Consider the reaction: 3NO (g) <--> NO 2(g) +N 2 O (g) H = -156 kJ How will this

Question

Consider the reaction:
3NO(g) <--> NO2(g) +N2O(g)
H = -156 kJ
How will this system at equilibrium shift in the followingcases?
(a) Nitrogen oxide (NO) is added to the system. Answer:(left/right/no effect)
(b) The temperature of the reaction mixture is lowered. Answer:(left/right/no effect)
(c) The total pressure is increased by adding argon gas. Answer:(left/right/no effect)
(d) Nitrogen dioxide (NO2) is removed from the system. Answer:(left/right/no effect)
(e) Nitrous oxide (N2O) is added to the system. Answer:(left/right/no effect)
(f) The volume of the reaction container is doubled. Answer:(left/right/no effect)

Explanation / Answer

      a) Nitrogen oxide (NO) isadded to the system. - equilibrium shifts to right            b) The temperature of thereaction mixture is lowered. - equilibrium shifts to right                 c) The total pressure isincreased by adding argon gas - equilibrium shifts to right       d) Nitrogen dioxide (NO2) isremoved from the system. - equilibrium shifts to right       e) Nitrous oxide (N2O) is addedto the system - equilibrium shifts to left       f)  The volume of thereaction container is doubled. - equilibrium shifts to left According to Lechatlier's principle , for an exothermicreaction the decrease in temperature will favour the forwardreaction. The increase in pressure will shift the equilibriumtowards less number of moles. The increase in voume ( decrease inpressure) shift the equilibrium towards more number of moles. Theincrease in the concentration of reactants shift theequilibrium towards products. The increase in the concentration ofproducts shift the equilibrium towards reactants.

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