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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Similar questions

Q. 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

Q. Mass of hydrogen atom in 43 g of hexane

(C_{6} H_{14})

is:

When 3.0g of carbon is burnt in 8.00g oxygen, 11.00g of carbon dioxide is produced. What mass of carbon dioxide will be formed when 3.00g of carbon is burnt in 50g of oxygen? Which law of chemical combination will govern your answer?

Q. How many litres of

O_{2}

at STP are needed for the complete combustion of

80 g

of liquid hexane (

C_{6} H_{14})

?
(

G i v e n : C_{6} H_{14} + O_{2} \to C O_{2} + H_{2} O

)

Q. Question 2
When 3.0 g of carbon is burnt in 8.00 g oxygen, 11.00 g of carbon dioxide is produced. What mass of carbon dioxide will be formed when 3.00 g of carbon is burnt in 50.00 g of oxygen? Which law of chemical combinations will govern your answer?

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20 g of hexane (C6H14) is combusted with an excess of oxygen. The mass of carbon dioxide formed will be: The chemical reaction is: C6H14+192O2→6CO2+7H2O

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