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Standard X

Chemistry

Saturated and Unsaturated Hydrocarbon

A sample of a...

Question

A sample of a gaseous hydrocarbon occupying $1.12$ liters at NTP when completely burnt in presence of oxygen produces $2.2$ g of $C O_{2}$ and $1.8$ g of $H_{2} O$ . Calculate the weight of the compound taken and the volume $O_{2}$ at NTP required for its burning. Find the molecular formula of the hydrocarbon.

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Solution

$22.4$ of hydrocarbon $= 1$ mol,
$1.12$ liter $= 0.05$ mol.
$C_{x} H y + (x + \frac{y}{4}) O_{2} ⟶ x C O_{2} + \frac{y}{2} H_{2} O$
$1$ mol of $C_{x} H y = x$ moles of $C O_{2}$
$0.05 x = 0.05 m o l e s x = 1$
$0.05$ mole of $C_{x} H y$ gives $= 0.1$ mole of $H_{2} O$
$1$ mole of $C_{x} H y$ gives $\frac{y}{2}$ moles of $H_{2} O$
$\frac{y}{2} = 2 ⟹ y = 4$
Hydrocarbon is $C H_{4}$ .

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A sample of a gaseous hydrocarbon occupying 1.12 liters at NTP when completely burnt in presence of oxygen produces 2.2 g of CO2and 1.8 g of H2O. Calculate the weight of the compound taken and the volume O2 at NTP required for its burning. Find the molecular formula of the hydrocarbon.

22.4 of hydrocarbon =1 mol,1.12 liter=0.05 mol.CxHy+(x+y4)O2⟶xCO2+y2H2O 1 mol of CxHy=x moles of CO20.05x=0.05molesx=10.05 mole of CxHy gives =0.1 mole of H2O 1 mole of CxHy gives y2 moles of H2Oy2=2⟹y=4Hydrocarbon is CH4.