Calculate the mass of butane needed to produce 61.9 g of carbon dioxide

20.4g

Explanation:

First, we need to write a balanced equation for the reaction of butane to produce carbon dioxide.

When butane undergo Combustion, it will produce carbon dioxide and water as shown below:

2C4H10 + 13O2 —> 8CO2 + 10H2O

Molar Mass of C4H10 = (12x4) + (10x1) = 48 + 10 = 58g/mol

Mass of C4H10 from the balanced equation = 2 x 58 = 116g

Molar Mass of CO2 = 12 + (2x16) = 12 + 32 = 44g/mol

Mass of CO2 from the balanced equation = 8 x 44 = 352g

From the equation,

116g of C4H10 produced 352g of CO2.

Therefore, Xg of C4H10 will produce 61.9g of CO2 i.e

Xg of C4H10 = (61.9 x 116)/352 = 20.4g

Therefore, 20.4g of butane(C4H10) is needed to produce 61.9g of CO2

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