(C) The ideal gas equation is $PV = nRT$,where $n = \frac{m}{M}$.Substituting $n$,we get $PV = \frac{m}{M} RT$.Since density $d = \frac{m}{V}$,we can

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

(C) The ideal gas equation is $PV = nRT$,where $n = \frac{m}{M}$.Substituting $n$,we get $PV = \frac{m}{M} RT$.Since density $d = \frac{m}{V}$,we can write $P = \frac{dRT}{M}$.For gas $A$: $P_A = \frac{d_A RT}{M_A}$.For gas $B$: $P_B = \frac{d_B RT}{M_B}$.The ratio is $\frac{P_A}{P_B} = \frac{d_A}{d_B} \times \frac{M_B}{M_A}$.Given $d_A = 3.0 \, g \, dm^{-3}$,$d_B = 1.5 \, g \, dm^{-3}$,and $M_A = \frac{1}{2} M_B$ (or $\frac{M_B}{M_A} = 2$).Substituting these values: $\frac{P_A}{P_B} = \frac{3.0}{1.5} \times 2 = 2 \times 2 = 4$.

Class 11 Chemistry States of Matter Ideal gas equation and Related gas laws

Medium

At the same temperature,gas $A$ is taken in a $0.5 \, dm^3$ flask and gas $B$ is taken in a $1 \, dm^3$ flask. If the density of $A$ is $3.0 \, g \, dm^{-3}$ and that of $B$ is $1.5 \, g \, dm^{-3}$,and the molar mass of $A$ is $1/2$ of $B$,what is the ratio of the pressures exerted by the gases?

A
$\frac{P_A}{P_B} = 2$
B
$\frac{P_A}{P_B} = 1$
C
$\frac{P_A}{P_B} = 4$
D
$\frac{P_A}{P_B} = 3$

Explore More

Browse All

Question Bank

All Subjects

Class 11 Questions

Class 11

Chemistry Questions

Chapter

States of Matter

Subtopic

Ideal gas equation and Related gas laws

If the volume of $N_2$ gas at $STP$ is $204.75 \, mL$,then calculate the volume of the gas at $1.5 \, bar$ pressure and $127 \, ^oC$ temperature.

Medium

View Solution

$A$ bulb of $1 \, L$ capacity contains $5 \, g$ of ethane. If the pressure increases to $10 \, atm$,what will be the temperature in $^oC$ at which the bulb will burst?

Difficult

View Solution

$A$ monoatomic ideal gas,initially at temperature $T_1$,is enclosed in a cylinder fitted with a frictionless piston. The gas is allowed to expand adiabatically to a temperature $T_2$ by releasing the piston suddenly. $L_1$ and $L_2$ are the lengths of the gas columns before and after the expansion,respectively. The ratio $\frac{T_2}{T_1}$ is:

EasyMHT CET 2021

View Solution

At $298 \, K$ temperature,$4 \, g$ of $H_2$ gas is filled in a $500 \, mL$ vessel. Due to a small hole in the vessel,after some time,the pressure in the vessel becomes $50 \, bar$. Find the number of $H_2$ molecules that have escaped from the vessel? $(R = 8.314 \times 10^{-2} \, L \, bar \, mol^{-1} \, K^{-1})$

Medium

View Solution

At $200 \ K$,an ideal gas $(X)$ present in a $1 \ L$ flask has a concentration of $1 \ mol \ L^{-1}$. At the same temperature,$0.1 \ mol$ of $X$ is added into the vessel. What is the final pressure of the gas in $atm$?
(Given $R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1}$)

MediumAP EAMCET 2023

View Solution

Vedclass Products

For Students

Vedclass Test Series

Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.

Start Free Trial

For Teachers

Exam Paper Generator

Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.

Try Free

For Institutes

Online Exam Module

Live online exams with unlimited students, 360° analytics & white-label branding.

See Demo

At the same temperature,gas $A$ is taken in a $0.5 \, dm^3$ flask and gas $B$ is taken in a $1 \, dm^3$ flask. If the density of $A$ is $3.0 \, g \, dm^{-3}$ and that of $B$ is $1.5 \, g \, dm^{-3}$,and the molar mass of $A$ is $1/2$ of $B$,what is the ratio of the pressures exerted by the gases?

Similar Questions

If the volume of $N_2$ gas at $STP$ is $204.75 \, mL$,then calculate the volume of the gas at $1.5 \, bar$ pressure and $127 \, ^oC$ temperature.

$A$ bulb of $1 \, L$ capacity contains $5 \, g$ of ethane. If the pressure increases to $10 \, atm$,what will be the temperature in $^oC$ at which the bulb will burst?

At $200 \ K$,an ideal gas $(X)$ present in a $1 \ L$ flask has a concentration of $1 \ mol \ L^{-1}$. At the same temperature,$0.1 \ mol$ of $X$ is added into the vessel. What is the final pressure of the gas in $atm$?(Given $R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1}$)

Vedclass Test Series

Exam Paper Generator

Online Exam Module

At $200 \ K$,an ideal gas $(X)$ present in a $1 \ L$ flask has a concentration of $1 \ mol \ L^{-1}$. At the same temperature,$0.1 \ mol$ of $X$ is added into the vessel. What is the final pressure of the gas in $atm$?
(Given $R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1}$)