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WorksheetsGrade 11: Rate and progress of reactions-W9
Total questions: 20
Worksheet time: 10mins
What is rate?
The measure of how much something changes within a specific time
The velocity of light in vacuum.
Speed of light.
The measure of the volume of products.
In Chemistry, the rate of reaction is:
time over concentration.
change of the amount of reactant or product per time.
concentration over volume.
change of the amount of reactant only.
In (a), the energy is:
Exothermic.
Athermic.
Endothermic.
In (b), the enthalpy change Δ H is
Negative.
Postivie.
An endothermic reaction absorbs heat, and an exothermic reaction releases heat.
True.
False.
In (A), no reaction occurs, we say, it is:
Ineffective collision.
Effective collision.
Unstable arrangement of atoms that forms for a moment at the peak of the activation energy barrier is:
Inactivated complex.
Collision theory.
Activated complex.
Barrier.
For a chemical reaction to occur and have an effective collision:
Particles must collide.
Particles must collide at proper orientation.
Particles must have enough kinetic energy to cross the activation energy barrier.
All of the above.
Which factor best describes this image?
Effect of particle size on reaction rate.
Effect on concentration on reaction rate.
Effect of temperature on reaction rate.
Effect of catalyst on reaction rate.
What does MnO2 represent in the tube (b)?
An inhibitor.
A product.
A catalyst.
An enzyme.
The best definition for inhibitor is:
A substance that increases the action of a catalyst.
A substance that decreases the action of a catalyst.
A substance that interferes with the action of a catalyst.
Find the overall rate for the following rate law:
Rate = k[A]2[B]2[C]3[D]0
Zeroth- order overall.
7th order overall.
5th order overall.
Third-order overall.
A proportionality constant relating the concentration of reactants to the rate of the reaction is:
Specific rate constant.
Rate law.
Specific constant volume.
Rate increment.
The rate of disappearance of A is:
dtd[A]
0.1515
50.15
- dtd[A]
V, X, and Z represent:
Intermediates.
Valleys.
Activated complexes.
In the following multistep reaction, there are:
Two intermediates formed as the reaction progresses.
Energy of reactants is less than energy of products.
Three intermediates formed as the reaction progresses.
The rate-determining step is:
Second-step.
First-step.
The oxygen atom is considered as:
A catalyst in this multi-step reaction.
An intermediate in this multi-step reaction.
Reactant only in this multi-step reaction.
In the following two-step reaction mechanism:
NO2 + F2 --> NO2F + F (slow)
NO2 + F --> NO2F (fast)
Which is the rate-determining step? and the intermediate?
Fast-step, and intermediate is NO2.
Slow-step, and intermediate is NO2F.
Slow-step, and intermediate is F.
The order of reaction w.r.t A, and overall order of reaction are:
Second-order w.r.t A, and overall order is 2.
Second-order w.r.t A, and overall order is 3.
First-order w.r.t A, and overall order is 2.
