Using the equation:2C4H10+13O2——> 8CO2+10H2O

If you produce 11.2g of water,how many liters of carbon dioxide are produced at 9.3 atm and 300*K?

Butane is used as a fuel in gas grills, and produces heat by the following reaction. 2C4H10(g) + 13O2(g) ĺ 8CO2(g) + 10H2O(l), ǻH°rxn= –5,314 kJ/mol. How many liters of CO2 are produced per 1.00 × 10^4 kJ of heat released? Assume STP and show all work

For the chemical reaction 2C₄H₁₀(g) + 13O₂(g) → 8CO₂(g) + 10H₂O(ℓ) assume that 10.6 g of C₄H₁₀ reacts completely to products. The density of CO₂ is 1.96 g/L. What volume in liters of CO₂ is produced?

For the reaction:

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

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