2HI(g) --> I2(g) + H2(g) Base your answers on the reaction and data shown below. All components are in the gas phase. Expt. Temperature Initial [HI] Initial Rate (M s-1) 1 750 K 0.1 M 1.51E-04 2 750 K 0.3 M 1.36E-03 3 900 K 0.2 M 8.72E-02 1) Write the overall rate expression for this reaction, based on the data in the table. What order is the reaction? Explain briefly. 2) What is the rate constant (k) at 750 K and at 900 K? Be sure to include units.
Questions 3-9, these are different parts of one giant question
2HI(g) --> I2(g) + H2(g)
Base your answers on the reaction and data shown below. All components are in the gas
phase.
Expt. Temperature Initial [HI] Initial Rate (M s-1)
1 750 K 0.1 M 1.51E-04
2 750 K 0.3 M 1.36E-03
3 900 K 0.2 M 8.72E-02
1) Write the overall rate expression for this reaction, based on the data in the table.
What order is the reaction? Explain briefly.
2) What is the rate constant (k) at 750 K and at 900 K? Be sure to include units.
3) What is the energy of activation (Ea) for this reaction, reported in kJmol?
4) What would be the rate at 625 K, using a starting concentration of 0.20 M HI?5) What is the equilibrium constant Kc for the reaction written as above under the
following conditions: The reaction was initiated by placing 5.000 x 10-3 moles of H2 and
1.000 x 10-3 moles of I2 in a 5.00 L flask, at 448°C. It has come to equilibrium and the experimenters found 1.87x10-3 moles of HI. Be sure to show both the form of the equilibrium expression and the ICE table needed to solve this.
6) In which direction would the reaction proceed to reach equilibrium if the concentrations of the species were 1.0 x 10-2 M HI, 5.0 x 10-3 M H2, and 1.5 x 10-2 M I2? Assume the equilibrium constant that you calculated above, and leave other conditions unchanged (448°C, 5.0 L flask). Show your work, and explain briefly.
7) Using the values from Appendix G of the text, calculate the ΔG°, the ΔH° and the ΔS° for this reaction as written above.
8) From the standard values above, calculate the theoretical equilibrium constant at 448°C.
9) Is it possible for this reaction to change from spontaneous to non-spontaneous or the opposite by changing the temperature? Explain briefly.
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