If a gas expands from $20 \ cm^3$ to $50 \ cm^3$ at a constant temperature $(T)$ under a pressure of $1 \ atm$,what will be the final pressure?
- A$20 \times \frac{1}{50} \ atm$
- B$50 \times \frac{1}{200} \ atm$
- C$1 \times \frac{1}{20} \times 50 \ atm$
- DNone of these
Explore More
Similar Questions
Calculate the pressure of $HCl$ gas having a density of $8 \, kg \, m^{-3}$ at a temperature of $-40 \, ^oC$. (Given: $R = 8.314 \, J \, K^{-1} \, mol^{-1}$,Molar mass of $HCl = 36.5 \, g \, mol^{-1} = 0.0365 \, kg \, mol^{-1}$)
Medium
View SolutionAt $27\, ^\circ C$ temperature and $1\, bar$ pressure,the volume of a gas is $25\, L$. If the temperature becomes $77\, ^\circ C$ at constant pressure,calculate the volume of the gas. (in $, L$)
Medium
View SolutionIf $28 \ g$ of $N_2$ gas occupies a volume of $10 \ L$ at a pressure of $2.46 \ atm$,the temperature will be ......... $K$.
Medium
View SolutionWhich of the following is equal to $[{\partial P/\partial V}]_T$ for an ideal gas?
Medium
View SolutionThe volume of a given amount of gas at $27^{\circ} C$ at constant pressure is $420 \ cm^3$. If the temperature is reduced by $20^{\circ} C$ at constant pressure, what will be the volume of the gas (in $cm^3$)?
Vedclass 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