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(A) The general combustion reaction for a hydrocarbon $C_xH_y$ is given by: $C_xH_y + (x + \frac{y}{4}) O_2 \rightarrow xCO_2 + \frac{y}{2} H_2O$ Give

Vedclass · Accepted Answer

$C_8H_6$

Vedclass · Answer

(A) The general combustion reaction for a hydrocarbon $C_xH_y$ is given by: $C_xH_y + (x + \frac{y}{4}) O_2 \rightarrow xCO_2 + \frac{y}{2} H_2O$ Given that the reaction produces $3$ equivalents of water,we have: $\frac{y}{2} = 3 \Rightarrow y = 6$ Given that the reaction requires $9.5$ equivalents of oxygen,we have: $x + \frac{y}{4} = 9.5$ Substituting $y = 6$: $x + \frac{6}{4} = 9.5$ $x + 1.5 = 9.5$ $x = 8$ Therefore,the molecular formula of the hydrocarbon $A$ is $C_8H_6$.

When a hydrocarbon $A$ undergoes combustion in the presence of air,it requires $9.5$ equivalents of oxygen and produces $3$ equivalents of water. What is the molecular formula of $A$?

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