CameraIcon
CameraIcon
SearchIcon
MyQuestionIcon


Question

Assuming that petrol is octane $$({ C }_{ 8 }{ H }_{ 18 })$$ and has density $$0.8 g { mL }^{ -1 }, 1.425$$ litre of petrol on complete combustion will consume:


A
50 mole of O2
loader
B
100 mole of O2
loader
C
125 mole of O2
loader
D
200 mole of O2
loader

Solution

The correct option is C $$125$$ mole of $${ O }_{ 2 }$$
As we know that,

$$\text{density} = \cfrac{\text{mass}}{\text{volume}}$$

Density of octane $$= 0.8 g\ m {L}^{-1}$$

Volume of octane $$= 1.425 L$$

$$\therefore \; 0.8 = \cfrac{mass}{1.425}$$

$$\Rightarrow \text{ given mass of octane} = 0.8 \times 1.425\times 1000 = 1140 g$$

Molecular mass of octane, $$\left( {C}_{8}{H}_{18} \right) = 114 g$$

No. of moles $$= \cfrac{\text{Given mass}}{\text{Molecular mass}} = \cfrac{1140}{114} = 10\text{ mole}$$

Combustion of octane-

$$2{C}_{8}{H}_{18} + 25 {O}_{2} \longrightarrow 16 C{O}_{2} + 18 {H}_{2}O$$

No. of moles of oxygen required for the combustion of 1 mole octane = 12.5 moles

$$\therefore$$ No. of moles of oxygen required for the combustion of 10 mole octane $$= \cfrac{12.5}{1} \times 10 = 125\text{ mole}$$

Hence, 1.425 litres of octane will consume 125 moles of oxygen.

Hence, the correct option is $$C$$

Chemistry

Suggest Corrections
thumbs-up
 
0


similar_icon
Similar questions
View More


similar_icon
People also searched for
View More



footer-image