Outline the steps needed to determine the limiting reactant when 27.4 g of propane, C3H8, is burned with 77.9 g of oxygen. Step 1: Write the balanced reaction equation. (Omit states-of-matter from your answer. Use the lowest possible whole number coefficients Step 2: Calculate the molar masses.Step 3: Determine the limiting reactant.Step 4: Calculate the theoretical yield of CO2 in grams

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Patrina SchowalterLv2

13 Dec 2019

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24.âLimiting Reagent problems, including Stoichiometry, Actual yield, Theoretical yield and Percent yield.

âA. I react 5.0 grams of propane, C3H8, with excess oxygen to produce water and carbon dioxide. Produce the balanced combustion equation of propane and determine the theoretical yield of water. If only 6.8 grams of water are produced what is the percent yield of water?

B. A 2.00 g sample of ammonia is mixed with 4.00 g of oxygen. Which is the limiting reagent and how much excess reactant remains on completion of the reaction? What is the theoretical yield of NO. The equation below represents this reaction. ____ NH3(g) + ____ O2(g) Â® ____ NO(g) + ____ H2O(g)

âC. If 23.54 grams of nitrogen is reacted with 11.14 grams of hydrogen. Balance the following reaction. What is the theoretical yield of this reaction and which component is the limiting reagent? If only 8.26 grams of ammonia are produced what is the percent yield? ____ N2(g) + ____ H2(g) Â® ____ NH3(g)

A 16.0 gram sample of propane gas (C³H⁸) is burned according to the equation C₃H₈(g) + 5O₂(g) â 3CO₂(g) + 4H₂O(g).

In an enclosed container with a volume of 2.25L at a temperature of 322K.

If the sample of propane burns completely and no oxygen remains in the container, calculate the mole fractions of CO₂ and H₂O.

Calculate the total pressure in the container after the reaction.

Calculate the partial pressure of CO₂ and H₂O in the container after the reaction.

If 12.1 grams of propane is burned in the presence of 10.2 atm of oxygen at the above temperature and volume conditions, determine the theoretical yield of H₂O.