For the reaction A+B----->C+D, doubling the concentration of both the reactants increases the reaction rate by 8 times and doubling the initial concentration of only B simply doubles the reaction rate. The rate law for the reaction is:
Correct answer: D. Rate = k[A]2[B]
- A. Rate = k[A][B]2
- B. Rate = k[A][B]
- C. R = k[A]1/2 [B]2
- D. Rate = k[A]2[B]
Explanation
It is overall 3rd order reaction. With respect to A, it is 2nd order reaction with respect to B is 1st order
Report an error
The more specific you are, the faster it gets fixed. A source beats an opinion.
Prefer email? [email protected]
About Reaction Kinetics
Reaction kinetics relates reaction rate to concentration, temperature, surface area and catalysts. Questions cover rate laws, reaction order, rate constants, activation energy and the activated complex, including how a catalyst lowers the activation energy without changing the overall energy change or equilibrium position.
Practise Reaction Kinetics
573 free Reaction Kinetics MCQs from Chemistry, each with the correct answer and an explanation. Unlimited attempts, no account needed.
Discussion
Stuck on an option, or know a faster way to get there? Ask or explain it here.
No comments yet. Be the first to explain this one.
Exams that ask Chemistry questions like this
Chemistry is on 14 papers prepared for on TestUstad, and all of them draw the same bank, so this question is worth knowing for every one of them.
More Reaction Kinetics questions
For a reaction A+2B ----> C, rate is given by Rate = k[A][B], hence the order of the reaction is:
The 2nd order reaction becomes 1st order when:
The unit of rate constant of second order reaction is:
The half-life period of zero order reaction is equal to:
For which of the reaction, half-life is inversely proportional to the initial concentration of the reactants?
If 'a' is the initial concentration of the reactant then half-life period of the reaction of nth order is directly proportional to: