A sample of a certain binary compound contains 6.93 g of silicon and 7.89 g of oxygen. What is the percent composition of the co

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2 months ago

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mpound?

2 answers:

lions [2.9K] · Answer 1 · 2026-03-15T12:03:04+03:00

Given, mass of silicon = 6.93 g

mass of oxygen = 7.89 g

Now calculate the moles of both silicon and oxygen:

$Number of moles = \frac{given mass}{molar mass}$

Substituting the provided mass values into the formula above:

$Number of moles of silicon = \frac{given mass of silicon in g}{molar mass of silicon}$

= $\frac{6.93 g}{28 g/mol}$

= $0.2475 mol$

$Number of moles of oxygen = \frac{given mass of silicon in g}{molar mass of silicon}$

= $\frac{7.89 g}{16 g/mol}$

= $0.493125 mol$

So,

Total moles = number of silicon + number of oxygen moles

= $0.493125 mol+0.2475 mol$ = $0.740625 mol$

$Percentage composition = \frac{number of moles of an atom}{total number of moles of the compound}\times 100$

Finally, input the values in the formula provided:

$Percentage composition of silicon= \frac{number of moles of silicon}{total number of moles of the compound}\times 100$

$Percentage composition of silicon= \frac{0.2475 mol}{0.740625 mol}\times 100$

= $33.41 percent$

$Percentage composition of oxygen= \frac{number of moles of oxygen}{total number of moles of the compound}\times 100$

$Percentage composition of silicon= \frac{0.493125 mol}{0.740625 mol}\times 100$

= $66. 58 percent$

Thus, the percent composition of silicon and oxygen is $33.41 percent$ and $66. 58 percent$

KiRa [2.9K] · Answer 2 · 2026-03-15T12:01:21+03:00

KiRa [2.9K]2 months ago

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