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
The theoretical yield of CO2 is 31.24 g of carbon dioxide.
The equation of the reaction is;
C6H14(l) + 19/2 O2(g) -----> 6CO2(g) + 7H2O(g)
Number of moles of hexane = 81.0g/86 g/mol = 0.94 moles
Number of moles of oxygen = 360.g/32 g/mol = 1.12 moles
To obtain the limiting reactant;
1 mole of liquid hexane reacts with 9.5 moles of oxygen
0.94 moles of liquid hexane reacts with 0.94 moles × 9.5 moles/ 1 mole
= 8.93 moles of oxygen
There is not enough oxygen hence it is the limiting reactant.
9.5 moles of oxygen yields 6 moles of carbon dioxide
1.12 moles of oxygen yields 1.12 moles × 6 moles/ 9.5 moles
= 0.71 moles of carbon dioxide
Mass of carbon dioxide = 0.71 moles of carbon dioxide × 44 g/mol
= 31.24 g of carbon dioxide
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