Chemical Equilibrium or Dynamic Equilibrium Quiz

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Kamran Fateh

Chemical Equilibrium or Dynamic Equilibrium

Chemical Equilibrium Batch 09

Chemical equilibrium occurs in a reversible chemical reaction when the forward and reverse reactions proceed at the same rate, resulting in constant concentrations of reactants and products over time. At this point, the system is balanced, though reactions continue dynamically. Chemical equilibrium is essential for predicting reaction behavior in various chemical and biological processes.

1 / 35

In the reaction if both $H_{2}$ and are doubled, then:

K changes

K remains the same

Reaction stops

Equilibrium shifts to the left

2 / 35

If is large and positive, it indicates that at equilibrium:

Products dominate

Reactants dominate

No change occurs

None of the above

3 / 35

Which of the following factors affect the value of for a reaction?

Catalyst

Temperature

Volume

Pressure

4 / 35

The value of for the reverse reaction is:

1 / 𝐾

None

5 / 35

The effect of increasing volume on a gaseous equilibrium depends on:

The number of moles of gases

Catalyst present

Type of gas

None

6 / 35

If number of moles of reactant and product are equal

Kp is less than Kc

Kp is greater than Kc

Kp is equal to Kc

None

7 / 35

The reaction quotient (Q) is used to determine:

Rate of reaction

Initial concentrations

Direction of shift to reach equilibrium

Value of 𝐾c

8 / 35

If Q > K, the reaction will shift:

Right

Left

Both direction

None

9 / 35

Which of the following best describes dynamic equilibrium?

No reaction occurs

The forward and reverse reactions occur at the same rate

Concentrations change constantly

The reaction stops once equilibrium is reached

10 / 35

If $K_{c} = 0.1$ , it indicates that:

Reactants are favored

Products are favored

Equilibrium does not occur

Equilibrium is in the middle

11 / 35

What is the effect of adding a catalyst on the equilibrium constant?

Increases it

Decreases it

No effect

Shift Kc

12 / 35

A large value of $K_{c}$ indicates that:

Products are favored at equilibrium

Reactants are favored at equilibrium

No reaction occurs

Reaction stops

13 / 35

In an exothermic reaction, increasing the temperature will:

Shift equilibrium to the right

Shift equilibrium to the left

Not affect equilibrium

Increase the concentration of products

14 / 35

What is the equilibrium constant (K) for a reaction where products are favored at equilibrium?

K is equal to 1

K is less than 1

K is greater than 1

None

15 / 35

If a reaction at equilibrium is disturbed, it will shift to counteract the disturbance. This is called:

Reaction Law

Le Chatelier’s Principle

Conservation Law

Reaction Quotient

16 / 35

For a reaction in which $Δ H < 0$ (exothermic), a decrease in temperature will:

Shift equilibrium to the left and decrease 𝐾

Shift equilibrium to the right and increase 𝐾

Shift equilibrium to the right and decrease 𝐾

Shift equilibrium to the left and increase 𝐾

17 / 35

For the reaction $N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)$ , if the system is at equilibrium and the volume of the container is decreased, what will happen?

The equilibrium will shift to the left, favoring 𝑁2O4

The equilibrium will shift to the right, favoring 𝑁O2

There will be no change in the position of equilibrium

The equilibrium constant 𝐾 will increase.

18 / 35

If a reaction has a large $K_{c}$ value, which of the following is true?

The reaction strongly favors the reactants.

The reaction strongly favors the products.

The reaction does not reach equilibrium.

The reaction rate is very high

19 / 35

In the equilibrium $C a C O_{3} (s) ⇌ C a O (s) + C O_{2} (g)$ , if the pressure is decreased, what happens to the equilibrium?

Shifts to the left

Shifts to the right

No change, as there are only solids present

𝐾 increases

20 / 35

For a reaction with $Δ G = 0$ at equilibrium, which of the following is true?

The system is not at equilibrium.

There is no net change in the concentrations of reactants and products.

The reaction only proceeds in the forward direction.

The equilibrium constant is equal to zero.

21 / 35

If the solubility of $A g_{2} C O_{3}$ in water is $s$ , what is the expression for its solubility product ?

Ksp = s2

Ksp = s3

Ksp = 4s3

None

22 / 35

If the Ksp of $M g (O H)_{2}$ is , what is the molar solubility of $M g (O H)_{2}$ in water?

1.0×10−5 M

1.3×10 -4 M

1.8×10 −6 M

2.5×10 −4 M

23 / 35

What does the solubility product constant (Ksp) represent?

The concentration of reactants in a solution

The equilibrium constant for a salt dissolving in water

The rate of reaction in a solution

The concentration of a gas

24 / 35

What happens to the solubility of a salt if a common ion is added to the solution?

Solubility increases

Solubility decreases

Solubility remains the same

Salt fully dissolves

25 / 35

Which of the following changes can disturb a dynamic equilibrium in a closed system?

Adding a catalyst

Changing the temperature

Decreasing the volume of a solid reactant

Removing a solvent

26 / 35

The average rate of a reaction over a time interval is defined as

The rate at a specific moment in time

The change in concentration of a reactant or product divided by the time interval

The total concentration of reactants consumed

The rate at which equilibrium is reached

27 / 35

The Law of Mass Action states that the rate of a reaction is directly proportional to:

The total volume of the reaction

The product of the molar concentrations of reactants, each raised to the power of their stoichiometric coefficients

The temperature of the system

The difference in concentration between products and reactants

28 / 35

For a reaction at equilibrium, the Law of Mass Action helps to determine:

The rate of the forward reaction only

The concentration of a catalyst needed

The equilibrium constant

The enthalpy change of the reaction

29 / 35

Which of the following is a synonym of "faun"?

Sprite

Satyr

Nymph

Troll

30 / 35

Why are filler activities important in a lesson plan?

They extend the lesson time

They are unrelated to the lesson content

They are related to the lesson content and help maintain focus

They are used to replace primary activities

31 / 35

What is the relationship between instruction and classroom management?

Instruction and management are unrelated.

Effective instruction can occur without proper classroom management

Classroom management should complement and support instruction.

Classroom management is secondary to instruction.

32 / 35

Why should positive behaviors be included in the curriculum?

To focus only on academic aspects

To ensure a balanced approach integrating cognitive and affective aspects

To avoid teaching social and emotional skills

To exclude behavioral development from the curriculum

33 / 35

What should teachers do before incorporating new teaching techniques into their lessons?

Begin using them immediately

Consult with students about their preferences

Undergo adequate training and familiarization

Avoid using them to prevent complications

34 / 35

How can mnemonic devices help students?

By increasing classroom noise

By converting information into a more memorable form

By replacing traditional teaching methods

By reducing the need for visual aids

35 / 35

What is the purpose of brainstorming in the classroom?

To create a lesson plan from scratch

To gather and organize students’ ideas for writing

To test students’ prior knowledge

To evaluate students’ understanding of content

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