For an ideal gas, the work of reversible expansion under isothermal conditions can be calculated by using the expression $w = - nRT$ in $V_{f} / V_{i}$
A sample containing 1.0 mol of an ideal gas is expanded isothermally and reversibly to ten times of its original volume, in two separate experiments. The expansion is carried out at 300 K and at 600 K respectively, Choose the correct option.

see full answer

High-Paying Jobs That Even AI Can’t Replace — Through JEE/NEET

🎯 Hear from the experts why preparing for JEE/NEET today sets you up for future-proof, high-income careers tomorrow.

An Intiative by Sri Chaitanya

$ΔU = 0$ in both cases.

Work done at 600 K is 20 times the work done at 300 K

Work done at 300 K is twice the work done at 600 K.

Work done at 600 K is twice the work done at 300 K

answer is C, D.

(Unlock A.I Detailed Solution for FREE)

JEE

NEET

Foundation JEE

Foundation NEET

CBSE

Detailed Solution

For reversible isothermal change,

$q = - w = nRT In$ $\frac{V_{f}}{V_{i}} = 2.303 nRT \log \frac{V_{f}}{V_{i}}$

$\frac{W_{600 K}}{W_{300 K}} = \frac{1 \times R \times 600 K In \frac{10}{1}}{1 \times R \times 300 K In \frac{10}{1}} = \frac{600}{300} = 2$

$∆ U = 0$ for ideal gas isothermal growth.
Since the temperature stays constant, the internal energy remains constant.
Consequently, $∆ U = 0$ .

Watch 3-min video & get full concept clarity

Ready to Test Your Skills?

Check your Performance Today with our Free Mock Test used by Toppers!

Take Free Test