1.

Which expression is wrong for first order reaction

Answer»

`K = (2.303)/(t) "log" ((A_(0))/(At))`
`k = (t)/(2.303) "log" ((A_(0))/(At))`
`-k = (t)/(2.303) "log" ((At)/(A_(0)))`
Rate = k[A]

Solution :The rate for FIRST ORDER reaction is expressed as :
`A to ` Products
Rate = `- (d[A])/(DT)`
Rate = k [A]
and the rate constant (k) is given as :
`k = (2.303)/(t)` log `([A_(0)])/([A_(t)])` or `-k = (2.303)/(t)` log `([A_(t)])/([A_(0)])`


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