1. Given the equilibrium reaction: N2(g) + O2(g) <---> 2NO(g) deltaH=180kJ mol-1 State the effect of each of the following potential stresses on the system: A) Temperature is decreased B) The pressure of the container is decreased, keeping volume constant C) A catalyst is added D) NO is removed as it forms E) Argon gas is added to the container 2. A) A shift to the left will occur, considering the enthalpy of reaction. B) Not sure about this one, as the only way to accomplish this is to remove particles from the container. My best guess is that, assuming an equal quantity of reactants vs. products is removed, there will be no shift as the ratio of moles of reactant to moles of product is 1:1. C) No change, as the catalyst will catalyze both the forward and reverse reactions equally. D) Shift to the right, as product collisions decrease as NO is removed. E) No change, as the argon will increase the total pressure, but will not react in collisions.