Chemistry
The equation for the burning of octane is:
2C8H18 + 25O2 ⟶ 16CO2 + 18H2O
(i) How many moles of carbon dioxide are produced when one mole of octane burns?
(ii) What volume at S.T.P. is occupied by the number of moles determined in (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?
Related Questions
(a) When carbon dioxide is passed over red hot carbon, carbon monoxide is produced according to the equation :
CO2 + C ⟶ 2CO
What volume of carbon monoxide at S.T.P. can be obtained from 3 g of carbon?
(b) 60 cm3 of oxygen was added to 24 cm3 of carbon monoxide and mixture ignited. Calculate:
(i) volume of oxygen used up and
(ii) Volume of carbon dioxide formed.
How much calcium oxide is obtained by heating 82 g of calcium nitrate? Also find the volume of NO2 evolved:
2Ca(NO3)2 ⟶ 2CaO + 4NO2 + O2
Ordinary chlorine gas has two isotopes 3517Cl and 3717Cl in the ratio of 3:1. Calculate the relative atomic mass of chlorine.
Silicon (Si = 28) forms a compound with chlorine (Cl = 35.5) in which 5.6 g of silicon combines with 21.3 g of chlorine. Calculate the empirical formula of the compound.