How many liters of oxygen at STP are produced from 175 grams of water? 2 C4h10 + 13 02 → 8 C02 + 10 H120

Answer

282 L

Convert 175 grams of water to moles. A: 175 g H2O = 9.72 moles H2O (molecular weight of water is 18 g/mol)
Determine limiting reactant. Since we're only given the amount of water, we need to convert it to moles of O2 using the balanced equation. 2 C4H10 + 13 O2 → 8 CO2 + 10 H2O. A: 9.72 moles H2O x (13/10) moles O2 per mole H2O = 12.6 moles O2.
Calculate volume of O2 at STP. 1 mole of any ideal gas at STP (Standard Temperature and Pressure) takes up a volume of 22.4 L. A: 12.6 moles O2 x 22.4 L/mol = 282.24 L
Round to the appropriate number of significant figures. A: 282 L of O2 at STP.