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The change in free energy accompanied by the isothermal reversible expansion of 1 mol of an ideal gas when it doubles its volume is ΔG1 The change in free energy accompanied by sudden isothermal irreversible doubling volume of 1 mole of the same gas is ΔG2 Ratio of ΔG1 and ΔG2
  • a)
    1                                                           
  • b)
    1/2                            
  • c)
    – 1                                                       
  • d)
       -1/2
Correct answer is option 'A'. Can you explain this answer?
Verified Answer
The change in free energy accompanied by the isothermal reversible exp...
∆G=nR∆T
Therefore, ∆G1/∆G2=1
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Most Upvoted Answer
The change in free energy accompanied by the isothermal reversible exp...
The change in free energy (ΔG) for an isothermal reversible expansion of an ideal gas can be calculated using the equation:

ΔG = -RT ln(V2/V1)

Where:
ΔG = change in free energy
R = gas constant (8.314 J/mol·K)
T = temperature (in Kelvin)
V2 = final volume
V1 = initial volume

In this case, the gas is doubling its volume, so V2/V1 = 2.

Substituting the values into the equation, we get:

ΔG = -RT ln(2)

Note: The natural logarithm of 2 is approximately 0.693.

Therefore, the change in free energy accompanied by the isothermal reversible expansion of 1 mol of an ideal gas when it doubles its volume is approximately -0.693RT.
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Community Answer
The change in free energy accompanied by the isothermal reversible exp...
∆G=nR∆T
Therefore, ∆G1/∆G2=1
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The change in free energy accompanied by the isothermal reversible expansion of 1 mol of an ideal gas when it doubles its volume is ΔG1 The change in free energy accompanied by sudden isothermal irreversible doubling volume of 1 mole of the same gas is ΔG2 Ratio of ΔG1 and ΔG2a)1b)1/2c)– 1 d)-1/2Correct answer is option 'A'. Can you explain this answer?
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