The balanced equation for combustion in an acetylene torch is shown below: 2c2h2 + 5o2 → 4co2 + 2h2o the acetylene tank contains 35.0 mol c2h2, and the oxygen tank contains 84.0 mol o2. how many moles of co2 are produced when 35.0 mol c2h2 react completely?

67.2 moles

Explanation:

According to the given balanced equation, 2 moles of acetylene combine with 5 moles of oxygen  to produce 4 moles of carbon dioxide .

Thus if 2 moles of acetylene combine with = 5 moles of oxygen

35 moles of acetylene combine with= moles of oxygen

But as only 84 moles of oxygen are available, acetylene is not a limiting reagent.

5 moles of oxygen reacts with = 2 moles of acetylene

84 moles of oxygen reacts with= moles of acetylene

Thus Oxygen is the limiting reagent as it limits the formation of products. Acetylene is excess reagent as it is present in excess.

2 moles of acetylene  produce= 4 moles of carbon dioxide .

33.6 moles of acetylene produce= moles of of carbon dioxide .

Mole is the amount of substance that is equal to Avogadro's constant. 67.2 mole of Carbon dioxide produced when 35.0 mol acetone react completely.

Mole is the amount of substance that is equal to Avogadro's constant.

Given here,

Means 2 moles of acetylene react with 5 moles of oxygen in the combustion reaction. to produce 4 moles of Carbon dioxide.

The molar ratio of Oxygen and acetylene is 5:2

The molar ratio of Acetylene and Carbon dioxide = 2:4

So, 84 moles of , react with

of acetone

hence,

33.6g of acetone react with

of Carbon dioxide

Therefore, we can conclude that 67.2 mole of Carbon dioxide produced when 35.0 mol acetone react completely.

To know more about mole concept, refer to the link:

link

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