20 g of hexane $(C_{6} H_{14})$ is combusted with an excess of oxygen. The mass of carbon dioxide formed will be:

The chemical reaction is: $C_{6} H_{14} + \frac{19}{2} O_{2} \to 6 C O_{2} + 7 H_{2} O$

30.87 g

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60.72 g

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70.84 g

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35.42 g

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Solution

The correct option is B 60.72 g
Balanced chemical equation,
$C_{6} H_{14} + \frac{19}{2} O_{2} \to 6 C O_{2} + 7 H_{2} O$
Mass of hexane = 20 g
Molar mass of hexane = 86 g/mol
Moles of hexane = $\frac{20}{86}$ = 0.23 mol
From the balanced chemical reaction,
$\frac{m o l e s o f h e x a n e}{1} = \frac{m o l e s o f c a r b o n d i o x i d e}{6}$
Moles of carbon dioxide = 1.38 mol
Mass of carbon dioxide = $1.38 \times 44 = 60.72 g$

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