Question

A gas of mass 1.6 g , kept at 760 mm Hg pressure and 273 K temperature, occupies a volume of 1.12 L.Find the molar mass of the gas and its vapour density with respect to hydrogen.
please give correct answer​

Answer 1

• Molar mass = $\sf{42.08\:gmol^{-1}}$
• Vapour Density = $\sf{21.04\:gmol^{-1}}$

Explanation:

Given,

• Mass of gas = 1.6 g
• Pressure = 760 my Hg
• Temperature = 273 k
• Volume = 1.12 l

Formula,

• PV = nRT

As we need to find 'n' - number of moles,

n = $\sf\dfrac{PV}{RT}$

• P = Pressure,
• T = Temperature,
• V = Volume and
• R = Gas constant $\sf{0.082\:l\:mol^{-1}\:k^{-1}}$

Substituting values,

$\sf{⟶\:n\:=}$$\sf\dfrac{PV}{RT}$

$\sf{⟶\:n\:=}$$\sf\dfrac{760\:×\:1.12}{0.082\:×\:273}$

$\sf{⟶}$$\sf\boxed{n\:=\:{38.024}}$

Molar Mass,

$\sf{⟶}$$\sf{No.\:of.\:Moles\:=}$ $\sf\dfrac{Given\:Mass}{Molar\:Mass}$

$\sf{⟶}$Molar Mass = $\sf\dfrac{Given\:Mass}{No.\:of.\:Moles}$

$\sf{⟶}$Molar Mass = $\sf\dfrac{1.6\:×\:1000}{38.024}$

$\sf{⟶}$Molar Mass = $\sf\boxed{{42.08\:g\:mol^{-1}}}$

Vapour Density,

$\sf{⟶}$ $\sf{Vapour Density}$ = $\sf\dfrac{Molar\:Mass}{2}$

$\sf{⟶}$$\sf{Vapour Density}$ = $\sf\dfrac{42.08}{2}$

$\sf{⟶}$$\sf{Vapour Density}$ = $\sf\boxed{{21.04\:g\:mol^{-1}}}$

• ∴ Molar mass = $\sf{42.08\:gmol^{-1}}$
• Vapour Density = $\sf{21.04\:gmol^{-1}}$

Answer 2

Explanation:

Molar mass = \sf{42.08\:gmol^{-1}}42.08gmol−1

Vapour Density = \sf{21.04\:gmol^{-1}}21.04gmol−1

Explanation:

Given,

Mass of gas = 1.6 g

Pressure = 760 my Hg

Temperature = 273 k

Volume = 1.12 l

Formula,

PV = nRT

As we need to find 'n' - number of moles,

n = \sf\dfrac{PV}{RT}RTPV

P = Pressure,

T = Temperature,

V = Volume and

R = Gas constant \sf{0.082\:l\:mol^{-1}\:k^{-1}}0.082lmol−1k−1

Substituting values,

\sf{⟶\:n\:=}⟶n= \sf\dfrac{PV}{RT}RTPV

\sf{⟶\:n\:=}⟶n= \sf\dfrac{760\:×\:1.12}{0.082\:×\:273}0.082×273760×1.12

\sf{⟶}⟶ \sf\boxed{n\:=\:{38.024}}n=38.024

Molar Mass,

\sf{⟶}⟶ \sf{No.\:of.\:Moles\:=}No.of.Moles= \sf\dfrac{Given\:Mass}{Molar\:Mass}MolarMassGivenMass

\sf{⟶}⟶ Molar Mass = \sf\dfrac{Given\:Mass}{No.\:of.\:Moles}No.of.MolesGivenMass

\sf{⟶}⟶ Molar Mass = \sf\dfrac{1.6\:×\:1000}{38.024}38.0241.6×1000

\sf{⟶}⟶ Molar Mass = \sf\boxed{{42.08\:g\:mol^{-1}}}42.08gmol−1

Vapour Density,

\sf{⟶}⟶ \sf{Vapour Density}VapourDensity = \sf\dfrac{Molar\:Mass}{2}2MolarMass

\sf{⟶}⟶ \sf{Vapour Density}VapourDensity = \sf\dfrac{42.08}{2}242.08

\sf{⟶}⟶ \sf{Vapour Density}VapourDensity = \sf\boxed{{21.04\:g\:mol^{-1}}}21.04gmol−1

∴ Molar mass = \sf{42.08\:gmol^{-1}}42.08gmol−1

Vapour Density = \sf{21.04\:gmol^{-1}}21.04gmol−1

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