For the following reaction determine if the described changes will shift the equilibrium to the right, left, will have no effect, or if the effect cannot be determined. 4 NH3(g) + 5 O2(g)   4 NO(g) + 6 H2O(g)           ΔH° = –904 kJ Changes: (a) Adding more water vapor (b) Increasing the temperature (c) Increasing the volume of the reaction vessel (d) Removing O2(g) (e) Adding 1 atm of Ne(g) to the reaction vessel

According to LeChatelier's principle, when the reaction quotient is less than the equilibrium constant of a reaction, the reaction: A must shift toward products to reach equilibrium. B must shift toward reactants to reach equilibrium. (c) results in an increase in standard enthalpy of formation of reactants. results in an increase in standard enthalpy of formation of products.

1 HgO(s) + 2 I−(aq) + H2O(l) ⇄  HgI2(g) + 2 OH−(aq)   ;    ∆H < 0 Consider the equilibrium above. Which of the following changes will increase the concentration of HgI2? (A) Increasing the concentration of OH−         (B) decreasing the pressure (C) Increasing the mass of HgO present      (D) Increasing the temperature           (E) Adding a catalyst 2 In which of the following systems would the equilibrium NOT be shifted by a change in the volume of the system at constant temperature? (A) CO(g) + NO(g) ⇄ CO2(g) + 1/2 N2(g)         (B) N2(g) + 3 H2(g) ⇄ 2 NH3(g) (C) N2(g) + 2 O2(g) ⇄ 2 NO2(g)                       (D) N2O4(g) ⇄ 2 NO2(g)                                        (E) NO(g) + O3(g) ⇄ NO2(g) + O2(g) 3. What substance is missing in the following reaction mechanism? Step 1           NO  +  ___   à  OONO                                                          Step 2        NO  +  OONO  à  2NO2…

The Keg for the equilibrium below is 7.52 · 102 at 480.0 °C. 2Cl2 (g) + 2H2O (g) = 4HCI (g) + O2 (g) What is the value of Keg at this temperature for the following reaction? HCI (g) + 1/202 (g) = 1/2C12 (g) + 1/2H2O (g) 1.91 7.52. 10-2 1.88x10-2 0.524