What is the density of one mole of $He$ (molar mass $= 4 \ g \ mol^{-1}$) at $300 \ K$ and a pressure of $0.82 \ atm$? $(R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1})$
- A$1.33 \times 10^{-2} \ g \ mL^{-1}$
- B$1.33 \times 10^{-2} \ g \ L^{-1}$
- C$1.33 \times 10^{-1} \ g \ L^{-1}$
- D$1.33 \times 10^{-1} \ g \ mL^{-1}$
Explore More
Similar Questions
Calculate the volume of $6.022 \times 10^{21}$ molecules of $CO_2$ at $300 \ K$ temperature and $2 \ bar$ pressure. $[R = 8.314 \times 10^{-2} \ bar \ L \ K^{-1} \ mol^{-1}]$ (in $mL$)
Medium
View SolutionWhich of the following graphs is correct for an ideal gas?
What will be the pressure exerted by a mixture of $3.2 \ g$ of methane and $4.4 \ g$ of carbon dioxide contained in a $9 \ dm^3$ flask at $27^{\circ} C$?
Medium
View SolutionThe value of the gas constant $R$ depends on which of the following?
Easy
View SolutionThe densities of two gases are in the ratio $1:2$ and their temperatures are in the ratio $2:1$. What is the ratio of their corresponding pressures?
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