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Which of the following statements is correct for the spontaneous adsorption of a gas:
- a)ΔS is negative and therefore, ΔH should be highly positive
- b)ΔS is negative and therefore, ΔH should be highly negative
- c)ΔS is positive and therefore, ΔH should be negative
- d)ΔS is positive and therefore, ΔH should be also be highly negative
Correct answer is option 'B'. Can you explain this answer?
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Explanation:
In the context of adsorption, the spontaneity of the process can be determined by the values of entropy (S) and enthalpy (H). The correct statement is option 'B': S is negative and therefore, H should be highly negative. This can be explained in detail as follows:
1. Entropy (S):
Entropy is a measure of the disorder or randomness of a system. If the gas molecules are freely moving in the gas phase, their entropy is generally higher compared to when they are adsorbed onto a solid surface. The gas molecules lose their freedom of movement and become more ordered when they adhere to the surface.
2. Enthalpy (H):
Enthalpy is a measure of the heat energy of a system. The enthalpy change during adsorption can be exothermic (negative) or endothermic (positive), depending on the nature of the adsorbent and the gas molecules.
3. Spontaneous adsorption:
For a process to be spontaneous, the overall change in Gibbs free energy (ΔG) should be negative. The Gibbs free energy change (ΔG) is related to entropy (S) and enthalpy (H) through the equation:
ΔG = ΔH - TΔS
where T is the temperature in Kelvin.
4. Relation between S, H, and spontaneity:
- If S is negative, it means that the system becomes less disordered upon adsorption. In this case, for the process to be spontaneous, the value of ΔH (enthalpy change) should be highly negative (exothermic).
- If S is positive, it means that the system becomes more disordered upon adsorption. In this case, for the process to be spontaneous, the value of ΔH (enthalpy change) should be negative (exothermic), but not necessarily highly negative.
5. Justification for option 'B':
The correct statement in the given options is option 'B'. If S is negative, as explained in point 4, the value of ΔH (enthalpy change) should be highly negative (exothermic) for the adsorption process to be spontaneous. This is because the negative value of ΔH offsets the negative value of -TΔS, resulting in a negative ΔG.
Therefore, option 'B' is correct: S is negative and therefore, H should be highly negative for spontaneous adsorption of a gas.
Note: The other options are incorrect because they do not follow the relationship between S, H, and spontaneity explained above.
In the context of adsorption, the spontaneity of the process can be determined by the values of entropy (S) and enthalpy (H). The correct statement is option 'B': S is negative and therefore, H should be highly negative. This can be explained in detail as follows:
1. Entropy (S):
Entropy is a measure of the disorder or randomness of a system. If the gas molecules are freely moving in the gas phase, their entropy is generally higher compared to when they are adsorbed onto a solid surface. The gas molecules lose their freedom of movement and become more ordered when they adhere to the surface.
2. Enthalpy (H):
Enthalpy is a measure of the heat energy of a system. The enthalpy change during adsorption can be exothermic (negative) or endothermic (positive), depending on the nature of the adsorbent and the gas molecules.
3. Spontaneous adsorption:
For a process to be spontaneous, the overall change in Gibbs free energy (ΔG) should be negative. The Gibbs free energy change (ΔG) is related to entropy (S) and enthalpy (H) through the equation:
ΔG = ΔH - TΔS
where T is the temperature in Kelvin.
4. Relation between S, H, and spontaneity:
- If S is negative, it means that the system becomes less disordered upon adsorption. In this case, for the process to be spontaneous, the value of ΔH (enthalpy change) should be highly negative (exothermic).
- If S is positive, it means that the system becomes more disordered upon adsorption. In this case, for the process to be spontaneous, the value of ΔH (enthalpy change) should be negative (exothermic), but not necessarily highly negative.
5. Justification for option 'B':
The correct statement in the given options is option 'B'. If S is negative, as explained in point 4, the value of ΔH (enthalpy change) should be highly negative (exothermic) for the adsorption process to be spontaneous. This is because the negative value of ΔH offsets the negative value of -TΔS, resulting in a negative ΔG.
Therefore, option 'B' is correct: S is negative and therefore, H should be highly negative for spontaneous adsorption of a gas.
Note: The other options are incorrect because they do not follow the relationship between S, H, and spontaneity explained above.
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Which of the following statements is correct for the spontaneous adsorption of a gas:a)ΔS is negative and therefore, ΔH should be highly positiveb)ΔS is negative and therefore, ΔH should be highly negativec)ΔS is positive and therefore, ΔH should be negatived)ΔS is positive and therefore, ΔH should be also be highly negativeCorrect answer is option 'B'. Can you explain this answer?
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