When $1 \ mole$ of gas is heated at constant volume,the temperature rises from $273 \ K$ to $546 \ K$. If heat supplied to the gas is $x \ J$,then find the correct statement from the following.
- A$Q = \Delta U = x \ J, W = 0$
- B$Q = W = x \ J, \Delta V = 0$
- C$\Delta V = 0, Q = W = -x \ J$
- D$Q = -W = x \ J, \Delta V = 0$
Explore More
Similar Questions
$A$ system gives out $x \ J$ of heat and does $y \ J$ of work on its surroundings. What is the internal energy change?
$A$ system absorbs $600 \ J$ of heat and does work equivalent to $300 \ J$ on its surroundings. The change in internal energy is ...... $J$.
Medium
View SolutionThe gas absorbs $100 \ J$ and is simultaneously compressed by a constant external pressure of $1.50 \ atm$ from $8 \ L$ to $2 \ L$ volume. Hence $\Delta U$ will be ..... $J$.
Medium
View Solution$A$ gas absorbs $150 \ J$ of heat and expands by $300 \ cm^3$ against a constant external pressure of $2 \times 10^5 \ N \ m^{-2}$. What is the change in internal energy $(\Delta U)$ of the system (in $J$)?
$A$ mixture of $2 \ mol$ of carbon monoxide and $1 \ mol$ of oxygen is ignited in a closed vessel to form carbon dioxide. If $\Delta H$ is the enthalpy change and $\Delta U$ is the change in internal energy,then:
Medium
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