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For the gaseous phase reaction : A(g) ra...

For the gaseous phase reaction : A(g) `rarr` products, occurring at constant volume the correct relation between `(dC_(A))/(dt),(dn_(A))/(dt)` and `(dP_(A))/(dt)` is : `[C_(A)rarr"Concentration of reactant A", n_(A)rarr"Moles of reactant A", P_(A) rarr "Partial pressure of reactant" A]`

A

`(dC_(A))/(dt)=(dn_(A))/(dt)=(dP_(A))/(dt)`

B

`(dC_(A))/(dt)=((dP_(A))/(dt))RT=(1)/(V)(dn_(A))/(dt)`

C

`(dC_(A))/(dt)=(1)/(RT)(dP_(A))/(dt)=(1)/(V)(dn_(A))/(dt)`

D

`(dC_(A))/(dt)=(1)/(V)(dn_(A))/(dt)=(1)/(V)(dP_(A))/(dt)`

Text Solution

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The correct Answer is:
C
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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 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:

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