Sucrose (C₁₂H₂₂O₁₁) is combusted in air according to the following reaction: C₁₂H₂₂O₁₁(s) + O₂(g) → CO₂(g) + H₂O(l) How many moles of carbon dioxide would be produced by the complete combustion of 15.6 grams of sucrose in the presence of excess oxygen?

What is the mass in grams of CO₂ that can be produced from the combustion of 4.06 moles of butane according to this equation: 2 C₄H₁₀(g) + 13 O₂(g) → 8 CO₂(g) + 10 H₂O(g)

What mass of oxygen is needed for the complete combustion of 3.70×10−3 g of methane?

Hydrocarbons such as propane burn in oxygen gas to produce heat. The balanced equation below shows the complete combustion of propane in oxygen. C3H₂(g) +50₂(g) → 3C0₂(g) + 4H₂O(g) How many moles of O₂ would be needed to cause the complete combustion of 3.00 g C3H8? moles

For the reaction C + 2H2 → CH4, how many grams of hydrogen are required to produce 5.8 moles of methane, CH4 ?

What mass of water is produced from the complete combustion of 4.70*10-3 g of methane?

0.300 g of Fe3O4 reacts with excess O₂ to give Fe₂O3 in 26.0% yield according to the following balanced equation. 4Fe3O4(s) + O₂(g) 6Fe₂O3(s) → Calculate the theoretical yield of Fe₂O3. g Calculate the actual yield of Fe2O3. g

Complete combustion of 4.10g of a hydrocarbon produced 13.3g of CO2 and 4.10g of H2O. What is the empirical formula for the hydrocarbon?

What is the mass in grams of CO₂ that can be produced from the combustion of 2.45 moles of butane according to this equation: 2 C₄H₁₀(g) + 13 O₂(g) → 8 CO₂(g) + 10 H₂O(g)

What is the mass in grams of CO₂ that can be produced from the combustion of 6.54 moles of butane according to this equation: 2 C₄H₁₀(g) + 13 O₂(g) → 8 CO₂(g) + 10 H₂O(g)