At 300 K and 1 atmospheric pressure, 10 mL of a hydrocarbon required 55 mL of O2 for complete combustion and 40 mL of CO2 is formed. The formula of the hydrocarbon is :

Question

At 300 K and 1 atmospheric pressure, 10 mL of a hydrocarbon required 55 mL of O2 for complete combustion and 40 mL of CO2 is formed. The formula of the hydrocarbon is : (A) C4H8  (B) C4H7Cl  (C) C4H10  (D) C4H6

Tardigrade Admin · Accepted Answer

C x H y +( x +( y /4)) O 2 longrightarrow xCO 2+( y /2) H 2 O 1010(x+(y/4)) 10 x By given data, 10(x+(y/4))=55 ldots . .(1) 10 x=40 ldots . .(2) ∴ x=4, y=6 ⇒ C4 H6

Q. At $300 K$ and $1$ atmospheric pressure, $10 m L$ of a hydrocarbon required $55 m L$ of $O_{2}$ for complete combustion and $40 m L$ of $C O_{2}$ is formed. The formula of the hydrocarbon is :

$C_{4} H_{8}$

$C_{4} H_{7} Cl$

$C_{4} H_{10}$

$C_{4} H_{6}$

$C_{x} H_{y} + (x + \frac{y}{4}) O_{2} ⟶ x C O_{2} + \frac{y}{2} H_{2} O$
$1010 (x + \frac{y}{4}) 10 x$
By given data, $10 (x + \frac{y}{4}) = 55 \dots .. (1)$
$10 x = 40 \dots .. (2)$
$∴ x = 4, y = 6 \Rightarrow C_{4} H_{6}$

Q. At 300K and 1 atmospheric pressure, 10mL of a hydrocarbon required 55mL of O2​ for complete combustion and 40mL of CO2​ is formed. The formula of the hydrocarbon is :

C4​H8​

C4​H7​Cl

C4​H10​

C4​H6​