A metal chloride contains 55.0 % of chlorine | vedclass

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(A) $1$. Calculate the molar mass of the metal chloride using the ideal gas law at $STP$ ($22400 \ mL$ per mole):$Molar \ mass = \frac{Mass 	imes 224

Vedclass · Accepted Answer

$MCl_2$

Vedclass · Answer

(A) $1$. Calculate the molar mass of the metal chloride using the ideal gas law at $STP$ ($22400 \ mL$ per mole):$Molar \ mass = \frac{Mass 	imes 22400}{Volume} = \frac{0.57 \ g 	imes 22400 \ mL/mol}{100 \ mL} = 127.68 \ g/mol$.$2$. Calculate the mass of chlorine in one mole of the compound:$Mass \ of \ Cl = 127.68 	imes 0.55 = 70.224 \ g$.$3$. Determine the number of chlorine atoms per molecule:$Number \ of \ Cl \ atoms = \frac{70.224}{35.5} \approx 2$.$4$. Therefore,the molecular formula is $MCl_2$.

$A$ metal chloride contains $55.0 \%$ of chlorine by weight. $100 \ mL$ of vapours of the metal chloride at $STP$ weigh $0.57 \ g$. The molecular formula of the metal chloride is $...$. (Given: Atomic mass of chlorine is $35.5 \ u$)

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