After the reaction how much octane is left

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After the reaction, how much octane is left?

2 C8H18 + 25 O2 –> 16 CO2 + 18 H20

0.660 mol of octane is allowed to react with .780 mol of oxygen.
Oxygen is the limiting reactant.
After the reaction, how much octane is left?


General guidance

Concepts and reason

This is based on the concept that the limiting reagent decides how much amount of other reactants will be consumed when the reaction takes place. This decides the amount of product formed. Limiting reagent itself consumed fully and when it consumed, the reaction stops. This is only determined by the help of a balanced chemical equation. Limiting reagent also helps us to identify the percentage yield of the reaction.

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Limiting reagent is also called as limiting reactant. In a reaction, it is limiting reagent consumed totally and the remaining reactants are called as excess reagents.

Percentage theoretical yield is defined as the amount of the formation of the product when the limiting reagent is consumed fully.


Step 1 of 3

Consider the reaction:

2 C,H,g+250, ™16 CO, +18 H,0

This reaction is balanced.

The given reaction is a balanced chemical equation since the number of moles of carbon, hydrogen and oxygen are same on both sides, i.e. 16 moles for carbon, 36 moles for hydrogen, and 50 moles for oxygen.

Step 2 of 3

Calculation for the amount of is consumed is as follows:

0.780 moles of O, X
2 mol of CH,8 = 0,0624 mol of CH8
25 mol of 2

Amount of octane () consumed is found out by dividing the number of the moles of octane involved (i.e. 2 moles) to the number of moles of limiting reagent involved (i.e. 25 moles) and multiply that number to the amount of limiting reagent consumed (i.e. 0.780 moles).

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