$PCl X_{5}$ dissociates as $PCl X_{5} PCl X_{3} + Cl X_{2}$ and is $40%$ dissociated at equilibrium. Taking $P = 31$ , $Cl = 35.5$ , find the vapour density of the equilibrium mixture, to two decimals.

Numerical answer type, tolerance 0.02.

Answer: 74.46

PCl X_{5}

= 31 + 177.5 = 208.5 g/mol. For 1 mol initially, moles at equilibrium = 1 + 0.4 = 1.4, mass unchanged. Average molar mass = 208.5/1.4 = 148.93; vapour density = 148.93/2 = 74.46.

Practice Mole Concept More on Average molar mass of mixtures, vapour density

Previous questionNext question

More questions on Average molar mass of mixtures, vapour density

N2O4 (92 g/mol) partly dissociates as N2O4 <=> 2NO2 at a certain temperature, and the equilibrium mixture has vapour density 34.5. The degre... JEE Main level
A mixture of CO (28 g/mol) and CO2 (44 g/mol) has vapour density 17.2. Find the mass percent of CO2 in the mixture, to the nearest integer. JEE Main level
A mixture of CH4 (16 g/mol) and O2 (32 g/mol) has a density of 1.340 g/L at STP (molar volume 22.4 L/mol). Find the volume percent of CH4 in... JEE Main level
Which of the following gas mixtures has an average molar mass of 30 g/mol? (Molar masses in g/mol: CH4 16, CO2 44, O2 32, N2 28, NO 30, C2H6... JEE Main level
A mixture of 1 mol N2 and 3 mol H2 (N=14, H=1) reacts by N2 + 3H2 -> 2NH3 until 25% of the N2 has reacted. The average molar mass of the res... JEE Advanced level
A mixture of H2 and N2 has a density 6.0 times that of hydrogen gas under the same conditions (H2=2, N2=28 g/mol). The mass percent of H2 in... JEE Advanced level

PClX5​ dissociates as PClX5​​PClX3​+ClX2​ and is 40% dissociated at equilibrium. Taking P=31, Cl=35.5, find the vapour density of the equilibrium mixture, to two decimals.

Answer: 74.46

More questions on Average molar mass of mixtures, vapour density

$PCl X_{5}$ dissociates as $PCl X_{5} PCl X_{3} + Cl X_{2}$ and is $40%$ dissociated at equilibrium. Taking $P = 31$ , $Cl = 35.5$ , find the vapour density of the equilibrium mixture, to two decimals.