301N F22


Gas Law Stoichiometry Extra Practice


Part 1

Not all stoichiometry problems have to be limiting reagent problems. If the question defines that one of the reactant is in excess, you are being told that the limiting reagent is the other reactant. Use this to solve the first three warmup problems.

N2(g) + 3H2(g) → 2NH3(g)

  1. When 3.00 moles of N2 react with excess hydrogen, how many moles of NH3 are formed?
  2. When 8.59 moles of H2 react with excess N2, how many moles of NH3 are formed?
  3. How many moles of H2 are needed to form 16.4 moles NH3 in the presence of excess N2?

Part 2

Using the following balanced chemical equation, solve for the total number of moles in the final reaction mixture for each set of starting amounts for the reagents. The reaction is run at 273.15 K and 1 atm pressure.

H2(g) + Cl2(g) → 2HCl(g)

  1. 4.00 moles of H2 and 8.00 moles Cl2
  2. 6.00 moles H2 and 4.00 moles Cl2
  3. 12.0 L H2 and 20.0 L Cl2

Part 3

Solve the next three questions using the following balanced chemical equation:

C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g)

  1. 12.6 L of C3H8 and 25.2 L of O2 react to completion. What is the final volume of all gases, assuming constant temperature and pressure?
  2. 1.35 moles of C3H8 and 8.51 moles O2 react to completion. What is the final volume if all the gases in the final reaction mixture are carefully stored at 400 K and 2.54 atm?
  3. This same reaction is run at a much colder temperature to ensure that the water produced by the reaction is in the liquid phase. Now you react 8.55 L of C3H8 with 18.5 L O2. What is the total volume of all species in the final reaction mixture?



CH301N · 51045 Chemistry In Our World I


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