6a) How does the shape of the shape of the response curve (partial pressure vs. time) change with increasing reaction order?

a) Faster slope earlier, followed by a long slower tail b) Slower slope earlier, followed by a faster slope c) Does not change with reaction order 6b) Were you able to find this graph?

7a) If the rate constant k doubles, what happens to the time taken to complete the reaction?

a) Takes twice as long to complete the reaction b) Takes half as long to complete the reaction

7b) In order to answer the question, you must change some parameters. Run the reaction twice to get two rates. Record your parameters and the rates you obtained.

7c) Explain, mathematically, why this is the case. Hint: look at the rate law and remember how rate is defined.

8a) If the rate constant k is cut in half, what happens to the time taken to complete the reaction?

a) Takes twice as long to complete the reaction b) Takes half as long to complete the reaction

8b) Again, in order to answer the question, you must change some parameters. Run the reaction twice to get two rates. Record your parameters and the rates you obtained.

8c) Explain, mathematically, why this is the case. Hint: look at the rate law and remember how rate is defined.

9a) Set up the reaction for the synthesis of ammonia: N2 (g) + 3H2 (g) 2NH3 (g). Set the initial partial pressures: Pi(N2) = 1 bar, Pi(H2) = 3 bar, Pi(NH3) = 0. Let the temperature and pressure factor be at the default values of 298.15K and 1.0. Using a first-order rate model (k=1, X=0, Y=1), what is the approximate half-life of H2 based on the kinetics tables produced by ChemReaX:

a) 0.2 second b) 0.23 second c) 0.35 second d) 0.4 second