gaseous butane ch3ch22ch3 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 1.74g of butane and 10.5g of oxygen gas?

A combustion reaction occurs whenever a substance reacts with oxygen and releases energy. For example, carbon dioxide and water are released when methane burns in oxygen. The formation of carbon dioxide indicates that the carbon present in methane has been oxidized. One mole of butane requires 6.5 moles of oxygen, so 13 moles of oxygen are required to completely burn 2 moles of butane.

calculation:-

CH₃CH₂CH₂CH₃ + 13/2O₂ ----------> 4CO₂ + 5H₂O

for limiting reagent

The molar mass of butane = 58 g

given mass = 1.74 g

mole = 1.74/ 58 = 0.03 mole

LR = 0.03/ stoichiometry

= 0.03

molar mass of O₂ = 32

given mass = 10.5 g

mole = 10.5/32

= 0.328 mole
LR = 0.328 / stoichiometry

= 0.328 × 2 / 13

= 0.051

Here LR is butane.

So, 58 gram butane prodece = 176 gram CO₂

1.74 gram butane produce = 176/58 × /1.74

Hence, the theoretical yield of carbon dioxide = 5.28 Gram of CO²

Less than 100% recovery. This is because the actual recovery is often lower than the theoretical value. This may be due to incomplete or competing reactions and sample loss during recovery. A balanced formula contains the same number of each type of atom on either side of the reaction arrow. To write a balanced equation reactants go to the left of the arrow and products go to the right of the arrow.

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