Answer:
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
