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For gaseous reactions, the rate is expre...

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 ?

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`(dc)/(d t) = (1)/(V)[(dn)/(d t)]` …(i)
(as `c = (n)/(V)`, where `n =` number of moles, `V =` volume of solution)
Uisng gas law equation,
`PV = n RT`
`V = (nRT)/(P)`
or `(n)/(V) = (P)/(RT)` or `(dn)/(V) = (dP)/(RT)` ...(ii)
Substituting Eq. (ii) in Eq. (i), we get
`(dc)/(d t) = (1)/(RT)[(dp)/(dt)]`
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