When $1 \ mole$ of gas is heated at constant volume and heat supplied is $500 \ J$,then which of the following is correct?
- A$\Delta U = -0.5 \ J, q = -500 \ J$
- B$q = -500 \ J, \Delta U = 0$
- C$q = 500 \ J, w = 0$
- D$w = 500 \ J, \Delta U = 0$
Explore More
Similar Questions
$A$ gas is allowed to expand in an insulated container against a constant external pressure of $10 \ atm$ from an initial volume $4.2 \ L$ to $5.2 \ L$. The change in internal energy $\Delta E$ of the gas will be $:-$
Easy
View SolutionJoule-Thomson expansion is:
Easy
View SolutionExplain the relationship between the change in heat at constant pressure and constant volume.
Difficult
View Solution$q$ and $w$ are both ....... functions and $q + w$ is a ....... function.
Easy
View SolutionThe correct option for free expansion of an ideal gas under adiabatic condition is
MediumNEET 2020
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