2c4h10(g)+13o2(g)→10h2o(g)+8co2(g); molar mass of butane 58.12g/mol calculate the mass of butane needed to produce 90.9 g of carbon dioxide. calculate the mass of butane needed to produce 90.9 g of carbon dioxide.

Answer : The mass of Butane needed is 29.946 g.

Solution : Given,

Molar mass of butane = 58.12 g/mole

Molar mass of carbon dioxide = 44.01 g/mole

Mass of carbon dioxide = 90.9 g

The Given net balanced chemical reaction is,

First we have to calculate the moles of carbon dioxide.

From the given chemical reaction, we conclude that

8 moles of produced from 2 moles

2.061 moles of produced from of

The moles of = 0.51525 moles

Now we have to calculate the mass of needed.

Mass of Butane = Moles of Butane × Molar mass of Butane

Mass of Butane = 0.51525 moles × 58.12 g/mole = 29.946 g

Therefore, the mass of Butane needed is 29.946 g.

fe 55.85 g/mol and h2o 18.02 g/mol.

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