The rate and mechanism of chemical reactions are studied in chemical kinetics. The elementary reactions are single step reactions having no mechanism. The order of reaction and molecularity are same for elementary reactions. The rate of forward reaction `aA + bB rarr cC + dD` is given as :
rate = `=((dx)/(dt))=-(1)/(a) (d[A])/(dt) =-(1)/(b) (d[B])/(dt) =(1)/(c)(d[C])/(dt)=(1)/(d) (d[D])/(dt)` or rate `=K [A]^(a) [B]^(b)`. In case of reversible reactions net rate expression can be written as : rate `= K_(1)[A]^(a)[B]^(b) – K_(2)[C]^(c)[D]^(d)`. At equilibrium, rate = 0. The constants `K, K_(1), K_(2)`, are rate constants of respective reaction. In case of reactions governed by two or more steps reactions mechanism, the rate is given by the solwest step of mechanism.
For the reaction : `aA rarr bB`,
`log [(-dA)/(dt) ]=log [(dB)/(dt)]+0.6," then "a:b` is :
The rate and mechanism of chemical reactions are studied in chemical kinetics. The elementary reactions are single step reactions having no mechanism. The order of reaction and molecularity are same for elementary reactions. The rate of forward reaction `aA + bB rarr cC + dD` is given as :
rate = `=((dx)/(dt))=-(1)/(a) (d[A])/(dt) =-(1)/(b) (d[B])/(dt) =(1)/(c)(d[C])/(dt)=(1)/(d) (d[D])/(dt)` or rate `=K [A]^(a) [B]^(b)`. In case of reversible reactions net rate expression can be written as : rate `= K_(1)[A]^(a)[B]^(b) – K_(2)[C]^(c)[D]^(d)`. At equilibrium, rate = 0. The constants `K, K_(1), K_(2)`, are rate constants of respective reaction. In case of reactions governed by two or more steps reactions mechanism, the rate is given by the solwest step of mechanism.
For the reaction : `aA rarr bB`,
`log [(-dA)/(dt) ]=log [(dB)/(dt)]+0.6," then "a:b` is :
rate = `=((dx)/(dt))=-(1)/(a) (d[A])/(dt) =-(1)/(b) (d[B])/(dt) =(1)/(c)(d[C])/(dt)=(1)/(d) (d[D])/(dt)` or rate `=K [A]^(a) [B]^(b)`. In case of reversible reactions net rate expression can be written as : rate `= K_(1)[A]^(a)[B]^(b) – K_(2)[C]^(c)[D]^(d)`. At equilibrium, rate = 0. The constants `K, K_(1), K_(2)`, are rate constants of respective reaction. In case of reactions governed by two or more steps reactions mechanism, the rate is given by the solwest step of mechanism.
For the reaction : `aA rarr bB`,
`log [(-dA)/(dt) ]=log [(dB)/(dt)]+0.6," then "a:b` is :
A
`3.98`
B
`2.18`
C
`1.48`
D
0
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The rate and mechamical reaction are studied in chemical kinetics. The elementary reactions are single step reaction having no mechanism. The order of reaction and molecularity are same for elementary reactions. The rate of forward reaction aA + bBrarr cC+dD is given as: rate =((dx)/(dt))=-1/a(d[A])/(dt)=-1/b(d[B])/(dt)=1/c(d[C])/(dt)=1/d(d[D])/(dt) or expression can be written as : rate =K_(1)[A]^(a)[B]^(b)-K_(2)[C]^(c )[D]^(d) . At equilibrium, rate = 0 . The constants K, K_(1), K_(2) are rate constants of respective reaction. In case of reactions governed by two or more steps reaction mechanism, the rate is given by the slowest step of mechanism. For a hypothetical reaction aA+bBrarr Product, the rate law is: rate =K[A]^(x)[B]^(y) , then:
The rate and mechamical reaction are studied in chemical kinetics. The elementary reactions are single step reaction having no mechanism. The order of reaction and molecularity are same for elementary reactions. The rate of forward reaction aA + bBrarr cC+dD is given as: rate =((dx)/(dt))=-1/a(d[A])/(dt)=-1/b(d[B])/(dt)=1/c(d[C])/(dt)=1/d(d[D])/(dt) or expression can be written as : rate =K_(1)[A]^(a)[B]^(b)-K_(2)[C]^(c )[D]^(d) . At equilibrium, rate = 0 . The constants K, K_(1), K_(2) are rate constants of respective reaction. In case of reactions governed by two or more steps reaction mechanism, the rate is given by the slowest step of mechanism. At the point of intersection of the two curve shown for the reaction: Ararr nB the concentration of B is given by:
The rate and mechamical reaction are studied in chemical kinetics. The elementary reactions are single step reaction having no mechanism. The order of reaction and molecularity are same for elementary reactions. The rate of forward reaction aA + bBrarr cC+dD is given as: rate =((dx)/(dt))=-1/a(d[A])/(dt)=-1/b(d[B])/(dt)=1/c(d[C])/(dt)=1/d(d[D])/(dt) or expression can be written as : rate =K_(1)[A]^(a)[B]^(b)-K_(2)[C]^(c )[D]^(d) . At equilibrium, rate = 0 . The constants K, K_(1), K_(2) are rate constants of respective reaction. In case of reactions governed by two or more steps reaction mechanism, the rate is given by the slowest step of mechanism. For the reaction, aArarr bB , log[(-dA)/(dt)]=log[(dB)/(dt)]+0.6 , then a:b is:
The rate and mechamical reaction are studied in chemical kinetics. The elementary reactions are single step reaction having no mechanism. The order of reaction and molecularity are same for elementary reactions. The rate of forward reaction aA + bBrarr cC+dD is given as: rate =((dx)/(dt))=-1/a(d[A])/(dt)=-1/b(d[B])/(dt)=1/c(d[C])/(dt)=1/d(d[D])/(dt) or expression can be written as : rate =K_(1)[A]^(a)[B]^(b)-K_(2)[C]^(c )[D]^(d) . At equilibrium, rate = 0 . The constants K, K_(1), K_(2) are rate constants of respective reaction. In case of reactions governed by two or more steps reaction mechanism, the rate is given by the slowest step of mechanism. The rate of formation of SO_(3) in the following reaction, 2SO_(2)+O_(2)rarr 2SO_(3) is 10 g sec^(-1) The rate of disappearance of O_(2) will be:
The rate and mechamical reaction are studied in chemical kinetics. The elementary reactions are single step reaction having no mechanism. The order of reaction and molecularity are same for elementary reactions. The rate of forward reaction aA + bBrarr cC+dD is given as: rate =((dx)/(dt))=-1/a(d[A])/(dt)=-1/b(d[B])/(dt)=1/c(d[C])/(dt)=1/d(d[D])/(dt) or expression can be written as : rate =K_(1)[A]^(a)[B]^(b)-K_(2)[C]^(c )[D]^(d) . At equilibrium, rate = 0 . The constants K, K_(1), K_(2) are rate constants of respective reaction. In case of reactions governed by two or more steps reaction mechanism, the rate is given by the slowest step of mechanism. For a reaction, 2ND_(3)rarrN_(2)+3D_(2) , (-d[ND_(3)])/(dt)=K_(1)[ND_(3)], (d[N_(2)])/(dt)=K_(2)[ND_(3)] (d[D_(2)])/(dt)=K_(3)[ND_(3)] , then:
The rate and mechamical reaction are studied in chemical kinetics. The elementary reactions are single step reaction having no mechanism. The order of reaction and molecularity are same for elementary reactions. The rate of forward reaction aA + bBrarr cC+dD is given as: rate =((dx)/(dt))=-1/a(d[A])/(dt)=-1/b(d[B])/(dt)=1/c(d[C])/(dt)=1/d(d[D])/(dt) or expression can be written as : rate =K_(1)[A]^(a)[B]^(b)-K_(2)[C]^(c )[D]^(d) . At equilibrium, rate = 0 . The constants K, K_(1), K_(2) are rate constants of respective reaction. In case of reactions governed by two or more steps reaction mechanism, the rate is given by the slowest step of mechanism. For the reaction, A+2B hArr AB_(2) , the rate of forward reaction is (dx)/(dt)=1xx10^(5)[A][B]^(2)-1xx10^(4)[AB_(2)] . The rate constants for forward and backward reactions are:
The rate and mechamical reaction are studied in chemical kinetics. The elementary reactions are single step reaction having no mechanism. The order of reaction and molecularity are same for elementary reactions. The rate of forward reaction aA + bBrarr cC+dD is given as: rate =((dx)/(dt))=-1/a(d[A])/(dt)=-1/b(d[B])/(dt)=1/c(d[C])/(dt)=1/d(d[D])/(dt) or expression can be written as : rate =K_(1)[A]^(a)[B]^(b)-K_(2)[C]^(c )[D]^(d) . At equilibrium, rate = 0 . The constants K, K_(1), K_(2) are rate constants of respective reaction. In case of reactions governed by two or more steps reaction mechanism, the rate is given by the slowest step of mechanism. For a gaseous reaction, the rate is expressed in terms of (dP)/(dt) in place of (dC)/(dt) or (dn)/(dt) where C is concentration, n is number of moles and 'P' is pressure of reactant. The three are related as:
The rate and mechamical reaction are studied in chemical kinetics. The elementary reactions are single step reaction having no mechanism. The order of reaction and molecularity are same for elementary reactions. The rate of forward reaction aA + bBrarr cC+dD is given as: rate =((dx)/(dt))=-1/a(d[A])/(dt)=-1/b(d[B])/(dt)=1/c(d[C])/(dt)=1/d(d[D])/(dt) or expression can be written as : rate =K_(1)[A]^(a)[B]^(b)-K_(2)[C]^(c )[D]^(d) . At equilibrium, rate = 0 . The constants K, K_(1), K_(2) are rate constants of respective reaction. In case of reactions governed by two or more steps reaction mechanism, the rate is given by the slowest step of mechanism. For the reaction, 2NO+Br_(2) hArr 2NOBr , the mechanism is given in two steps: (1) NO+Br_(2) overset("fast")(hArr)NOBr_(2) (2) NOBr_(2)+NO overset("slow")(rarr)2NOBr The rate expression for the reaction is: