AIIMS Chemistry Equilibrium Class 11 Questions

Assertion: Ferromagnetic compound is more attracted in magnetic field.

Reason: Because all electron are aligned in same direction.

Which of the following has max. solubility at low pH?

The value of ionic product of water at $393\text{ K}$ is

For the endothermic reaction $\text{A}_2 \rightarrow 2\text{A}$, which of the following will increase yield of monomer?

Assertion: $\text{H}_2\text{O}$ shows atmospheric nature.

Reason: According to Bronsted theory, it acts as acid with $\text{NH}_3$ and a base with $\text{H}_2\text{S}$.

Assertion : If value ofequilibrium constant is $K_c$ for $A + B \rightleftharpoons C$. If chemical reaction is reversed $C \rightleftharpoons A + B$., then value of equilibrium constant will be $1/K_c$.Reason : Equilibrium constant depends upon the expression of chemical reaction.

Solubility of a sparingly soluble salt $\text{XB}_2$ in water is $x$. What will be its solubility in a solution of $\text{yB}$ having concentration of $0.001\text{M}$ ?

$20\text{ mL}$ of $0.1\text{ M}$ acetic acid is mixed in a solution of $\text{NaOH}$. If $10\text{ mL}$ of $0.1\text{ M}$ $\text{NaOH}$ is present, then $\text{H}^+$ concentration in the resulting solution is ($\text{K}_\text{a}\text{ of acetic acid} = 1.7 \times 10^{-5}$)

CaCO₃(s) → CaO(s) + CO₂(g) at constant temperature, the pressure will increase if:

What happens on increasing pressure at constant temperature?

Calculate ionisation constant for pyridinium chloride, Given that $\text{H}^+$ ion concentration is $3.6 \times 10^{-4}\text{ M}$ and its concentration is $0.02\text{ M}$.

Which is least soluble in aqueous medium?

Mixture of two metals having mass $2\text{ gm }(A = 15, B = 30)$ and are bivalent and dissolve in $\text{HCl}$ and evolve $2.24\text{ L }\text{H}_2$ at STP. what is mass of A present in mixture?

$\text{A} + 2\text{B} \rightleftharpoons 2\text{C} \quad \text{K} = ?$

$2\text{ mole}$ each $\text{A}$ and $\text{B}$ present in $10\text{ lt}$ so that $\text{C}$ form is $1\text{ mole}$, Calculate $\text{K}_\text{c}$

$\text{CH}_3 - \text{CH} = \text{CH} - \text{CH} = \text{N} - \text{CH}_3 \xrightarrow{\text{LiAlH}_4} \text{What is final product?}$

Question : $\text{K}_\text{c}$ for the reaction $\text{N}_2\text{(g)} + \text{O}_2\text{(g)} \rightleftharpoons 2\text{NO(g)}$ at $300\text{ K}$ is $4.0 \times 10^{-6}$. $\text{K}_\text{p}$ for the above reaction will be $(\text{R} = 2\text{ cal mol}^{-1}\text{K}^{-1})$

Assertion: Na₂SO₃ solution give basic solution in litmus solution Reason: It react with water and H₂SO₃ form

Assertion : If $Q_c$ (reaction quotient) $< K_c$ (equilibrium constant) reaction moves in direction of reactants.

Reason : Reaction quotient is defined in the same way as equilibrium constant at any stage of the reaction.

For the reaction:

$\text{H}_2(\text{g}) + \text{CO}_2(\text{g}) \rightleftharpoons \text{CO}(\text{g}) + \text{H}_2\text{O}(\text{g})$

If the initial concentration of $[\text{H}_2] = [\text{CO}_2]$ and $x\text{ mol/L}$ of hydrogen is consumed at equilibrium, the correct expression of $k_p$ is:

Calculate the degree of hydrolysis and $\text{pH}$ of $0.02\text{ M}$ ammonium cyanide ($\text{NH}_4\text{CN}$) at $298\text{ K}$

($K_a \text{ of HCN} = 4.99 \times 10^{-9}$, $K_b \text{ of NH}_4\text{OH} = 1.77 \times 10^{-5}$)

Assertion (A): Adding an inert gas to the dissociation equilibrium of $\text{N}_2\text{O}_4$ at constant temperature and pressure increases the dissociation.

Reason (R): Due to the addition of the inert gas, the molar concentration of reactants and products decreases.

Kₚ for the reaction A ⇌ B is 4. If initially only A is present then what will be the partial pressure of B after equilibrium?

‘a’ moles of PCl₅ are heated in a closed container to equilibrate PCl₅(g) ⇌ PCl₃(g) + Cl₂(g) at pressure of p atm. If x moles of PCl₅ dissociate at equilibrium, then

Consider the reaction equilibrium Ice ⇌ Water – x kcal The favourable conditions for forward reaction are

In a basic buffer, 0.0025 mole of NH₄Cl and 0.15 mole of NH₄OH are present. The pH of the solution will be (pKₐ) = 4.74.

For the gas phase reaction, C2H4 + H2 ⇌ C2H6; [ΔH = -32.7 kcal] Carried out in a vessel, the equilibrium concentration of C2H4 can be increased by

Assertion: A catalyst does not influence the value of equilibrium constant. Reason: Catalyst influence the rate of both forward and backward reactions equally.

Which has the highest pH?

$\frac{K_p}{K_c}$ for following reaction will be $\text{CO}_{(g)} + \frac{1}{2}\text{O}_{2(g)} \rightarrow \text{CO}_{2(g)}$

At 60° and 1 atm, N₂O₄ is 50% dissociated into NO₂ then Kₚ is

Kₛₚ of CaSO₄·5H₂O is 9 × 10⁻⁶, find the volume for 1 g of CaSO₄ (M.wt. = 136).

Which of the following is not a characteristic of equilibrium?

25 mL, 0.2 M Ca(OH)₂ is neutralised by 10 mL of 1 M HCl. Then pH of resulting solution is

What is the pH of 0.01 M glycine solution? For glycine Ka₁ = 4.5×10⁻³ and Ka₂ = 1.7×10⁻¹⁰ at 298 K.

Assertion: The equilibrium constant is fixed and a characteristic for any given chemical reaction at a specified temperature. Reason: The composition of the final equilibrium mixture at a particular temperature depends upon the starting amount of reactants.

pH of a 0.01 M solution (Kₐ = 6.6 × 10⁻⁴)

A vessel of one litre capacity containing 1 mole of SO₃ is heated till a state of equilibrium is attained. 2SO₃(g) ⇌ 2SO₂(g) + O₂(g). At equilibrium, 0.6 moles of SO₂ had formed. The value of equilibrium constant is

The equilibrium constant for mutarotation of α-D Glucose ⇌ β-D Glucose is 1.8. What percentage of α form remains at equilibrium?

Assertion: Ice ⟶ water, if pressure is applied water will evaporate. Reason: Increases of pressure pushes the equilibrium towards the side in which number of gaseous molecule increases.

Assertion: In an acid-base titration involving strong base and a weak acid, methyl orange can be used as an indicator. Reason: Methyl orange changes its colour in pH range of 7 to 9.

What is the correct relationship between the pHs of isomolar solutions of sodium oxide (pH₁), sodium sulphide (pH₂), sodium selenide (pH₃) and sodium telluride (pH₄)?

The dissociation equilibrium of a gas AB₂ can be represented as 2AB₂(g) ⇌ 2AB(g) + B₂(g). The degree of dissociation is x and is small compared to 1. The expression relating the degree of dissociation (x) with equilibrium constant Kₚ and total pressure p is

The correct order of increasing [H₃O⁺] in the following aqueous solutions is

Assertion: According to Le⁻Chatelier’s principle addition of heat to an equilibrium solid ⇌ liquid results in decrease in the amount of solid.

Reason: Reaction is endothermic, so on heating forward reaction is favoured.

The pH of the solution obtained on neutralisation of 40 mL 0.1 M NaOH with 40 mL 0.1 M CH₃COOH is

Assertion : Mixture of CH₃COOH and CH₃COONH₄ is an example of acidic buffer.

Reason : Acidic buffer contains equimolar mixture of weak acid and its salt with weak base.

Assertion : The equilibrium constant is fixed and a characteristic for any given chemical reaction at a specified temperature.

Reason : The composition of the final equilibrium mixture at a particular temperature depends upon the starting amount of reactants.

40 ml of 0.1 M ammonia solution is mixed with 20 ml of 0.1 M HCl. What is the pH of the mixture? (pKₐ of ammonia solution is 4.74)

Assertion : Sb₂S₃ is not soluble in yellow ammonium sulphide.

Reason : The common ion effect due to S²⁻ ions reduces the solubility of Sb₂S₃.

When 10 ml of 0.1 M acetic acid (pKₐ = 5.0) is titrated against 10 ml of 0.1 M ammonia solution (pKₐ = 5.0), the equivalence point occurs at pH