Question

How many moles of lead (II) chloride will be formed from a reaction between $6.5$ g of $PbO$ and $3.2$ g of $HCl$?

[Atomic wt. of $Pb=207$ g/mol]

• A. $0.011$
• B. $0.029$
• C. $0.044$
• D. $0.333$

Answer 1

Answer: (B)

$0.029$

The balanced reaction is as follows :

$PbO+2HCl\to PbC{l}_2+H_{2}O$
Mass given: $6.5$ g $3.2$ g

No. of moles: $\frac{6.5}{223}$ $\frac{3.2}{36.5}$
$=0.029$ $=0.087$

Ratio of moles given
and stoichiometry $\frac{0.029}{1}$ $\frac{0.087}{2}$

coefficient: $=0.029$ $=0.0435$

As $0.029$ is lower than $0.0435$, $PbO$ is limiting reagent and product will form according to the number of moles of $PbO$ (given).

So, moles produced of $PbC{l}_2=\frac{1}{1}\times 0.029=0.029$ moles.

Hence the correct option is B.