Butane, C4H10, reacts with oxygen, O2, to form water, H2O, and carbon dioxide, CO2, as shown in the following chemical equation: 2C4h10 (g) + 13O2 (g) - >10H2O (g) + 8CO2 (g)

Calculate the mass of water produced when 1.77 grams of butane reacts with excessive oxygen?

Calculate the mass of butane needed to produce 71.6 of carbon dioxide.

The balanced chemical reaction is:

2C4H10 (g) + 13O2 (g) - >10H2O (g) + 8CO2 (g)

Calculate the mass of water produced when 1.77 grams of butane reacts with excessive oxygen?

1.77 g C4H10 (1 mol C4H10/58.14 g C4H10) (10 mol H2O / 2 mol C4H10) (1.01 g H2O / 1 mol H2O) = 0.15 g H2O

Calculate the mass of butane needed to produce 71.6 of carbon dioxide.

71.6 g CO2 (1 mol CO2 / 44.01 g CO2) (2 mol C4H10 / 8 mol CO2) (58.14 g C4H10 / 1 mol C4H10) = 23.65 g C4H10