The gaseous hydrocarbon Acetylene, $C_{2} H_{2}$ used in welder's torches, releases $1300 K J$ , when $1 m o l e$ of $C_{2} H_{2}$ undergoes combustion, then which of the following is not true?

Combustion of Acetylene is an exothermic reaction

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The balanced chemical reaction of combustion of Acetylene is:

C_{2} H_{2} + 5 O_{2} \to 2 C O_{2} + H_{2} O

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2 m o l e s

of water produced when

2

moles of Acetylene reacts

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44 g

C O_{2}

produced, when

13 g

of Acetylene reacts

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Solution

The correct option is D The balanced chemical reaction of combustion of Acetylene is: $C_{2} H_{2} + 5 O_{2} \to 2 C O_{2} + H_{2} O$
Option B is not true as the balanced equation is:-
$C_{2} H_{2} + \frac{5}{2} O_{2} \to$ $2 C O_{2} + H_{2} O$ (balanced)

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Similar questions

How many molecules of oxygen are required for complete combustion of 1 mole of acetylene ( $C_{2} H_{2}$ )?

- 394 k J, - 286 k J

- 1301 k J

C_{2} H_{2}

How many molecules of oxygen are required for complete combustion of 1 mole of acetylene $(C_{2} H_{2})$ ?

[C_{2} H_{2}]

200 c m^{3}

C O_{2}

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