Suppose 135 moles of a monatomic ideal gas undergo an isothermal expansion from

Question

Suppose 135 moles of a monatomic ideal gas undergo an isothermal expansion from 1.00 m3 to 4.00 m3, as shown in the figure(Figure 1) .

Part A:

What is the temperature at the beginning of this process?

Ti=_________K

Part B:

What is the temperature at the end of this process?

Tf=_________K

Part C:

How much work is done by the gas during this expansion?

W=________kJ

Suppose 135 moles of a monatomic ideal gas undergo an isothermal expansion from 1.00 m3 to 4.00 m3, as shown in the figure(Figure 1). What is the temperature at the beginning of this process? What is the temperature at the end of this process? How much work is done by the gas during this expansion?

Explanation / Answer

Initial pressure P = 400 * 10^ 3 Pa Initial volume V = 1 m ^ 3 No.of moles n = 135 we know PV =nRT from this initial temperature T = PV / nR where R = gas ocntsant = 8.314 J / mol K plug the values we get T = 356.382 K This is an isothermal process.So, final temperature T ' =356.382 K work done W = nRT ln( V ' / V ) where V ' = final volume = 4 m ^ 3 plug the values we get W = 135* 8.314* 356.382 ln ( 4 /1 ) =554517.18019 J Since temperature is not changed in isothermal process

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