Fundamentals of thermodynamics

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One mole of an ideal gas is heated at constant pressure from 0°C to 100°C. If the gas were expanded isothermally and reversibly at O°C from 1 atm to some other pressure P_twhat must be the final pressure if the maximum work is equal to the work involved in (a)?

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Solution

Now the work equivalent to 198.7 cal is used up in causing reversible isothermal expansion of gas at 0°C, then
$\begin{array}{l} W_{R} = - 2.303 n R T \log_{10} \frac{P_{1}}{P_{2}} \\ ∴ - 198.7 = - 2.303 \times 1 \times 1.987 \times 273 \log_{10} \frac{1}{P_{t}} \\ ∴ P_{t} = 0.694 atm \end{array}$

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Fundamentals of thermodynamics

Remember concepts with our Masterclasses.

One mole of an ideal gas is heated at constant pressure from 0°C to 100°C. If the gas were expanded isothermally and reversibly at O°C from 1 atm to some other pressure Pt what must be the final pressure if the maximum work is equal to the work involved in (a)?

Now the work equivalent to 198.7 cal is used up in causing reversible isothermal expansion of gas at 0°C, thenWR=−2.303nRTlog10⁡P1P2∴−198.7=−2.303×1×1.987×273log10⁡1Pt∴Pt=0.694atm

Ready to Test Your Skills?

free study material

One mole of an ideal gas is heated at constant pressure from 0°C to 100°C. If the gas were expanded isothermally and reversibly at O°C from 1 atm to some other pressure P_twhat must be the final pressure if the maximum work is equal to the work involved in (a)?