Question

Given, \[S{O_2}(g) + C{l_2}(g) \to S{O_2}C{l_2}(g)\] If \[8\]g of \[S{O_2}\] is mixed with 14.2g of \[C{l_2}\], and one mole of \[S{O_2}C{l_2}\] is \[135\]g, What is the number of moles in \[C{l_2}\] (chlorine) and \[S{O_2}\] (sulfur dioxide)?

Answer 1

Hint: Sulfuryl chloride is an inorganic compound with additives. At room temperature, it's far from a colorless liquid with a pungent odor. Sulfuryl chloride isn't always decided in nature, as can be inferred from its fast hydrolysis. Sulfuryl chloride is generally stressed with thionyl chloride.

Complete answer:
We will use the additives to calculate the number of moles the amount of moles is given mass divided with the useful resource of the usage of the molar mass for any species/atom/chemical or compound. In the question, the masses of sulfur and chlorine are given, and their molar mass is mentioned it's the sum of character atoms present.
Numbers of moles with apprehend to sulfur dioxide will be:
Molar mass of sulfur dioxide will be: \[32 + 16 + 16 = 64g/mol\]
 \[
  No.\,of \, moles = \dfrac{8}{{64.07}} \\
   = 0.125mol \\
 \]
A number of moles with recognition to chlorine will be:
Molar mass of chlorine will be: \[70.9g/mol\].
 \[
  No.\,of\,moles = \dfrac{{14.2}}{{70.9}} \\
   = 0.197mol \\
 \]
Sulfur dioxide is found in much less quantity compared to chlorine, so we are able to say that there may be a molar extra.
And so AT MOST we are able to shape \[0.125\]mol of sulfuryl chloride, a mass (given \[100\% \] yield) of
 \[0.125mol \times 134.96g/mol = 16.9g\]

Note:
Sulfuryl chloride is used as its miles a pourable liquid, its miles considered extra on hand than to dispense. It is used as a reagent inside the facet of the conversion of C-H to C-Cl adjacent to activating substituent which incorporates carbonyls and sulfoxides. It moreover chlorinated alkanes, alkenes, alkynes, aromatics, ethers (which encompass tetrahydrofuran), and epoxides.