2Pb(NO3)2 (s) = 2PbO(s) + 4NO2 (g) + O2 (g) a) If oxygen is added to the system

Question

2Pb(NO3)2 (s) = 2PbO(s) + 4NO2 (g) + O2 (g)

a) If oxygen is added to the system at equilibrium, how will the concentration of nitrogen be affected? Why?

b) How will the amount of lead (II) nitrate in the container be affected by the removal of oxygen? Why?

c) How will the addition of lead (II) oxide to the system at equilibrium affect the equilibrium concentration of nitrogen dioxide? Why?

d) This system is endothermic, what effect would an increase in temperature have on the rate of the forward reaction? Would the equilibrium constant increase or decrease?

Explanation / Answer

2Pb(NO3)2 (s) -------> 2PbO(s) + 4NO2 (g) + O2 (g)

conc of products are increases the equilibrium shift to left side.

a.If oxygen is added to the system at equilibrium,the conc of products decreases the equilibrium shift to left side. So conc of nitrogen is decreases.

b.The conc of products are decreases the equilibrium shift to right side.The removal of oxygen theequilibrium shift to right side.So the amount of Pb(NO3)2 is decreases.

c.conc of products are increases the equilibrium shift to left side..If is added to the system at equilibrium,the conc of products decreases the equilibrium shift to left side. So conc of nitrogendioxide is decreases.

d.Edothermic reaction is takes place the high temperature. This system is endothermic, increase in temperature have on the rate of the forward reaction is increases.

The equilibrium constant increase with temperature.

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