Problem PageQuestion Liquid hexane will react with gaseous oxygen to produce gaseous carbon dioxide and gaseous water . Suppose 6.9 g of hexane is mixed with 17.3 g of oxygen. Calculate the maximum mass of water that could be produced by the chemical reaction. Round your answer to significant digits.

The maximum mass of water that could be produced by the chemical reaction is 10.1 g

Explanation:

The equation of reaction involves the combustion of 2 moles of hexane (C6H14) with 19 moles of oxygen (O2) to produce 12 moles of carbon dioxide (CO2) and 14 moles of water (H2O)

From the equation of reaction above,

2 moles of C6H14 (172 g) produced 14 moles of H2O (252 g)

6.9 g of C6H14 would produce (6.9×252/172) = 10.1 g of water (to 3 significant figures)

Also, from the equation of reaction,

19 moles of O2 (608 g) produced 14 moles of H2O (252 g)

17.3 g of O2 would produce (17.3×252/608) = 7.17 g of water (to 3 significant figures)

Maximum mass of water produced = 10.1 g

3.2x10^7