Question

5 mole of an ideal gas expands isothermally and irreversibly from a pressure of 10 atm to 1 atm against a constant external pressure of 1 atm. find the wirr at 300 k :- (1) –15.921 kj (2) –11.224 kj (3) –110.83 kj (4) none of these

Answer 1

Answer : The correct option is, (3) -11.224 KJ

Solution :

The formula used for isothermal irreversible ideal gas is,

$w=-P_{2}(V_{2}-V_{1})$

or we can write as,

$w=-nRT(1-\frac{P_2}{P_1})$

where,

w = work done

n = number of mole of gas = 5 moles

R = gas constant = 8.314 J/Kmole

T = temperature of gas = 300 K

$P_1$ = initial pressure of gas = 1 atm

$P_2$ = final pressure of gas = 10 atm

Now put all the given values in the above formula, we get the work done.

$w=-(5mole)\times (8.314J/moleK)\times (300K)[(1-\frac{1atm}{10atm})]=-11223.9J=-11.224KJ$

Therefore, the work done is, -11.224 KJ

Answer 2

Answer:

option 2 is correct. -11.224 kj