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Stoichiometric Calculations

When burnt in...

Question

When burnt in air, $14.0$ g mixture of carbon and sulphur gives a mixture of $C O_{2}$ and $S O_{2}$ in the volume ratio of $2 : 1$ by volume. Being measured at the same conditions of temperature and pressure, number of moles of carbon is:

A

0.75

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B

0.5

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C

0.40

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D

0.25

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Solution

The correct option is A $0.5$
The volume ratio produced = 2:1
That means double the moles of carbon dioxide is produced
Let, mass of carbon = x g
Mass of S = $(14 - x)$ g

Moles of carbon= $\frac{x}{12}$

Moles of S = $\frac{14 - 4}{32}$

and we have

$2 \times m o l e s o f c a r b o n = m o l e s o f S$

$2 \times \frac{x}{12} = \frac{14 - x}{32}$

On soving, we get x = 6 g

$∴$ Moles of carbon = $\frac{6}{12} = 0.5$

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