA, CAB, and CBA β€” each arrangement being unique due to the order of the letters.

    2. Definition of Configuration (Combination)

    Configuration, often referred to as combination, involves selecting items from a larger set where the order of selection does not matter. It’s used to calculate the number of ways to choose a subset where the sequence is irrelevant. For example, selecting 2 letters from A, B, and C would result in combinations like AB, AC, and BC, where AB is considered the same as BA.

    Differences Between Permutation and Configuration

    • Order Importance: In permutations, the order of items is important, while in configurations, the order is not considered.
    • Formulae: The formula for permutations of \(r\) items from \(n\) is \(P(n, r) = \frac{n!}{(n-r)!}\), and the formula for configurations of \(r\) items from \(n\) is \(C(n, r) = \frac{n!}{r!(n-r)!}\).

    Calculation for Selecting Three Days Out of Seven

    1. Permutation Calculation

    To find the number of permutations of selecting 3 days out of 7 (considering the order in which they are selected matters), we use the permutation formula:

    \[
    P(7, 3) = \frac{7!}{(7-3)!} = \frac{7 \times 6 \times 5 \times 4!}{4!} = 7 \times 6 \times 5 = 210
    \]

    There are 210 different ways to select and arrange 3 days from a week.

    2. Configuration Calculation

    To find the number of configurations (combinations) of selecting 3 days out of 7 (where the order does not matter), we use the combination formula:

    \[
    C(7, 3) = \frac{7!}{3!(7-3)!} = \frac{7 \times 6 \times 5}{3 \times 2 \times 1} = 35
    \]

    There are 35 ways to select 3 days from a week without considering the order of the days.

    Conclusion

    The choice between permutation and configuration depends on whether the order of items is important in a given context. Permutations are used when the sequence affects the outcome, while configurations are appropriate for scenarios where only the choice of items matters, not the sequence. In the example of selecting days from a week, the substantial difference in results between permutations and configurations (210 vs. 35) highlights the impact of considering order.

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N.K. Sharma
N.K. Sharma
Asked: May 5, 2024In: IGNOU Assignments

Define the term β€˜chemical potential’ and discuss the effect of temperature on chemical potential.

Define the term β€˜chemical potential’ and discuss the effect of temperature on chemical potential.

ChemistryGENERAL PHYSICAL CHEMISTRYIGNOUMCH-013MSCCHEM
  1. Abstract Classes Power Elite Author
    Added an answer on May 5, 2024 at 3:21 pm

    Definition of Chemical Potential Chemical potential is a thermodynamic quantity that represents the potential energy change of a system when an infinitesimal amount of substance is added to the system, keeping temperature and pressure constant. It can be thought of as the energy change per unit addiRead more

    Definition of Chemical Potential

    Chemical potential is a thermodynamic quantity that represents the potential energy change of a system when an infinitesimal amount of substance is added to the system, keeping temperature and pressure constant. It can be thought of as the energy change per unit addition or removal of a particle from a system. Essentially, it indicates how the Gibbs free energy of the system changes as the amount of substance changes, making it a crucial factor in understanding chemical reactions and phase changes.

    Effects of Temperature on Chemical Potential

    1. Fundamental Relationship

    The chemical potential (\(\mu\)) of a substance is not only a function of its concentration but also of temperature and pressure. The relationship between chemical potential and temperature at constant pressure can be derived from the fundamental thermodynamic equations:

    \[
    \left(\frac{\partial \mu}{\partial T}\right)_P = -S
    \]

    where \(S\) is the molar entropy of the substance. This equation implies that the chemical potential of a substance decreases with an increase in temperature at constant pressure, provided the entropy (\(S\)) is positive, which is generally the case.

    2. Practical Implications

    • Influence on Reaction Direction: As temperature increases, the chemical potentials of the reactants and products change, influencing the direction of the chemical reaction. According to Le Chatelier’s principle, if a reaction produces heat (exothermic), increasing the temperature will increase the chemical potentials of the products more than the reactants, potentially driving the reaction in the reverse direction.
    • Impact on Phase Transitions: The chemical potentials of different phases (solid, liquid, gas) of a substance also depend on temperature. For example, the melting of ice into water as temperature increases is a result of the chemical potential of water becoming more favorable (lower) than that of ice at temperatures above 0Β°C.

    3. Dependence on Entropy

    The change in chemical potential with temperature is directly tied to the entropy of the substance. A higher entropy value indicates a greater decrease in chemical potential with temperature. This relationship underlines the intrinsic connection between the disorder within a system and its energetic favorability under varying thermal conditions.

    Conclusion

    Understanding the chemical potential and its temperature dependence is essential in the fields of chemical thermodynamics and reaction engineering. It provides insights into how substances behave under different thermal conditions, influencing everything from industrial synthesis to environmental processes. The decrease in chemical potential with temperature, due to positive entropy, plays a critical role in determining the direction of chemical reactions and the stability of various phases in a substance.

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Bhulu Aich
Bhulu AichExclusive Author
Asked: May 5, 2024In: IGNOU Assignments

If the enthalpy and entropy changes are not affected by the change in temperature calculate the temperature at which the system will attain equilibrium.

If the enthalpy and entropy changes are not affected by the change in temperature calculate the temperature at which the system will attain equilibrium.

ChemistryGENERAL PHYSICAL CHEMISTRYIGNOUMCH-013MSCCHEM
  1. Abstract Classes Power Elite Author
    Added an answer on May 5, 2024 at 3:19 pm

    1. Introduction to Gibbs Free Energy Gibbs free energy (G) is a thermodynamic potential that helps predict the direction of chemical processes and reactions. The change in Gibbs free energy (\(\Delta G\)) indicates the spontaneity of a process: if \(\Delta G\) is negative, the process is spontaneousRead more

    1. Introduction to Gibbs Free Energy

    Gibbs free energy (G) is a thermodynamic potential that helps predict the direction of chemical processes and reactions. The change in Gibbs free energy (\(\Delta G\)) indicates the spontaneity of a process: if \(\Delta G\) is negative, the process is spontaneous; if positive, it is non-spontaneous. The equation governing Gibbs free energy is:

    \[
    \Delta G = \Delta H – T\Delta S
    \]

    Here, \(\Delta H\) is the change in enthalpy, \(T\) is the temperature in Kelvin, and \(\Delta S\) is the change in entropy. This formula is crucial in determining the energy changes under constant pressure and temperature conditions.

    2. Understanding Enthalpy (\(\Delta H\)) and Entropy (\(\Delta S\))

    Enthalpy (\(\Delta H\)) measures the total energy of a thermodynamic system, incorporating both the internal energy and the energy due to pressure and volume, expressed in joules per mole (J/mol). A positive \(\Delta H\) signifies heat absorption by the system (endothermic process), while a negative \(\Delta H\) signifies heat release (exothermic process).

    Entropy (\(\Delta S\)), on the other hand, is a measure of the system’s disorder or randomness, expressed in joules per mole per Kelvin (J/K/mol). An increase in entropy (\(\Delta S > 0\)) suggests a transition to more disorder, whereas a decrease (\(\Delta S < 0\)) indicates a transition to less disorder.

    3. Spontaneity and Temperature Dependence

    The spontaneity of a process is determined by \(\Delta G\). At constant temperature and pressure, if \(\Delta G < 0\), the process is spontaneous. The influence of \(\Delta G\) is dependent on \(\Delta H\), \(\Delta S\), and the temperature \(T\). Temperature significantly affects spontaneity by altering the contribution of entropy to the Gibbs free energy.

    If \(\Delta H\) and \(\Delta S\) are constant and unaffected by temperature changes, the equation \(\Delta G = \Delta H – T\Delta S\) can be directly used to predict how temperature influences the spontaneity of the process.

    4. Calculation of Equilibrium Temperature

    To find the temperature at which the system is at equilibrium (\(\Delta G = 0\)), we can rearrange the Gibbs free energy equation:

    \[
    0 = \Delta H – T_{eq}\Delta S
    \]

    Solving for \(T_{eq}\) (equilibrium temperature):

    \[
    T_{eq} = \frac{\Delta H}{\Delta S}
    \]

    Given that \(\Delta H = 52 \text{ kJ mol}^{-1}\) and \(\Delta S = 165 \text{ JK}^{-1} \text{ mol}^{-1}\), we convert \(\Delta H\) to joules:

    \[
    \Delta H = 52000 \text{ J mol}^{-1}
    \]

    Substituting these values into the equation for \(T_{eq}\):

    \[
    T_{eq} = \frac{52000 \text{ J mol}^{-1}}{165 \text{ JK}^{-1} \text{ mol}^{-1}}
    \]

    \[
    T_{eq} = 315.15 \text{ K}
    \]

    This calculation implies that at a temperature of 315.15 K, the system reaches a state of equilibrium where the process is neither spontaneous nor non-spontaneous.

    Conclusion

    The analysis of Gibbs free energy provides critical insights into the temperature dependence of chemical reactions and processes. By evaluating changes in enthalpy and entropy, one can determine not only the spontaneity of a process at a given temperature but also predict the temperature at which the system will achieve equilibrium. For the given changes in enthalpy and entropy, the calculated equilibrium temperature is 315.15 K. At this temperature, the changes in enthalpy and entropy balance each other out, resulting in zero change in Gibbs free energy, indicating a state of equilibrium. This understanding is crucial in chemical thermodynamics for designing processes that require precise control over temperature to achieve desired outcomes.

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Bhulu Aich
Bhulu AichExclusive Author
Asked: May 5, 2024In: IGNOU Assignments

An isothermal and isobaric process is accompanied by changes in enthalpy and entropy as 52 kJ mol-1 and 165 JK-1 mol-1 , respectively. Predict whether the process be spontaneous at 400K.

An isothermal and isobaric process is accompanied by changes in enthalpy and entropy as Ξ”H = 52 kJ mol^-1 and Ξ”S = 165 JK^-1 mol^-1, respectively. Predict whether the process be spontaneous at 400K.

ChemistryGENERAL PHYSICAL CHEMISTRYIGNOUMCH-013MSCCHEM
  1. Abstract Classes Power Elite Author
    Added an answer on May 5, 2024 at 3:12 pm

    To determine if the process is spontaneous at a given temperature, we can use the Gibbs free energy change (\(\Delta G\)), which is related to the changes in enthalpy (\(\Delta H\)) and entropy (\(\Delta S\)) through the equation: \[ \Delta G = \Delta H - T\Delta S \] Where: - \(\Delta H\) is the chRead more

    To determine if the process is spontaneous at a given temperature, we can use the Gibbs free energy change (\(\Delta G\)), which is related to the changes in enthalpy (\(\Delta H\)) and entropy (\(\Delta S\)) through the equation:

    \[
    \Delta G = \Delta H – T\Delta S
    \]

    Where:
    – \(\Delta H\) is the change in enthalpy,
    – \(T\) is the temperature in Kelvin,
    – \(\Delta S\) is the change in entropy.

    Given:
    – \(\Delta H = 52 \text{ kJ mol}^{-1} = 52000 \text{ J mol}^{-1}\) (since 1 kJ = 1000 J)
    – \(\Delta S = 165 \text{ JK}^{-1} \text{ mol}^{-1}\)
    – \(T = 400 \text{ K}\)

    Plugging these values into the equation for \(\Delta G\):

    \[
    \Delta G = 52000 \text{ J mol}^{-1} – 400 \text{ K} \times 165 \text{ JK}^{-1} \text{ mol}^{-1}
    \]

    We can calculate \(\Delta G\) as follows:

    \[
    \Delta G = 52000 \text{ J mol}^{-1} – 66000 \text{ J mol}^{-1}
    \]

    \[
    \Delta G = -14000 \text{ J mol}^{-1}
    \]

    Since \(\Delta G\) is negative, the process is spontaneous at 400 K.

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