What is the theoretical yield of product obtained in the reaction of 3 moles of propene with excess amount of hydrogen gas, using a Pt-Al2O3 catalyst at 343K, given the following balanced equation:

C3H6 + H2 --> C3H8

The reaction is known to follow first order kinetics with rate constant of 0.025 L/mol*s at 343K. What will be the conversion of propene after 15 minutes of reaction time and what will be the corresponding yield of product propane?

A reaction follows first-order kinetics, with a rate constant of 4.49 ✕ 10^−4 s^−1. If the initial concentration of the reactant is 1.59 ✕ 10^−1M, what will be the concentration after 10.0 minutes of reaction?

------- M??

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

​A. 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) ® ____ NO(g) + ____ H2O(g)

​C. 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) ® ____ NH3(g)

The theoretical yield of a reaction is the amount of product obtained if the limiting reactant is completely converted to product. Consider the reaction: 2 CO(g) + O2(g) → 2 CO2(g) If 19.8 g CO is mixed with 14.06 g O2, calculate the theoretical yield (g) of CO2 produced by the reaction.