Reaction  BaO2(s)   ⇌   BaO(s)  +  O2(g);  ∆H=+ve. In equilibrium condition, pressure of O2 depends on

BaO2(s)   ⇌   BaO(s)  +  O2(g);    ∆H=+veAccording to the law of mass action, the rate of forward reaction = r1r1 ∝  BaO2    or    r1 =k1  BaO  But concentration of solid = 1, then  r1 =k1Similarly the rate of backward reaction = r2r2 ∝  BaO  O2   or    r2 =k2  BaO  O2∵    conc. of BaO=1or     r2 =k2 O2At equilibrium, r1 = r2 k1 =k2 O2   or     k1 =k2.  pO2where, pO2 = partial pressure of O2or   k1k2 = pO2 (equilibrium constant)∵     k1k2 = k    or    pO2So, from the above it is clear that pressure of O2 does not depend upon the concentration of reactants. The given equation is an endothermic reaction. It the temperature of such reaction is increased, then dissociation of BaO2 would increase, and more O2 is produced.