Blog Log in Get Started Free

Equilibrium MCQs for NEET — Chemistry Questions with Answers

Q: Are these Equilibrium questions free to attempt?

Yes. You can attempt every Equilibrium question on this page for free without logging in, and check the correct answer with a detailed explanation instantly.

Q: Do I need an account to practise Equilibrium MCQs?

No account is required to attempt questions and view answers. A free account adds bookmarks, personal notes, and progress tracking.

Q: Are these previous year NEET questions?

The bank mixes NEET previous year questions (PYQs) with practice questions, each tagged with its exam appearances where applicable.

Practice free Equilibrium (Chemistry) NEET multiple-choice questions online with instant answers and detailed explanations. No login required.

All Physics Chemistry Botany Zoology

Language English हिंदी

Chapter Difficulty Show only questions I answered incorrectly Clear Register free for difficulty & keyword filters

● ● ● ● ●

The equilibrium constant for the reaction $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$ is $K_c$. If the temperature is increased for this exothermic reaction, what happens to the value of $K_c$?

A. $K_c$ increases. B. $K_c$ decreases. C. $K_c$ remains unchanged. D. $K_c$ depends only on initial concentrations.

You've reached today's free limit of 20 questions. Log in to keep practising for free.

Explanation

The NCERT states, 'The equilibrium constant for an exothermic reaction (negative $\Delta H$) decreases as the temperature increases.' For the formation of ammonia, $\Delta H$ is negative (exothermic).

● ● ● ● ●

For the thermal decomposition of calcium carbonate, $CaCO_3(s) \rightleftharpoons CaO(s) + CO_2(g)$, the equilibrium constant $K_p$ at 1100 K is 2.00. What is the partial pressure of $CO_2(g)$ at equilibrium at this temperature?

A. 2.00 Pa B. $2.00 \times 10^5$ Pa C. 1.00 Pa D. $0.48$ bar

You've reached today's free limit of 20 questions. Log in to keep practising for free.

Explanation

The NCERT states, 'Kp = $pCO_2$ = $2 \times 10^5$ Pa/10^5 Pa = 2.00'. This means that $pCO_2$ divided by $10^5$ Pa equals 2.00, so $pCO_2 = 2.00 \times 10^5$ Pa. The example explicitly demonstrates this calculation for $K_p$ in the context.

● ● ● ● ●

An endothermic reaction has a $\Delta H > 0$. If the temperature of this reaction at equilibrium is increased, what will be the effect on its equilibrium constant ($K_c$)?

A. $K_c$ will decrease. B. $K_c$ will increase. C. $K_c$ will remain constant. D. The effect on $K_c$ cannot be determined without specific values.

You've reached today's free limit of 20 questions. Log in to keep practising for free.

Explanation

The NCERT specifies, 'The equilibrium constant for an endothermic reaction (positive $\Delta H$) increases as the temperature increases.'

● ● ● ● ●

In a heterogeneous equilibrium involving solids, such as $Ni(s) + 4CO(g) \rightleftharpoons Ni(CO)_4(g)$, why are the concentrations of pure solids not included in the equilibrium constant expression?

A. They do not react. B. Their concentrations are very low. C. Their concentrations or partial pressures do not vary and are considered constant. D. They only act as catalysts.

You've reached today's free limit of 20 questions. Log in to keep practising for free.

Explanation

The NCERT states, 'it must be remembered that for the existence of heterogeneous equilibrium pure solids or liquids must also be present (however small the amount may be) at equilibrium, but their concentrations or partial pressures do not appear in the expression of the equilibrium constant' because they are constant. This is also implicitly shown in the $CaCO_3$ decomposition example.

● ● ● ● ●

Which of the following characteristics is NOT true for an equilibrium constant?

A. It is dependent on temperature. B. Its value allows prediction of the direction of a reaction when not at equilibrium. C. It provides information about the speed at which equilibrium is attained. D. It can be used to calculate equilibrium concentrations.

You've reached today's free limit of 20 questions. Log in to keep practising for free.

Explanation

The NCERT explicitly states, 'An equilibrium constant does not give any information about the rate at which the equilibrium is reached.' However, it can predict the extent and direction of a reaction, and calculate equilibrium concentrations, and is temperature dependent.

● ● ● ● ●

For the reaction $H_2(g) + O_2(g) \rightleftharpoons 2H_2O(g)$ at 500 K, the equilibrium constant $K_c = 2.4 \times 10^{47}$. If, at a certain instant, the concentration quotient $Q_c$ is $1.0 \times 10^{40}$, in which direction will the reaction proceed?

A. To the left (reverse direction). B. To the right (forward direction). C. The system is already at equilibrium. D. No reaction will occur.

You've reached today's free limit of 20 questions. Log in to keep practising for free.

Explanation

The NCERT states that the direction of reaction can be predicted by the reaction quotient ($Q_c$) which is equal to $K_c$ at equilibrium. If $Q_c < K_c$, the reaction will proceed in the forward direction to reach equilibrium. Here, $1.0 \times 10^{40} < 2.4 \times 10^{47}$, so the reaction will proceed in the forward direction.

● ● ● ● ●

How does the equilibrium constant for the reverse reaction relate to the equilibrium constant for the forward reaction?

A. It is equal. B. It is the negative of the forward reaction's constant. C. It is the inverse of the forward reaction's constant. D. It is the square of the forward reaction's constant.

You've reached today's free limit of 20 questions. Log in to keep practising for free.

Explanation

The NCERT states, 'The equilibrium constant for the reverse reaction is equal to the inverse of the equilibrium constant for the forward reaction.'

● ● ● ● ●

If a reaction has an equilibrium constant $K_c = 1.0$, what can be inferred about the relative amounts of reactants and products at equilibrium?

A. Only reactants are present. B. Only products are present. C. Reactants and products are present in comparable amounts. D. The reaction does not occur.

You've reached today's free limit of 20 questions. Log in to keep practising for free.

Explanation

A $K_c$ value of 1.0 falls between $10^{-3}$ and $10^3$. As per the NCERT, in this range, 'the concentrations of the reactants and products are comparable, when the system is in equilibrium.'

● ● ● ● ●

When does the expression for the equilibrium constant become applicable?

A. At the start of the reaction. B. When the concentrations of reactants begin to decrease. C. Only when the concentrations of reactants and products have attained constant values at the equilibrium state. D. When the temperature of the system changes.

You've reached today's free limit of 20 questions. Log in to keep practising for free.

Explanation

The NCERT lists as an important feature: 'Expression for equilibrium constant is applicable only when concentrations of the reactants and products have attained constant value at equilibrium state.'

NEET 2023

● ● ● ● ●

Amongst the given options which of the following molecules/ions acts as a Lewis acid?

A. NH₃ B. H₂O C. BF₃ D. OH⁻

You've reached today's free limit of 20 questions. Log in to keep practising for free.

Explanation

BF₃ has incomplete octet around B and accepts an electron pair.

Ready to ace NEET?

Free access · No credit card required

Browse All Questions Create Free Account

Frequently Asked Questions

Yes. You can attempt every Equilibrium question on this page for free without logging in, and check the correct answer with a detailed explanation instantly.

No account is required to attempt questions and view answers. A free account adds bookmarks, personal notes, and progress tracking.

The bank mixes NEET previous year questions (PYQs) with practice questions, each tagged with its exam appearances where applicable.