How much energy must be transferred as heat for a reversible isothermal expansion J. of an ideal gas at 132°C if the entropy of the gas increases by 46.0 K
How much energy must be transferred as heat for a reversible isothermal expansion J. of an ideal gas at 132°C if the entropy of the gas increases by 46.0 K
College Physics
11th Edition
ISBN:9781305952300
Author:Raymond A. Serway, Chris Vuille
Publisher:Raymond A. Serway, Chris Vuille
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![**Question:**
How much energy must be transferred as heat for a reversible isothermal expansion of an ideal gas at 132°C if the entropy of the gas increases by 46.0 J/K?
**Explanation:**
In an isothermal process, the temperature remains constant. To find the energy transferred as heat (Q), when the entropy (ΔS) increases, we use the relationship for reversible processes:
\[ Q = T \times \Delta S \]
Where:
- \( T \) is the absolute temperature in Kelvin (K).
- \( \Delta S \) is the change in entropy.
Convert the temperature from °C to K:
\[ T(K) = 132 + 273.15 = 405.15 \, K \]
Given:
- \( \Delta S = 46.0 \, J/K \)
Substituting the values:
\[ Q = 405.15 \, K \times 46.0 \, J/K \]
Calculate to find the energy transferred as heat.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1df78ed7-7bf9-40d0-9ea6-9fdf014e5eeb%2Fefe040fe-90cc-4b42-9c5c-aebe3ed47284%2Fam0i81_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Question:**
How much energy must be transferred as heat for a reversible isothermal expansion of an ideal gas at 132°C if the entropy of the gas increases by 46.0 J/K?
**Explanation:**
In an isothermal process, the temperature remains constant. To find the energy transferred as heat (Q), when the entropy (ΔS) increases, we use the relationship for reversible processes:
\[ Q = T \times \Delta S \]
Where:
- \( T \) is the absolute temperature in Kelvin (K).
- \( \Delta S \) is the change in entropy.
Convert the temperature from °C to K:
\[ T(K) = 132 + 273.15 = 405.15 \, K \]
Given:
- \( \Delta S = 46.0 \, J/K \)
Substituting the values:
\[ Q = 405.15 \, K \times 46.0 \, J/K \]
Calculate to find the energy transferred as heat.
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