A reaction was found to be zero-order in A and third-order in B. Increasing the concentration of A by a factor of 3 and the concentration of B by a factor of 2 will cause the reaction rate to _____ increase by a factor of 2 remain constant increase by a factor of 6 increase by a factor of 8
Added by Joan R.
Close
Step 1
The reaction is zero-order in A, which means the rate of the reaction is independent of the concentration of A. So, increasing the concentration of A by a factor of 3 will not affect the reaction rate. Show more…
Show all steps
Your feedback will help us improve your experience
Adi S and 71 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
When the concentration of reactant in the reaction: $\mathrm{A} \rightarrow \mathrm{B}$ is increased by 8 times, the rate increases only by 2 times. The order of reaction is (a) 3 (b) $\frac{1}{3}$ (c) 2 (d) $\frac{1}{2}$
Chemical Kinetics
Exercises I
3. The rate law for the reaction A + B → C + D Is first order with respect to [A] and second order with respect to [B]. If [A] is halved and [B] is doubled, the rate of the reaction will A. remain the same B. increase by a factor of 2 C. increase by a factor of 4 D. increase by a factor of 8
Adi S.
The reaction A + 2B --> products has been found to have the rate law, rate = k[A] [B]^2 . While holding the concentration of A constant, the concentration of B is increased from x to 3x. Predict by what factor the rate of reaction increases.
David C.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
Watch the video solution with this free unlock.
EMAIL
PASSWORD