Given the equation:
C2H6 (g) + O2 (g) → CO2 (g) + H2O (g) (not balanced)
Determine the number of liters of CO2 formed at STP when 891.6 grams of C2H6 is burned in excess oxygen gas.
Your answer should be numerical and neglect units (e.g., if you calculate 3.5L then input 3.5).

The volume of CO₂ produced at STP when 891.6 grams of C2H6 is burned in excess oxygen gas is 1331.4 liters.What is the volume in liters of CO₂ produced when  891.6 grams of C2H6 is burned in excess oxygen gas?The volume of a gas produced at STP is determined from the mole ratio of the reaction that produces the gas.The mole ratio of the reaction that produces the gas is obtained from the equation of the reaction.Considering the given data, the volume of CO₂ produced when  891.6 grams of C2H6 is burned in excess oxygen gas is calculated as follows:Equation of reaction: 2 C₂H₆ (g) + 7 O₂ (g) → 4 CO₂ (g) + 6 H₂O (g)2 moles of C₂H₆ when burned in excess oxygen at STP produces 4 moles of CO₂.The number of moles of C₂H₆ in 891.6 grams is calculated as follows:Moles = mass / molar massThe molar mass of C₂H₆ = 30 g/molMoles of C₂H₆ in 891.6 g = 891.6 / 30Moles of C₂H₆ = 29.72 molesHence moles of CO₂ produced = 29.72 * 4/2 molesVolume of 1 mole of CO₂ at STP = 22.4 litersVolume of CO₂ produced = 29.72 * 4/2 * 22.4Volume of CO₂produced = 1331.4 liters.Learn more about gas volume at STP at: https://brainly.com/question/28717703#SPJ1