Oxygen oxidises ethyne to carbon dioxide and water as shown by the equation:
$2 C_{2} H_{2} + 5 O_{2} \to 4 C O_{2} + 2 H_{2} O$

What volume (in $d m^{3}$ ) of ethyne gas at STP, is required to produce $8.4 d m^{3}$ of carbon dioxide? $[H = 1, C = 12, O = 16]$

(Please give your in the form of nearest integer)

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Solution

$2 C_{2} H_{2} + 5 O_{2} \to 4 C O_{2} + 2 H_{2} O$
2vol. 5vol. 4vol. 2vol.
If $4$ vol. of $C O_{2}$ is produced by $2$ vol. of $C_{2} H_{2}$ at STP,
then $8.4 d m^{3}$ of $C O_{2}$ is produced by $\frac{2}{4} \times 8.4 =$ 4.2 $d m^{3}$ of ethyne.

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Oxygen oxidises ethyne to carbon dioxide and water as shown by the equation:2C2H2+5O2→4CO2+2H2OWhat volume (in dm3) of ethyne gas at STP, is required to produce 8.4 dm3 of carbon dioxide? [H=1,C=12,O=16](Please give your in the form of nearest integer)

2C2H2+5O2→4CO2+2H2O2vol. 5vol. 4vol. 2vol.If 4vol. of CO2 is produced by 2 vol. of C2H2 at STP,then 8.4dm3 of CO2 is produced by 24×8.4= 4.2 dm3 of ethyne.

$2 C_{2} H_{2} + 5 O_{2} \to 4 C O_{2} + 2 H_{2} O$
2vol. 5vol. 4vol. 2vol.
If $4$ vol. of $C O_{2}$ is produced by $2$ vol. of $C_{2} H_{2}$ at STP,
then $8.4 d m^{3}$ of $C O_{2}$ is produced by $\frac{2}{4} \times 8.4 =$ 4.2 $d m^{3}$ of ethyne.