Math Problem Statement
1 mole of an ideal gas expands isothermally and reversibly from 5 dm^3 to 10 dm^3 at 300K. Calculate q, w, ∆U, ∆H, ∆G and ∆A.
Solution
To solve this problem, we will use the properties of an isothermal, reversible expansion of an ideal gas.
Given Data
- Initial volume,
- Final volume,
- Temperature,
- Number of moles,
- For an ideal gas,
Key Formulas and Concepts
-
Isothermal Process: Since the temperature is constant, the internal energy change and the enthalpy change for an ideal gas.
-
Heat and Work:
- Heat absorbed by the system in an isothermal, reversible expansion .
- The work done by the gas in an isothermal process, as .
-
Gibbs Free Energy Change (∆G):
- For an isothermal, reversible process, .
-
Helmholtz Free Energy Change (∆A):
- For an isothermal process, .
Solution Steps
1. Calculate (Heat Absorbed)
Substitute the values:
2. Calculate (Work Done)
Since for an isothermal process:
3. Calculate (Change in Internal Energy)
For an ideal gas undergoing an isothermal process:
4. Calculate (Change in Enthalpy)
For an ideal gas in an isothermal process:
5. Calculate (Change in Gibbs Free Energy)
6. Calculate (Change in Helmholtz Free Energy)
Summary of Results
Would you like a deeper explanation of any specific step?
Here are some related questions to explore further:
- How would the calculations change if the expansion were adiabatic instead of isothermal?
- What would happen to and if the process were not reversible?
- Can you calculate the entropy change for this process?
- How does the ideal gas assumption affect these calculations?
- How would these values change if the temperature were different?
Tip: In isothermal processes for ideal gases, and are always zero since they depend only on temperature changes.
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Math Problem Analysis
Mathematical Concepts
Thermodynamics
Ideal Gas Laws
Isothermal Processes
Formulas
q = nRT ln(V2/V1)
w = -q
∆U = 0 (for isothermal process of an ideal gas)
∆H = 0 (for isothermal process of an ideal gas)
∆G = nRT ln(V2/V1)
∆A = -nRT ln(V2/V1)
Theorems
First Law of Thermodynamics
Properties of Isothermal Expansion in Ideal Gases
Suitable Grade Level
Undergraduate
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