Using the following equation, determine the % yield from the following reaction if 30.65 g of octane (c_8 8 h_{18} 18 ) react with excess oxygen to produce 81.75 g of co_2 2 (g) 2c_8 8 h_{18} 18 (i) + 25o_2 2 (g) → 16co_2 2 (g) + 18h_2 2 o(l)

86.4%

Explanation:

MM (C₈H₁₈) = 12*8+1*18 = 114

MM (CO₂) = 12 + 16*2 = 44

moles of C₈H₁₈ = 30.65 / 114 = 0.269

moles of CO₂ = 81.75 / 44 = 1.860

The % Yield is the amount of a product formed divided by the theorical amount formed if the limiting reactant reacts 100%.

The amount formed of CO₂ is 1.860 moles

The theorical amount formed is obtained with the rule of three and the stoichiometric coefficients.

2 moles of C₈H₁₈ produces 16 moles of CO₂

0.269 moles of C₈H₁₈ produces x moles of CO₂

x = 0.269 * 16 / 2 = 2.152 moles

2b2t

explanation:

2b2t