Most Important Chemical Equilibrium Quiz Test Online

Chemical Equilibrium Quiz Test Online

Chemical Equilibrium Test. 1

1 / 20

1) If Kc value is very large, the equilibrium position will shift:

It remains unchanged.

It is always a constant value.

Toward reactants (left).

Toward products (right).

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2) If Kc value is very small, the equilibrium position will shift:

Toward products (right).

It is always a constant value.

Toward reactants (left).

It remains unchanged.

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3) Which statement correctly describes a reversible reaction?

Forward and reverse reactions take place at different times and under different conditions.

Forward and reverse reactions occur simultaneously under the same conditions.

Only the forward reaction occurs; the reverse reaction does not take place.

Both forward and reverse reactions occur, but under different conditions.

4 / 20

For the reaction:

The units of the equilibrium constant (Kc) are:

Concentration⁻¹ (Conc.⁻¹)

Concentration (Conc.)

Concentration² (Conc.²)

No units

5 / 20

For the reaction

If the equilibrium concentrations of H₂, I₂, and HI are 8, 3, and 24mol/dm³, respectively, what is the equilibrium constant

6 / 20

For the reaction:

At equilibrium, the concentrations of CO, H₂, and CH₃OH become constant. What will happen?

Equilibrium state is disturbed.

Reaction slows down.

Equilibrium state remains undisturbed.

Reaction speeds up.

7 / 20

For the following reaction in the gaseous phase:

CO +1/2O2 ⇌ CO2, Kc/Kp is

(RT)^−(1/2)

(RT) ^1

(RT) ^−1

(RT)^ (1/2)

8 / 20

If temperature is increased, how will the reaction shift?

Remains unchanged

Decreases the rate of reaction

Backward direction

Forward direction

9 / 20

For the reaction:

The forward reaction is favored by:

Decreasing the concentration of H₂

Decreasing temperature

Adding NH₃ at equilibrium

Adding a catalyst

10 / 20

10)

For the given reaction:

Kp >Kc

Kp=Kc

Kp<Kc

Kp=Kc=0

11 / 20

11) One mole of HI was sealed in a tube and heated at 440°C until equilibrium was reached. If HI was found to be 50% dissociated, the equilibrium constant Kc for the reaction is:

0.5

0.25

0.625

12 / 20

12) In a given system, water and ice are in equilibrium. If pressure is applied, what will happen?

More ice is melted

The amount of ice and water remains the same

Both A and B

More ice is formed

13 / 20

13)

In the reaction:

If ΔH is negative, the formation of AB(g) will be favored at:

Low temperature and high pressure

High temperature and low pressure

High temperature and high pressure

Low temperature and low pressure

14 / 20

14) At equilibrium, the concentration of reactants and products is:

Constant

Unstable

Maximum

Minimum

15 / 20

15)

For the reaction:

The equilibrium constant (K) is affected by:

Catalyst

Temperature

Total pressure

Concentration

16 / 20

16) Which of the following correctly represents the relationship between Kp and Kc?

Kc = Kp (RT)Δⁿ

Kp = Kc (R/N)Δⁿ

Kp = Kc (R)Δⁿ

Kp = Kc (RT)Δⁿ

17 / 20

17)

At equilibrium, the concentrations of SO₂, O₂, and SO₃ are 2M, 2M, and 4M, respectively, for the reaction:

What is the Kc value?

0.2

18 / 20

18) One mole of ethyl alcohol was treated with one mole of acetic acid at 25°C. If 2/3 of the acid changes into ester at equilibrium, the equilibrium constant of the reaction will be:

19 / 20

19) For what value of Kc is the forward reaction almost complete?

10³⁰

10⁻³⁰

20 / 20

20) In the Haber process, equilibrium gas mixture contains ___ NH₃ by volume.

55%

20%

35%

70%

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The average score is 52%

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Chemical Equilibrium Test. 2

1 / 20

If the temperature is decreased, what will happen to the formation of NH₃, given that the reaction is reversible and exothermic?

NH₃ will start decomposing

The reaction will remain unaffected

The formation of NH₃ will decrease

The formation of NH₃ will increase

2 / 20

The ionization of BaSO₄ is suppressed by:

Adding BaCl₂

Decreasing temperature

Increasing temperature

Adding NaCl

3 / 20

3) The catalyst used in the Haber process is:

Fe (Iron)

MgO

SiO₂

Al₂O₃

4 / 20

4) Which of the following is a basic buffer solution?

(COOH)₂ / (COONa)₂

NH₄OH / NH₄Cl

HF / NaF

H₂CO₃ / Na₂CO₃

5 / 20

5) For a sparingly soluble salt , the solubility is "S" mol/dm³. The solubility product (Ksp) is given by:

Ksp = 27S⁴

Ksp = S²

Ksp = 4S³

Ksp = 27S³

6 / 20

6) If ionic product > Ksp, then the solution is:

Ideal

Supersaturated

Saturated

Unsaturated

7 / 20

7) When CO₂ gas is passed through a saturated solution of calcium carbonate (CaCO₃), the solubility of CaCO₃:

Decreases

First increases, then decreases

Remains unchanged

Increases

8 / 20

8) For an acidic buffer, if:

[Salt] > [Base]

[Salt] < [Acid]

[Salt] = [Acid]

[Salt] > [Acid]

9 / 20

9) If the ionic product = Ksp, the solution is

Unsaturated

Supersaturated

Saturated

Dilute

10 / 20

10)

If Na₂SO₄ is added to a solution of BaSO₄, BaSO₄ will precipitate due to:

Decrease in temperature

Salt hydrolysis

Common ion effect

Increase in solubility

11 / 20

11) A basic buffer solution can be prepared by mixing:

A strong base and its salt with a weak acid

A strong acid and its salt with a weak base

A weak base and its salt with a strong acid

A weak acid and its salt with a strong base

12 / 20

12) The solubility product (Ksp) is applicable only for substances whose molar concentrations are:

Equal to 0.1M

Equal to or less than 0.01

Greater than 0.1

Equal to1M

13 / 20

13)

A chemical substance that releases H⁺ ions when dissolved in water is known as:

Base

Amphoteric

Acid

Neutral

14 / 20

14) A buffer solution is a solution that resists the change in:

None of these

pOH

pKb

15 / 20

15) Which Henderson equation is correct?

pH=pKa+log([salt]/[acid])

pOH = pKb + log ([Salt] / [Base])

pH = pKb + log ([Base] / [Acid])

pH = pKa + log ([Acid] / [Salt])

16 / 20

16) A buffer solution contains equal concentrations of acid (X) and its conjugate base, where the Ka for X is 10⁻³. The pH of the buffer is:

17 / 20

17) The pH of an ideal buffer solution is:

Less than 7

18 / 20

18) Units of equilibrium constant (Kc) for the following reaction:

A+B⇌2C

mol² dm⁻⁶

No unit

mol/dm³

mol⁻¹ dm³

19 / 20

19) In a saturated solution of AB, the molar concentration of A⁺ and B⁻ ions is 1 × 10⁻⁵ M. Find Ksp?

1.5 × 10⁻⁵

1.0 × 10⁻¹⁰

1.0 × 10⁻⁵

2.0 × 10⁻²

20 / 20

20) Buffer action can be explained by:

Common ion effect

Mass action law

All of these

Le Chatelier’s principle

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The average score is 64%

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Chemical Equilibrium Test. 3

1 / 20

1) Which one of the following bases has the highest Kb value?

CH₃NH₂

NH₃

C₂H₅NH₂

NaOH

2 / 20

2) Which of the following is the correct representation for Ksp of BaSO₄?

BaSO₄ ⇌Ba²⁺ + SO₄²⁻

Ksp = [Ba²⁺][SO₄²⁻] / [BaSO₄]

Ksp = [BaSO₄] / ([Ba²⁺][SO₄²⁻])

Ksp = [Ba²⁺][SO₄²⁻]

Ksp = [Ba²⁺] + [SO₄²⁻]

3 / 20

If the pKa of formic acid (HCOOH) is 3.75, the pH of an equimolar solution of formic acid and sodium formate is:

4.75

3.75

2.75

4 / 20

Which of the following factors affect the equilibrium position?

Only concentration

Temperature, concentration, and pressure

Catalyst only

None of these

5 / 20

5) What is the relationship between pH and pKa?

pH=pKa−log[Acid/Base]

pH=pKa+log[ Acid /Base]

pH=pKa+log[Base/Acid]

pKa=pH−log[Acid/Base]

6 / 20

In the equation Kp = Kc (RT)ⁿ, if Δn > 0, then:

Kp<0

Kp<Kc

Kp=Kc

Kp>Kc

7 / 20

7) At 25°C, the solubility product constant (Ksp) for the PbSO₄ system is:

1.0 × 10⁻¹⁴ mol² dm⁻⁶

6.4 × 10⁻⁷ mol² dm⁻⁶

1.8 × 10⁻¹⁰ mol² dm⁻⁶

1.6 × 10⁻⁸ mol² dm⁻⁶

8 / 20

8) Human blood has pH of:

7.50 - 8.00

6.50 - 7.00

7.20 - 7.25

7.35 - 7.40

9 / 20

The Kc unit for the reaction:

mol⁻² dm⁶

mol⁻³ dm⁹

mol² dm⁻⁶

mol dm⁻³

10 / 20

10) For which of the following equilibrium reactions, K has no units?

2A+B ⇌2C

A+2B ⇌2C

A+B ⇌C+D

A+3A ⇌2C

11 / 20

11)

For maximum yield of NO₂, according to Le Chatelier’s Principle, the reaction:

should be carried out at:

High temperature and low pressure

Low temperature and low pressure

Low temperature and high pressure

High temperature and high pressure

12 / 20

12)

BaF₂ is sparingly soluble, having a solubility product (Ksp) of 1.5 × 10⁻⁶. What will be its solubility?

1.1 × 10⁻³ M

8.1 × 10⁻³ M

5.2 × 10⁻³ M

7.2 × 10⁻³ M

13 / 20

13)

Consider the following reversible reaction:

The initial concentrations are:

Ethanol (CH₃CH₂OH) = 1 mol
Acetic acid (CH₃COOH) = 1 mol
Ethyl acetate (CH₃COOCH₂CH₃) = 0 mol
Water (H₂O) = 0 mol

At equilibrium, the concentrations are:

CH₃CH₂OH = 0.333 mol
CH₃COOH = 0.333 mol
CH₃COOCH₂CH₃ = 0.666 mol
H₂O = 0.666 mol

If 1 mole each of CH₃CH₂OH and CH₃COOH are added, what will be the new equilibrium concentrations?

[CH₃COOH] = 1.333, [CH₃COOCH₂CH₃] = 0.666, [CH₃CH₂OH] = 0.333, [H₂O] = 1.666

[CH₃COOH] = 0.333, [CH₃COOCH₂CH₃] = 1.333, [CH₃CH₂OH] = 0.333, [H₂O] = 1.333

[CH₃COOH] = 0.666, [CH₃COOCH₂CH₃] = 1.333, [CH₃CH₂OH] = 0.666, [H₂O] = 1.333

[CH₃COOH] = 0.333, [CH₃COOCH₂CH₃] = 1.666, [CH₃CH₂OH] = 1.333, [H₂O] = 0.666

14 / 20

14)

The product of ion concentrations in a saturated solution of a sparingly soluble salt at 310 K, each raised to the power of its stoichiometric coefficient, is known as

Equilibrium constant (Kc)

Solubility product (Ksp)

Reaction quotient (Q)

Ionic product

15 / 20

15)

The equilibrium constant (Kc) for the reaction N₂(g) + O₂(g) ⇌ 2NO(g) is 4.0 x 10⁻⁴ at a certain temperature. What is the value of Kc for the reaction 2NO(g) ⇌ N₂(g) + O₂(g) at the same temperature?

4.0 x 10⁻⁴

2.5 x 10³

2.0 x 10⁻²

2.5 x 10⁴

16 / 20

16)

Precipitation takes place when the ionic product of the ions in a solution is:

Equal to unity

Equal to Ksp

Less than Ksp

Greater than Ksp

17 / 20

17) What is the pH of 0.01 M HCl?

18 / 20

18)

Which of the following factors influence a reversible chemical reaction based on Le Chatelier’s Principle?

Temperature, pressure, and concentration

catalyst

Volume and catalyst

None of these

19 / 20

19) The pH of human blood is:

6.7 - 8

7.35 - 7.4

7.5

20 / 20

20)

What will be the pH of an HCl solution with a concentration of 10⁻² M?

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The average score is 70%

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Chemical Equilibrium Test. 4

1 / 8

As the forward reaction is exothermic, an increase in temperature shifts the equilibrium:

To the right, increasing C

To the left, increasing A and B, while decreasing C

To the right, increasing A and B while C remains the same

To the left, decreasing A and B while increasing C

2 / 8

2) In a gaseous reaction where the number of moles of reactants and products are the same, the relationship between Kp and Kc is:

Kc < Kp

None of these

Kp = Kc

Kc > Kp

3 / 8

3) The pKa values of some acids at room temperature are given below. Which one is the strongest acid?

HI (pKa = -10)

HCl (pKa = -7)

H₂SO₄ (pKa = -3)

HNO₃ (pKa = -1.4)

4 / 8

The production of NH₃ will be highest at:

Low temperature and low pressure

Low temperature and high pressure

High temperature and high pressure

High temperature and low pressure

Since the forward reaction is exothermic, a lower temperature favors NH₃ formation. Additionally, since fewer gas molecules are on the right side, increasing pressure shifts equilibrium toward NH₃ production.

5 / 8

5) The purification of table salt (NaCl) by passing HCl gas through its saturated aqueous solution is an example of:

Common ion effect

Hess’s law

Law of mass action

Henry’s law

6 / 8

6) Which statement is correct regarding the reaction:
2NOCl ⇌ 2NO + Cl₂

Kp > Kc

Kp < Kc

Kp = Kc

None of the above

7 / 8

7) Ice and water are in equilibrium within a closed system. If the pressure is decreased, the equilibrium will shift:

Affecting the entire system at equilibrium.

No change in equilibrium.

Reverse, leading to more water freezing.

Forward, causing more ice to melt.

8 / 8

8) Which industrial process is represented by the reaction: N₂ + 3H₂ ⇌ 2NH₃?

Contact process

Solvay process

Haber’s process

Avogadro’s law

Your score is

The average score is 82%

Most Important Chemical Equilibrium Quiz Test Online

Chemical Equilibrium Quiz Test Online

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