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Work Done in Isothermal Reversible Process

Consider an i...

Question

Consider an ideal gas that occupies 2.50 $d m^{3}$ at a pressure of 3 bar. If the gas is compressed isothermally at a constant pressure $P_{e x t}$ , so that the final volume becomes 0.5 $d m^{3}$ . Calculate the value of $P_{e x t}$ and the work done respectively.
Given: $1 b a r . L$ = 100 $J$

20 b a r

and

1000 J

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15 b a r

and

3000 J

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30 b a r

and

1500 J

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10 b a r

and

3750 J

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Solution

The correct option is B $15 b a r$ and $3000 J$
For isothermal process of an ideal gas,
we can use, PV = constant.
So, $P_{1} V_{1} = P_{2} V_{2}$
where $P_{1}$ = 3 bar
$V_{1} = 2.5 d m^{3}$
$V_{2} = 0.5 d m^{3}$
using these values to find $P_{2}$ ,
$P_{2}$ = 15 bar
work done for irreversible process is
w = $- P_{e x t} Δ V$
w = $- 15 \times (0.5 - 2.5$ ) $b a r . d m^{3}$
$= 3000 J$

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Work Done in Isothermal Reversible Process

Standard XII Chemistry

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Consider an ideal gas that occupies 2.50 dm3 at a pressure of 3 bar. If the gas is compressed isothermally at a constant pressure Pext, so that the final volume becomes 0.5 dm3. Calculate the value of Pext and the work done respectively. Given: 1 bar.L = 100 J

The correct option is B 15 bar and 3000 JFor isothermal process of an ideal gas, we can use, PV = constant. So, P1V1=P2V2 where P1 = 3 bar V1=2.5 dm3 V2=0.5 dm3 using these values to find P2, P2 = 15 bar work done for irreversible process is w = −PextΔV w = −15×(0.5−2.5) bar.dm3 =3000 J

Consider an ideal gas that occupies 2.50 $d m^{3}$ at a pressure of 3 bar. If the gas is compressed isothermally at a constant pressure $P_{e x t}$ , so that the final volume becomes 0.5 $d m^{3}$ . Calculate the value of $P_{e x t}$ and the work done respectively.
Given: $1 b a r . L$ = 100 $J$