For the following reaction 6 experiments have been run and the data collected is in the following table: 2 MnO4-(aq) + 5 H2C2O4 (aq) + 6 H+ (aq) ---> 2 Mn2+ (aq) + 10 CO2 (g) + 8 H2O (l) Experiment [MnO4-], M [H2C2O4], M [H+], M Rate, M/s 1 0.2410 0.3470 0.2690 0.1147 2 0.3260 0.6210 0.2270 0.2776 3 0.5630 0.5740 0.7420 0.4431 4 0.2410 0.3470 0.3840 0.1147 5 0.4140 0.5740 0.5610 0.3258 6 0.3260 0.4930 0.4910 0.2203 a) Write the rate expression. _____________ b) Calculate the rate constant, k. __________________ c) If the concentration of MnO4-,H2C2O4, & H+ are 0.155 M, 0.293M, and 0.475M respectively, what is the rate of the reaction? ____________________

The value of ArxnH° is 12.93 kJ/mol at 850 K for H₂ (g) + 12 (g) = 2 HI(g) (a) Assuming that ArxnH° is independent of temperature, compute Kp at 700 K given that it is 29.1 at 1000 K. (b) Under this same assumption (constant ArxnHᵒ), at what temperature would you predict that the equilibrium constant for this reaction would have the value Kp = 20?

13.86. The rate constant for the reaction NO₂(g) + O3(g) → NO3(g) + O₂(g) was determined over a temperature range of 40 K, with the following results: T (K) 203 213 223 233 243 k (M¹s¹) 4.14 X 105 7.30 X 105 1.22 X 106 1.96 X 106 3.02 X 106 a. Determine the activation energy for the reaction. b. Calculate the rate constant of the reaction at 300 K.

Please answer ALL parts of the question and show your work. Consider this reaction: N2(g) + 3H2(g)  <------>  2NH2(g)          H= -123kJ Describe how the concentration of H2 will be affected by each of the following changes to the system at equilibrium. Will it increase, decrease, or not change? (a) The volume of the reaction chamber is decreased (b) Helium gas is added to the reaction chamber (c) The temperature is increased (d) N2 has is added to the reaction chamber