1. Tardigrade
  2. Question
  3. Chemistry
  4. Reaction A + B longrightarrow C + D follows following rate law: rate = k [ A ]+(1/2)[ B ](1/2). Starting with initial conc. of 1 M of A and B each, what is the time taken for concentration of A become 0.25 M. Given: k =2.303 × 10-3 sec -1.

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Q. Reaction $A + B \longrightarrow C + D$ follows following rate law : rate $= k [ A ]^{+\frac{1}{2}}[ B ]^{\frac{1}{2}}$. Starting with initial conc. of $1 \,M$ of $A$ and $B$ each, what is the time taken for concentration of A become $0.25\, M$. Given : $k =2.303 \times 10^{-3} sec ^{-1}$.

Chemical Kinetics

Solution:

It is a first order reaction
$ t =\frac{2.303}{2.303 \times 10^{-3}} \log \frac{1}{0.25} $
$ t =1000 \times 0.6=600$ second