For $1 \text{ mole}$ of an ideal gas expanding isothermally from $1 \text{ L}$ to $10 \text{ L}$ at $300 \text{ K}$,the value of $\Delta U$ is: $(R = 2 \text{ cal mol}^{-1} \text{ K}^{-1})$
- A$163.7 \text{ cal}$
- B$0 \text{ cal}$
- C$1381.1 \text{ cal}$
- D$9 \text{ L-atm}$
Explore More
Similar Questions
Five moles of an ideal gas at $1 \ bar$ and $298 \ K$ is expanded into vacuum to double the volume. The work done is :-
What is the constant external pressure of an ideal gas when expanded from $2 \times 10^{-2} \ m^3$ to $3 \times 10^{-2} \ m^3$,if the work done by the gas is $-5.09 \ kJ$?
The pressure of a gas is $100 \ kPa$. If it is compressed from $1 \ m^{3}$ to $10 \ dm^{3}$,find the work done. (in $J$)
At a definite temperature,for which of the following reactions will the value of $(\Delta E - \Delta H)$ be maximum?
Difficult
View SolutionThe difference between $C_p$ and $C_v$ can be derived using the empirical relation $H = U + PV$. Calculate the difference between $C_p$ and $C_v$ for $10$ moles of an ideal gas.
Easy
View SolutionVedclass Products
For Students
Vedclass Test Series
Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.
Start Free TrialFor Teachers
Exam Paper Generator
Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.
Try FreeFor Institutes
Online Exam Module
Live online exams with unlimited students, 360° analytics & white-label branding.
See Demo