Two litres of an an ideal gas at pressure of $10$ atm expands isothermally to a final volume of $10$ litres conducted reversibly. How much heat is absorbed?

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Solution

$N . K . t, P v = n R T,$
or $T = \frac{P v}{n R}$
$R T = P_{1} V_{1}$ for $n = 1$
So, $R T = 2 \times 10 = 20.$
So heat absorbed is $1.20. l i t r e s$
$(\frac{10}{2}) = 32.2 J .$
$∴$ heat absorbed= $32.2 J$

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2L of an ideal gas at a pressure of 10 atm expansion isothermally into a vacuum until its total volume is 10L.

(i) How much heat is absorbed and how much work is done in the expansion?

(ii) How much heat is absorbed if this system expands against a constant external pressure of 1 atm?

(iii) How much heat is absorbed if the expansion is conducted reversibly at 298K.

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Two litres of an an ideal gas at pressure of 10 atm expands isothermally to a final volume of 10 litres conducted reversibly. How much heat is absorbed?

N.K.t,Pv=nRT,or T=PvnRRT=P1V1 for n=1So, RT=2×10=20.So heat absorbed is 1.20. litres(102)=32.2 J.∴ heat absorbed= 32.2J

Two litres of an an ideal gas at pressure of $10$ atm expands isothermally to a final volume of $10$ litres conducted reversibly. How much heat is absorbed?

$N . K . t, P v = n R T,$
or $T = \frac{P v}{n R}$
$R T = P_{1} V_{1}$ for $n = 1$
So, $R T = 2 \times 10 = 20.$
So heat absorbed is $1.20. l i t r e s$
$(\frac{10}{2}) = 32.2 J .$
$∴$ heat absorbed= $32.2 J$