Elementary unimolecular reaction have first order rate laws, elementary bimolecular reaction have second order rate laws. A rate law is often derived from a proposed mechanismby imposiing the steady state approximation by assuming that there in pre equilibrium A proposal mechanism must be constant with the experimental rate law. The decomposition of O_(3) obeys the mechanism given below, Step 1: O_(3)hArrO_(2)+(O)- fast Step 2: O_(3)+(O)toO_(2)+O_(2)- slow H_(2)+Br_(2)to2HBr Mechaism : Br_(2)hArr2Br (fast) H_(2)+brtoHBr+H(slow) H+BrtoHBR (Fast) Order of the reaction is

Elementary unimolecular reaction have first order rate laws, elementar

1.	Elementary unimolecular reaction have first order rate laws, elementary bimolecular reaction have second order rate laws. A rate law is often derived from a proposed mechanismby imposiing the steady state approximation by assuming that there in pre equilibrium A proposal mechanism must be constant with the experimental rate law. The decomposition of O_(3) obeys the mechanism given below, Step 1: O_(3)hArrO_(2)+(O)- fast Step 2: O_(3)+(O)toO_(2)+O_(2)- slow H_(2)+Br_(2)to2HBr Mechaism : Br_(2)hArr2Br (fast) H_(2)+brtoHBr+H(slow) H+BrtoHBR (Fast) Order of the reaction is
Answer» 0<BR>0.1 1.5 0.2 Solution :`K_(C)=([Br]^(2))/([Br_(2)])implies[B_(r)]=SQRT(K_(c).[Br_(2)]),r=K_(2).[H_(2)][B_(r)],r=K_(2).[H_(2)](K_(C))^(1/2).[Br_(2)]^(1/2),r=K.[H_(2)]^(1)[Br_(2)]^(1/2)`