\text { a. The rate of the reaction } 2 \mathrm{NO}_{2}(g) \rightleftharpoons \mathrm{N}_{2} \mathrm{O}_{4}(g) \text { is given by the rate law below: } \text { Rate }=\mathrm{k}\left[\mathrm{NO}_{2}\right]^{2} What would the rate of the reaction be under the following conditions? (4 points) \text { rate constant }=1.8 \times 10^{3}(\mathrm{~L} / \mathrm{mol}) / \mathrm{s} \left[\mathrm{NO}_{2}\right]=0.007 \mathrm{M} b. One step in the industrial production of hydrogen gas involves reacting C0 with steam according to the reaction CO(g) + H,0(g) = CO-(g) + H;(g). Heat is produced in this reaction, which is represented by the following diagram. Use the equation and diagram to answer the following questions. (12 points)

i. What would increasing the temperature do to the hydrogen yield? Explain your answer. ii. What would increasing the temperature do to the reaction rate? Explain your answer.points) iii. Label the activation energy on the energy diagram. (2 points) iv. This reaction is run using an iron catalyst. What would adding iron to the reaction do to the energy diagram? Explain your answer and draw the change on the energy diagram. (4points)