2A + B → Product If the reactant 'B' is in excess, the order of reaction with respect to 'A' in given rate law is: Rate = k[A]2[B] is:
Correct answer: A. 2nd order reaction
- A. 2nd order reaction
- B. 1st order reaction
- C. Pseudo 1st order reaction
- D. 3rd order reaction
Explanation
Rate equation is mentioned and in case rate equation, especially order of reaction, is mentioned, then those are the only things to be considered. In this case, oder of reaction is 2+0=2 (SECOND 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
By considering Arrhenius equation, the graph between '1/T' and 'log K', which of the following graph represents the relationship between log K and 1/T?
If the reactant or product of a chemical reaction can absorb ultraviolet, visible or infrared radiation, then the rate of a chemical reaction can best be measured by which one of the following methods?
According to collision theory of bimolecular reaction in gas phase, the minimum amount of energy required for an effective collision is known as:
The rate constant 'k' is 0.693 min-1. The half-life for the first-order reaction will be:
Reactants in a transition state:
Actual yield is a/an: