A balloon carries 40.0 gallons of liquid propane (density 0.5005 g/L). What volume of CO2 and H2O gas is produced by the combustion of this propane? (C3H8 + 5O2>> 3CO2 + 4H2O

utane, C4H10C4H10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is 2C4H10(g)+13O2(g)→8CO2(g)+10H2O(l)2C4H10(g)+13O2(g)→8CO2(g)+10H2O(l) At 1.00 atmatm and 23 ∘C∘C, what is the volume of carbon dioxide formed by the combustion of 4.00 gg of butane? Express your answer with the appropriate units.

The human body burns glucose (C6H₁2O6) for energy according to this chemical reaction: C6H12O6 +60₂-6CO₂ + 6H₂O The products of the reaction are carbon dioxide (CO₂) and water (H₂O). Interestingly, all of the carbon dioxide and much of the water exits the body through the lungs: on every breath, the average person exhales 500. mL of air, which is typically enriched to 4% CO₂ and 5% water vapor by volume. In short, when a person loses weight by dieting, the weight that is lost actually departs his body as a gas, every time he exhales. Each kilogram of body fat lost requires exhaling about 2.9 kg of carbon dioxide. Calculate how many breaths it takes an average person to "exhale" 1.00 kg of fat. Round your answer to the nearest thousand. You'll need to know that the density of CO₂ is 2.0 kg/m³. 0 ☐ ☐x10 X

Aspirin (C9H8O4) is synthesized by reacting salicyclic acid (C7H6O3) with acetic anhydride (C4H6O3). The chemical equation is:C7H6O3 + C4H6O3  C9H8O4 + HC2H3O2a. If we react 100. g of acetic anhydride with 100. g of salicyclic acid, what mass of aspirin do we expect to produce? (theoretical yield)b. If the percent yield comes out to 84%, what mass of aspirin did the reaction actually produce? (what is the actual yield?)

The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane (C8H18)(C8H18) and calculate how many kilograms of carbon dioxide are added to the atmosphere per 8.7 kgkg of octane burned. ( HintHint: Begin by writing a balanced equation for the combustion reaction.)

2C4H10 + 13O2 = 8CO2 + 10H2O How many grams of CO2 are produced by burning 9.41 g of C4H10?

Consider the following balanced chemical reaction: HNO3 + 3H2 → NH2OH + 2H2O If 25.0 grams of HNO3 were mixed with 8.70 grams of H2 gas, how many grams of the excess reagent (i.e. either H2 or HNO3) would remain once the reaction is complete?  Molar mass of HNO3 = 63.01 g/mol Molar mass of NH2OH = 33.03 g/mol

2H2(g) + O2(g) -> 2H2O(g) Calculate the mass (in grams) of water vapor produced when 56.0 g of pure hydrogen gas burns in air.

The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane (C8H18)(C8H18) and calculate how many kilograms of carbon dioxide are added to the atmosphere per 4.2 kgkg of octane burned. ( HintHint: Begin by writing a balanced equation for the combustion reaction.)