55. Given: 2A(g) <=> B(g) + C(g) ΔH° = +27 kJ, K = 3.2 x 10^-4.

Which of the following would be true if the temperature were increased from 25°C to 100°C?

1. The value of K would be smaller.

2. The concentration of A(g) would be increased.

3. The concentration of B(g) would increase.

42. The energy profiles for four different reactions are shown. Which reaction requires the most energetic collisions to reach the transition state?

3. Which of the following are equal for a chemical system at equilibrium?

8. If the reaction quotient Q has a smaller value than the related equilibrium constant, K, __________

The activation energy for the reaction in which CO₂ decomposes to CO and a free radical oxygen atom, O, has an activation energy of 37,8 kJ/mol. The frequency factor is 1,6x10⁷s^-1. What is the rate constant (s^-1) for this reaction at 298 K?

58. Given: A(s) + B(l) <=> C(g) + D(g) ΔH° = 84.3 kJ.

If the above reactants and products are contained in a closed vessel and the reaction system is at equilibrium, the number of moles of C can be decreased by which of the following? (Note that the reactants are solid and liquid.)

The following rate constants were obtained in an experiment in which the decomposition of gaseous N₂O₅ was studied as a function of temperature. The products were NO₂ and NO₃.

   T (^oC)           k (s^-1)       

   47            0,45

   81            7,0

Determine the rate constant (s^-1) for this reaction at 149 ^oC.  

47. Which of the following occurs when reactants are added to a chemical reaction in solution or the gas phase at equilibrium?

44. The following energy profiles for four different reactions are shown. Which reaction is the most exothermic?

57. Given the following reaction at equilibrium, which of the following alterations will increase the amount (in moles) of SO2Cl2:

SO2(g) + Cl2(g) <=> SO2Cl2(g) ΔH° = -67 kJ