Q.

Assuming that petrol is octane C8H18 and has a density of 0.8gm/ml,1.425 litres of petrol on complete combustion will consume

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a

50 moles of O2

b

100 moles of O2

c

125 moles of O2

d

200 moles of O2

answer is C.

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Detailed Solution

Petrol is assumed as octane having a chemical formula C8H18 and when this undergoes combustion it forms carbon dioxide and water.

The balanced chemical equation is

2C8H18+25O216CO2+18H2O

 The density, d=0.8gm/ml

The molar mass of C8H18=114 g/mol

Volume of petrol given =1.425 L

We know, density, d= mass/volume mass =0.8×1.425×1000=1140 g

And no. of moles = given mass/molar mass

So, the no. of moles of octane =1140/114=10

2 moles of C8H18 requires 25 moles of O2

10 moles of C8H18 requires =252×10=125

Hence, 10 moles of C8H18 requires 125 moles of O2.

 

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