1
Question
For a process A+B→ products, the rate is first order with respect to A and first order with respect to B. When 1.0 mole each of A and B are taken in a one litre vessel, the initial rate is 1×10−2 molL−1s−1 . The rate of the reaction when 90% of the reactants have been converted into products would be:
For a process A+B→ products, the rate is first order with respect to A and first order with respect to B. When 1.0 mole each of A and B are taken in a one litre vessel, the initial rate is 1×10−2 molL−1s−1 . The rate of the reaction when 90% of the reactants have been converted into products would be:
Open in App
Solution
The correct option is B 1×10−4 molL−1s−1
The rate law expression is r=k[A][B].
The initial rate is 1×10−2molL−1s−1.
Hence, 1×10−2molL−1s−1=k[1][1].
k=1×10−2molL−1s−1.
90% reactants are converted into products.
[A]=0.1molL−1s−1and[B]=0.1molL−1.
=k[A][B]=1×10−2(0.1)(0.1)=1×10−4molL−1s−1.
The rate law expression is r=k[A][B].
The initial rate is 1×10−2molL−1s−1.
Hence, 1×10−2molL−1s−1=k[1][1].
k=1×10−2molL−1s−1.
90% reactants are converted into products.
[A]=0.1molL−1s−1and[B]=0.1molL−1.
=k[A][B]=1×10−2(0.1)(0.1)=1×10−4molL−1s−1.
Suggest Corrections
0
Similar questions
View More
Join BYJU'S Learning Program
Explore more
Join BYJU'S Learning Program
