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Using Le Chatelier’s principle, predict the direction of the net reaction in each of the following equilibrium systems, as a result of increasing the pressure at constant temperature. a. N_2 (g) + O_2 (g) 2 NO(g) b. PCl_5 (g) PCl_3 (g) + Cl_2 (g) c. CO(g) + Cl_2 (g) COCl_2 (g) What effect (shift to the right or left) does an increase in temperature have on each of the following systems at equilibrium? a. 3 O_2 (g) 20_3 (g) delta H = 284 kJ b. 2SO_3 (g) + O_2 (g) 2SO_3 (g) delta H = – 198.2 kJ
Expert Answer
when there is increase in pressure equilibrium shift towards fewer moles of gas
2 a difference of moles btween right and left side is zero so it will have no effect
2b it will shift towards left because it has less no of moles
2 it will shift towards right because it has less no of moles
3 a H>0 so its endothermic it will shift towards right in increase in temp
3 b H<0 so its exothermic it will shift towards left in increase in temp
its because in endothermic energy is needed in favour of reaction so it will recieve more energy to move forward
in exothermic energy is released .
