Propane (C3H8) burns in oxygen to produce carbon dioxide and water. C 3 H 8 (g)+5O 2 (g)→3CO 2 (g)+4H 2 O(g) Calculate the mass of CO 2 that can be produced if the reaction of 45.0 g of propane and sufficient oxygen has a 60.0% yield

Nitric Oxide can be made from the oxidation of ammonia as shown below. A reaction between 8.5 g of NH3 and 25.0 g of O₂ produces 12.0 g of NO. What is the percent yield for this reaction? 4 NH3(g) + 5O₂(g) → 4 NO(g) + 6 H₂O(g) Molar masses (in g mol-¹): NH3 17.034, 0₂ 32.00, NO 30.01, H₂O 18.016

What is the mass in grams of NO that will be produced from 22.9 g of NO, reacted with excess water in the following chemical reaction? 3 NO2(g) + H,0(1) → 2 HNO3(g) + NO(g) 2 ΗΝΟ:

The combustion of methane is shown in the following reaction:CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) A) If 15.0 moles of CO2(g) is produced, how many moles of methane are required? B) If 20.0 moles of O2(g) are consumed, how many moles of water are produced?