State the order of reaction with respect to a reactant, R, if:
a) the rate of reaction doubles when [R] doubles
b) the rate of reaction is unchanged when [R] triples
c) the rate of reaction reduces by a factor of four when [R] is halved
Solution
vR=−d[R]/dt=k[R]n - rate equation [1]
a) v1=v2/2 and [R1]=[R2]/2
Hense
k[R1]n=k[R2]n/2
([R1]/[R2])n=1/2
n=log[R2][R1]0,5=log210,5=1
b) v1=v2 and [R1]=[R2]/3
Hence
k[R1]n=k[R2]n
([R1]/[R2])n=1
n=log[R2][R1]1=0
c)v1=4v2 and [R1]=2[R2]
Hence
k[R1]n=4k[R2]n
([R1]/[R2])n=4
n=log[R2][R1]4=log24=2
Answer: a) n=1, b) n=0, c) n=2
Reference: https://en.wikipedia.org/wiki/Rate_equation
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