Question

Liquid hexane CH3CH24CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O . What is the theoretical yield of carbon dioxide formed from the reaction of 81.0g of hexane and 360.g of oxygen gas?

Answer 1

The theoretical yield of carbon dioxide formed from the reaction of 81.0g of hexane and 360.g of oxygen gas is  312.63 grams

calculation

 step 1 :write the equation for reaction

2CH3(CH2)4CH3  +19 O2  →   12CO2  +14 H2O

step2:

   find moles of each reactant

mole= mass/molar mass

moles of CH3(CH2)4CH3 =  81 g / 86 g/mol = 0.942 moles

moles of O2=  360g/32  =11.25  moles

step 3:   find the moles of CO2

since O2 is the limiting reagent  and the mole ratio in equation above of O2 :CO2 is 19 :12 the moles of CO2

=  11.25 x12/19 =7.1053 moles

step  4: find the theoretical yield

= moles x  molar mass (44g/mol)

- 7.1053 moles x 44 g/mol= 312.63 grams

Answer 2

Answer:

248.6352 grams is the theoretical yield of carbon dioxide formed from the reaction.

Explanation:

$2CH_3(CH_2)_4CH_3 +19O_2\rightarrow 12CO_2+14H_2O$

Moles of hexane= $\frac{81.0 g}{86 g/mol}=0.9418 mol$

Moles of oxygen gas = $\frac{360 g}{32 g/mol}=11.25 mol$

Moles of hexane are in limited quantity. So, the theoretical yield of carbon dioxide formed will depend upon moles of hexane.

2 moles of hexane gives 12 moles of carbon dioxide.

Then 0.9418 mol of hexane will gives:

$\frac{12}{2}\times 0.9418 mol=5.6508 mol$

Mass of 5.6508 moles of carbon dioxide gas L:

$5.6508 mol\times 44 g/mol=248.6352 g$

248.6352 grams is the theoretical yield of carbon dioxide formed from the reaction.