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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Similar questions

Q. Consider an ideal gas that occupies

2.50 d m^{3}

at a pressure of 3.00 bar. If the gas is compressed isothermally at a constant pressure

p_{e x t},

so that the final volume is

0.500 d m^{3},

calculate the smallest possible value of

p_{e x t}

and the work done using

p_{e x t}

Consider an ideal gas that occupies $2.50 d m^{3}$ at a pressure of 3.00 bar. If the gas is compressed isothermally at a constant pressure $p_{e x t},$ so that the final volume is $0.500 d m^{3},$ calculate the smallest possible value of $p_{e x t}$ and the work done using $p_{e x t}$ .