The rate law for the reaction below is given by the expression \(k\,[A][B]\)
\(A + B \rightarrow \text{Product}\)
If the concentration of B is increased from 0.1 to 0.3 mole, keeping the value of A at 0.1 mole, the rate constant will be :
\(A + B \rightarrow \text{Product}\)
If the concentration of B is increased from 0.1 to 0.3 mole, keeping the value of A at 0.1 mole, the rate constant will be :
Show Hint
- \(k\)
- \(k/3\)
- \(3k\)
- \(9k\)
The Correct Option is A
Solution and Explanation
So the rate constant remains \(k\).
Answer: (1) \(k\)
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