The 2nd order reaction becomes 1st order when:
Correct answer: B. One of the reactants is in large excess
- A. One of the reactants is limiting
- B. One of the reactants is in large excess
- C. None of the reactants is in large excess
- D. Both reactants in large excess
Explanation
The substance taken in small amount controls the rate and the order is noted with respect to that substance. If the cone. Of any reactant is taken in excess it will not involve in rate determination step.
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
The unit of rate constant of second order reaction is:
The specific rate constant of a chemical reaction is the rate of the reaction when the concentration of the reactant is:
Which method for rate determination is useful for those reaction, which involve small volume change in solutions?
For a reaction A+2B ----> C, rate is given by Rate = k[A][B], hence the order of the reaction is:
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:
The half-life period of zero order reaction is equal to: