Silicon (Si = 28) Forms a compound with chlorine (Cl = 35.5 ) in which 5.6 g of silicon combines with 21.3 g of chlorine. Calculate the empirical formula of the compound.

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Solution

Given mass of silicon (Si) = 5.6 g
Given mass of chlorine (Cl) = 21.3 g
Molar mass of silicon = 28.09 g
Molar mass of chlorine = 35.5 g
n = $fraction numerator G i v e n space m a s s space over denominator space M o l a r space m a s s end fraction$
Number of moles (n) of silicon = $fraction numerator 5.6 over denominator 28.09 end fraction$ = 0.1993 moles

Number of moles of chlorine = $fraction numerator 21.3 over denominator 35.5 end fraction$ = 0.6 moles
Now , For silicon number of moles should be divided with least number of moles,
For silicon = $fraction numerator space 0.1993 over denominator 0.1993 end fraction$ = 1
For chlorine = $fraction numerator 0.6 over denominator 0.1993 end fraction$ = 3
Hence , the empirical formula will be

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