WorksheetsUnit 12 Review_2
Total questions: 34
Worksheet time: 41mins
According to the given diagram which of the following is incorrect?
Energy of reactants is 50 kJ
Energy of products is 100 kJ
The activation energy is 250 kJ
Delta H is +50 kJ
Reaction pathway-PE graph of a reaction is given. Which of the following is correct for the REVERSE reaction?
It is endothermic
Delta H is -50 kJ/mol
Energy of the activated complex is 200 kJ.
Products are more energetic than the reactants.
Which of the following is correct for this reaction?
This might be a combustion reaction.
This might be a neutralization reaction.
This might be an exothermic reaction.
This might be a double displacement (replacement) reaction.
What is the definition of rate of reaction
The rate of reaction is defined as the amount of reactant used up or the amount of a product obtained per unit time
The rate of reaction is defined as the amount of product used up or the amount of a reactant product per unit time
the rate of reaction is defined as the amount of a reactant used up or a product obtained
the rate of reaction is defined as the time taken over the amount of reactant used up
Which of the following statements is correct?
The rate is constant throughout the reaction.
Rate is fastest at the beginning of a reaction.
Rate is fastest at the end of a reaction.
The change in rate depends on the type of the reaction.
During a chemical reaction, the concentration of reactant "A" decreases from 1.2 M to 1.0 M in 10 seconds. The rate of this reaction is:
0.020 M/s
0.20 M/s
2.0 M/s
20. M/s
During a chemical reaction, the concentration of reactant "B" increased from 1.6 M to 3.2 M in 5 seconds. The rate of this reaction is:
0.32 M/s
0.80 M/s
8.0 M/s
0.64 M/s
Which of the following is not used to measure the rate of a chemical reaction?
Color change
Change in pressure
Change in electrical conductivity
Change in atomic numbers
According to the collision theory which of the following could be concluded?
I. Not all collisions result in chemical reaction.
II. All collisions with enough energy will result in a chemical reaction.
III. All collisions with correct orientation will result in a chemical reaction.
I only
I and II
I and III
I, II and III
Which of the following statements is correct?
As the concentration increases, number of effective collisions will increase so the reaction will take place faster.
As the concentration decreases, number of effective collisions will decrease so the reaction will take place faster.
As the concentration increases, number of effective collisions will increase so the reaction will take place slower.
As the concentration decreases, number of effective collisions will decrease so the reaction will take place slower.
Which of the following statements is correct?
As the temperature increases the average kinetic energies of the species increase so the reaction takes place faster.
As the temperature decreases the average kinetic energies of the species increase so the reaction takes place faster.
As the temperature increases the average kinetic energies of the species increase so the reaction takes place slower.
Temperature does not have any effect on the reaction rate.
Which of the following statements is correct?
As the surface area increases, there is more surface for reactions to occur and this increases the rate of reactions.
10 g of a big chunk of CaCO3 rock will react faster than 10 g CaCO3 dust.
The concentration of solid particles are constant so the size of the particles are not important for the rate of the reactions.
The size of the particles does not effect the reaction rate as long as the mass of the particles is the same.
Which of the following is INCORRECT for catalysts?
Catalysts speed up chemical reactions without being used up.
Catalysts decrease the activation energy of chemical reactions.
When you use a catalyst, you will need to use less energy for reaction to take place.
Catalysts energize the reactants so the catalyzed reactions take place faster.
In a chemical reaction, when you double the concentration of one of the reactants
the rate doubles.
the rate does not change because it depends on the concentration of the products.
the rate may or may not change.
the rate halves.
2X + 3Y --> 2Z
In the given reaction
* when the concentration of X is doubled the rate increases 2 times
* When the concentration of Y is doubled the rate increases 4 times.
The order of the reaction with respect to X is 2.
The order of the reaction with respect to Y is 3.
The overall reaction order is 5.
The order with respect to Y is 2.
3X + Y --> Q + Z
The order of the reaction with respect to X is 2.
The overall order of this reaction is 4.
First 2 statements are correct.
The order of the reaction cannot be determined only from the equation.
When the concentration of a reactant is tripled the rate of the reaction increases 9 times. The order of this reaction with respect to that reactant is
1
2
3
insufficient data
A possible rate law for a second overall order of a reaction cannot be __________________
Rate = k [A][B]
Rate = k [B]2
Rate = k [A]2
Rate = k [A]2[B]
The rate law for the reaction 2X(g) + Y(g) → 2Z(g) is first order in X and third order overall. What is the rate law for the reaction?
Rate = k [X]2[Y]
Rate = k 2[X][Y]
Rate = k [X][Y]2
Rate = k [X]3[Y]
According to the given data, what is the overall order of this reaction?
0
1
2
Insufficient data
both 1st order
both second order
F2 - 1st order
CIO2 - 2nd order
F2 - 2nd order
CIO2 - 1st order
The following data were measured for the reaction BF3(g) + NH3(g) —> F3BNH3(g)
This reaction is
second order with respect to NH3
second order with respect to BF3
first order with respect to NH3
3rd order overall
k in the rate law is the specific heat constant. The "k" value increases _____ .
if more concentrated solutions are used as reactant
if a catalyst is used
if smaller reactants are used
if temperature is increased
What is the "k" value for this reaction?
3.41
0.293
0.0133
Insufficient data
Which of the following is/are example(s) for irreversible reactions?
Burning of coal
Baking a cake
I and II
None of them
At equilibrium
I. The concentrations of the reactants and the products are the same
II. Mole number of the reactants and products are the same
III. The rate of the forward reaction and the reverse reactions are equal
IV. Concentrations of the reactants or the products do not change
III and IV
I, II and III
II, III and IV
I, II, III and IV
Which of the following is correct for a system reaching upon a chemical equilibrium?
The rate of the reverse reaction decreases by time.
The rate of the forward reaction increases by time.
The concentration of the products increase until equilibrium is reached.
At equilibrium the rates of forward and reverse reactions are constant but they might be different from one another.
2SO2(g) + O2(g) ⇌ 2SO3(g)
Adding O2(g) will
(Pick 2)
shift equilibrium right
shift equilibrium left
Increase the concentration of SO2.
Increase the concentration of SO3.
2SO2(g)+O2(g) ⇌ 2SO3(g)
Decreasing the volume of container will
(pick 2)
decrease the pressure
increase the pressure
decrease SO3 concentration
2SO2(g)+O2(g)⇌2SO3(g)
Using a catalyst will
(Pick 2)
make the reaction reach equilibrium faster
decrease the activation energy
increase the SO3 concentration
2SO2(g)+O2(g) ⇌ 2SO3(g) + Heat
Decreasing the temperature will
(Pick 2)
shift equilibrium right
shift equilibrium left
increase the O2 concentration
decrease the O2 concentration
decrease SO3 concentration
2SO2(g)+O2(g) ⇌ 2SO3(g) + Heat
Which two of the following will shift the reaction to the reactants?
(Pick 2)
Removing SO2
Increasing the temperature
Decreasing the volume
Adding O2
Removing SO3
2SO2(g)+O2(g) ⇌ 2SO3(g) + Heat
Which two of the following will shift the reaction to the products?
(Pick 2)
Adding O2
Increasing the temperature
Increasing the pressure
Removing SO2
Using a catalyst
2SO2(g)+O2(g) ⇌ 2SO3(g) + Heat
Which two of the following will decrease the equilibrium concentration of SO2?
(Pick 2)
decreasing the temperature
increasing the temperature
removing O2
adding O2
decreasing the pressure
