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The equation for the burning of octane is: 

2C8H18 + 25O2 → 16CO2 + 18H2

(i) How many moles of carbon dioxide are produced when one mole of octane barns? 

(ii) What volume, at sip, is occupied by the number of moles determined in (b) (i) ? 

(iii) If the relative molecular mass of carbon dioxide is 44, what is the mass of carbon dioxide produced by burning two moles of octane? 

(iv) What is the empirical formula of octane?

1 Answer

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(i)

One mole of octane forms 8 moles of CO2 on burning.

(ii) At STP one mole of gas occupies 22.4 litres

 ∴    8 moles of CO2 will occupy = 22.4 x 8

                                                 = 179.2 l.

(iii) From equation we know that 2 moles of octane produces 16 moles of CO2

∴  Mass of CO2 produced = 16 x 44

                                        = 704

(iv) Empirical formula of octane is C4H9.

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