For gaseous reactions, the rate is expressed in terms of `dP//dt` instead of `dc//dt` or `dn//dt` (where `c` is the concentration and `n` the number of `mol`). What is the relation among these expresisons ?

For the ideal gaseous reaction, the rate is generally expressed in terms of (dP)/(dt) instead of (dC)/(dt) or (dn)/(dt) (where C= (n)/(V) is concentration and n the no. of moles). What is the relation among these three expressions if T and V are constant?

For the ideal gaseous reaction, the rate is generally expressed in terms of (dP)/(dt) instead of (dC)/(dt) or (dn)/(dt) (where C= (n)/(V) is concentration and n the no. of moles). What is the relation among these three expressions if T and V are constant?

For the ideal gaseous reaction, the rate is generally expressed in terms of (dP)/(dt) instead of (dC)/(dt) or (dn)/(dt) (where C= (n)/(V) is concentration and n the no. of moles). What is the relation among these three expressions if T and V are constant?

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 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:

For a hypothetical reaction AtoL the rate expression is rate =-(dC_(A))/(dt)

The rate of a gaseous reaction is generally expressed in terms of (dP)/(dt) . If it were expressed in terms of change in number of moles per unit time ((dn)/(dt)) or in terms of change in molar concentration per unit time ((dC)/(dt)) , which of the following relationship will hold good ?