**Question **# 5) For each of the following reactions, predict the shift in equilibrium if the temperature of the system is increased: \text { a) } \mathrm{N}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \leftrightarrows 2 \mathrm{NO}(\mathrm{g}) \text { b) } 2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \leftrightarrows 2 \mathrm{SO}_{3}(\mathrm{~g}) 1. Describe 2 of the four conditions that apply to all equilibrium systems. (2 marks) 2. a) Write an equilibrium expression for the following reaction. (1 mark) \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{NO}_{2}(\mathrm{~g}) \leftrightarrows \mathrm{NO}(\mathrm{g})+\mathrm{SO}_{3}(\mathrm{~g}) b) If the concentration of SO2 and NO2 gas in a flaskare both 0.055mol/L, is the system at equilibrium? Ifnot, which direction will it shift to achieveequilibrium? 3. For the reaction given below, determine which direction the system will shift (if at all) in response to the given stresses. 2 \mathrm{H}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \leftrightarrows 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \leftrightarrows \Delta \mathrm{H}=- 241kJ/mol a) Increasing temperature b) Decreasing pressure c) Adding carbon monoxide gas d) Adding an inert gas d) Adding an inert gas