Required
1. Which of the following represent proper K expressions? Check all that apply.
2. The equilibrium constant expression can be derived empirically by measuring equilibrium concentrations of reactants and products. It can also be determined theoretically by assuming that reaction rates are equal in the forward and reverse direction at equilibrium. Since both the observed result, and the theoretical prediction are the same, what can we conclude about the theory of equal reaction rates in opposing directions at equilibrium?
3. The reaction N2O4 (g) 2NO2 (g) is endothermic. Based on this information, you would expect the value of K for this reaction to a) increase as the temperature increases. b) decrease as the temperature increases. c) be unaffected by a temperature increase.
4. You must always makes sure that the concentrations in the equilibrium row of an IRE table are in the same proportion as the balanced equation coefficients. True False
5. At a certain temperature, a container is filled with CH4 and H2S. It is heated to 1000 K, and allowed to reach an equilibrium. The concentrations of each substance at equilibrium are found to be:
What is the value of K for the reaction 2H2S (g) + CH4 (g) 4 H2 (g) + CS2 (g)?
6. If you started with an empty 1 litre container, put in 0.1 mole of HI (g) and let it react according to this equation:
then when the reaction reached an equilibrium at a temperature where K = 1.62 x 10-2, the concentrations of all reacting species would be: [HI] = [H2] = [I2] =
7. Kc for the Sabatier reaction CO2 (g) + 4 H2 (g) CH4 (g) + 2H2O (g) is 4.25 x 10-2 at 450 oC. If 1 mol/L of CO2 and 0.1 mol/L of H2 are the input concentrations into a Sabatier reactor at this temperature, then what will the equilibrium concentrations be of each reacting species? Hint: use an iterative method to solve this problem. [CO2] = [H2] = [CH4] = [H2O] =
8. In the Sabatier reaction at 800 K, the value of Kc = 1.88 x 10-3. If at these conditions, the [CO2] = 0.910, [H2] = 0.172, and [CH4] = 6.00 x 10-3 mol/L, then at the equilibrium CO2 (g) + 4 H2 (g) CH4 (g) + 2H2O (g), what is [H2O]? [H2O] =
9. If some Ba(OH)2 (s) is dissolved in water to form a saturated solution, which of the following represents the Ksp expression?
10. It takes 23.25 mL of the above saturated solution of Ba(OH)2 to neutralize 50.0 mL of 0.100 HCl. What is the value of the Ksp for Ba(OH)2 (s)?