Question

In a laboratory, 23.5 g of cyclohexane is burned and 5.5 liters of carbon dioxide was obtained. a) Balance the reaction b) Calculate the reaction yield. dCO2 = 1.9 g/L

Answer 1

The balanced reaction will be

C6H12(l) + 9O2(g) ------ 6CO2(g) + 6H2O(l)

Molar mass of cyclohexane = 6 * 12 + 6 * 1 = 78 gm/mol

Number of moles of cyclohexane = Mass/molar mass = 23.5/78 = 0.3012 moles

Mass of CO2 obtainted = Volume * Density

=> 5.5L * 1.9 g/L

=> 10.45 grams

Molar mass of CO2 = 12 + 2 * 16 = 44 gm/mol

Number of moles of CO2 obtained = 10.45/44 = 0.2375 moles

1 mole of C6H12 would give 6 moles of CO2

Hence number of moles of CO2 produced if 100% yield = 0.3012 * 6 = 1.8072

Reaction Yield = 0.2375/1.8072 * 100 = 13.1418%