Grade 11 : Chemistry - Equilibrium (Set 3)

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Grade 11 : Chemistry - Equilibrium (Set 3)— Questions & Detailed Solutions

An ice-water system is maintained at 273 K and 1 atm in a closed insulated cylinder fitted with a frictionless piston.
Which of the following statements correctly describes what happens when the external pressure on the system is increased?

(A)

The melting point of ice increases, and more ice forms.

(B)

The melting point of ice decreases, and more ice melts.

(C)

Equilibrium remains completely unaffected because both phases are condensed states.

(D)

Water vapor pressure increases while the amount of liquid water decreases.

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation:For the phase transition $\text{Ice} \rightleftharpoons \text{Water}$, liquid water has higher density than ice, meaning water occupies a smaller volume. By Le Chatelier's principle, increasing pressure shifts equilibrium towards the lower volume phase (liquid water). Consequently, the melting point of ice decreases and more ice melts.

For the gas-phase reaction $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$ at 700 K, if $K_c = 3.0 \times 10^2\text{ L mol}^{-1}$, what is the value of $K_p$ in $\text{atm}^{-1}$? (Use $R = 0.0821\text{ L atm K}^{-1}\text{mol}^{-1}$)

(A)

$1.72 \times 10^4$

(B)

5.22

(C)

300

(D)

0.191

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation:The relationship between $K_p$ and $K_c$ is given by $K_p = K_c(RT)^{\Delta n_g}$. Here, $\Delta n_g = 2 - (2 + 1) = -1$. Substituting values: $K_p = 300 \times (0.0821 \times 700)^{-1} = 300 / 57.47 = 5.22\text{ atm}^{-1}$.

A 2.0 L rigid vessel initially contains 0.4 mol of gas $A$ and 0.8 mol of gas $B$. They react according to the equation: $A(g) + 2B(g) \rightleftharpoons C(g)$. At equilibrium, 0.2 mol of gas $C$ is present.
What is the equilibrium constant $K_c$ for this reaction?

(A)

$12.5m^{-2}$

(B)

$25.0m^{-2}$

(C)

$50.0m^{-2}$

(D)

$6.25m^{-2}$

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation:At equilibrium, moles formed of $C = 0.2\text{ mol}$. Moles of $A$ remaining $= 0.4 - 0.2 = 0.2\text{ mol}$. Moles of $B$ remaining $= 0.8 - 2(0.2) = 0.4\text{ mol}$. Concentrated values in 2.0 L: $[A] = 0.1m$, $[B] = 0.2m$, $[C] = 0.1m$. $K_c = \frac{[C]}{[A][B]^2} = \frac{0.1}{(0.1)(0.2)^2} = \frac{1}{0.04} = 25.0m^{-2}$.

Given the following equilibrium constants at 1000 K:
(1) $N_2(g) + O_2(g) \rightleftharpoons 2NO(g)$, $K_1 = 4.0 \times 10^{-4}$
(2) $NO(g) + \frac{1}{2}O_2(g) \rightleftharpoons NO_2(g)$, $K_2 = 1.0 \times 10^2$
What is the equilibrium constant $K_3$ for the reaction $2NO_2(g) \rightleftharpoons N_2(g) + 2O_2(g)$?

(A)

0.25

(B)

4.00

(C)

$2.5 \times 10^{-3}$

(D)

$4.0 \times 10^{-2}$

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation:To obtain $N_2(g) + 2O_2(g) \rightleftharpoons 2NO_2(g)$, add reaction (1) and $2 \times$ reaction (2). The equilibrium constant for this combination is $K_{\text{forward}} = K_1 \times K_2^2 = (4.0 \times 10^{-4}) \times (10^2)^2 = 4.0$. The target reaction is the exact reverse of this combination, so $K_3 = \frac{1}{K_{\text{forward}}} = \frac{1}{4.0} = 0.25$.

For the gaseous equilibrium system $PCl_5(g) \rightleftharpoons PCl_3(g) + Cl_2(g)$, what is the effect of adding an inert gas like Helium at constant pressure?

(A)

The equilibrium shifts in the forward direction.

(B)

The equilibrium shifts in the backward direction.

(C)

The equilibrium remains completely unaffected.

(D)

The equilibrium constant $K_c$ increases.

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation:Adding an inert gas at constant pressure increases the overall volume of the system. The system shifts in the direction that produces a greater number of moles of gas (where $\Delta n_g > 0$). For $PCl_5 \rightleftharpoons PCl_3 + Cl_2$, $\Delta n_g = +1$, so the reaction shifts forward.

For the reaction $A(g) + B(g) \rightleftharpoons 2C(g)$, the equilibrium constant $K_c$ is 16. At a given instant, a reaction vessel contains $[A] = 0.5m$, $[B] = 0.5m$, and $[C] = 4.0m$.
Which statement correctly describes the state and direction of the reaction system?

(A)

The system is at equilibrium because $Q_c = K_c$.

(B)

$Q_c > K_c$; the reaction will proceed in the backward direction to reach equilibrium.

(C)

$Q_c < K_c$; the reaction will proceed in the forward direction to reach equilibrium.

(D)

The reaction has ceased completely.

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation:Calculate the reaction quotient: $Q_c = \frac{[C]^2}{[A][B]} = \frac{(4.0)^2}{(0.5)(0.5)} = \frac{16}{0.25} = 64$. Since $Q_c (64) > K_c (16)$, products must decrease and reactants must increase; hence the reaction shifts backward.

Which of the following species acts as a Brønsted-Lowry base but NOT as an Arrhenius base in aqueous medium?

(A)

NaOH

(B)

KOH

(C)

$NH_3$

(D)

$Ca(OH)_2$

View Correct Answer & Detailed Solution

✓ Correct Option: (C)

Explanation:$NH_3$ acts as a Brønsted-Lowry base because it accepts a proton ($H^+$) to form $NH_4^+$. However, it is not an Arrhenius base because it does not possess hydroxide ($OH^-$) ions in its chemical formula to directly yield $OH^-$ upon dissociation.

What is the conjugate base of the hydrogenphosphate ion, $HPO_4^{2-}$?

(A)

$H_3PO_4$

(B)

$H_2PO_4^-$

(C)

$PO_4^{3-}$

(D)

$H_4PO_4^+$

View Correct Answer & Detailed Solution

✓ Correct Option: (C)

Explanation:A conjugate base is formed by removing one proton ($H^+$) from an acid species. Removing $H^+$ from $HPO_4^{2-}$ yields $PO_4^{3-}$ (phosphate ion).

Equal volumes of $0.02m HCl$ solution and $0.04m HNO_3$ solution are mixed together. What is the pH of the resulting mixture? (Given: $\log_{10} 3 \approx 0.48$)

(A)

1.22

(B)

1.52

(C)

1.70

(D)

2.00

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation:Let equal volume be $V$. Total moles of $H^+ = (0.02 \times V) + (0.04 \times V) = 0.06V$. Total volume $= 2V$. Resulting $[H^+] = \frac{0.06V}{2V} = 0.03m = 3 \times 10^{-2}m$. $\text{pH} = -\log(3 \times 10^{-2}) = 2 - \log 3 = 2 - 0.48 = 1.52$.

Q10

A 0.10 M aqueous solution of a weak monobasic acid HA has an ionization constant $K_a = 1.0 \times 10^{-5}$. What is the pH of this solution?

(A)

1.0

(B)

3.0

(C)

5.0

(D)

7.0

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation:For a weak acid HA, $[H^+] = \sqrt{K_a \cdot C} = \sqrt{1.0 \times 10^{-5} \times 0.10} = \sqrt{10^{-6}} = 10^{-3}m$. Therefore, $\text{pH} = -\log(10^{-3}) = 3.0$.

Q11

If the degree of dissociation of a 0.01 M monobasic weak acid solution is 0.05 (5%), what is its acid dissociation constant $K_a$?

(A)

$2.5 \times 10^{-5}$

(B)

$5.0 \times 10^{-4}$

(C)

$2.5 \times 10^{-3}$

(D)

$1.0 \times 10^{-4}$

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation:According to Ostwald's Dilution Law for weak electrolytes with small $\alpha$: $K_a = C \alpha^2$. Substituting $C = 0.01m$ and $\alpha = 0.05$: $K_a = 0.01 \times (0.05)^2 = 0.01 \times 0.0025 = 2.5 \times 10^{-5}$.

Q12

Given that the acid dissociation constant $K_a$ for the ammonium ion ($NH_4^+$) is $5.6 \times 10^{-10}$ at $25^\circ\text{C}$, what is the base dissociation constant $K_b$ for $NH_3$? ($K_w = 1.0 \times 10^{-14}$)

(A)

$1.79 \times 10^{-5}$

(B)

$5.60 \times 10^{-4}$

(C)

$1.79 \times 10^{-9}$

(D)

$5.60 \times 10^{-24}$

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation:For any conjugate acid-base pair in aqueous solution: $K_a \times K_b = K_w$. Thus, $K_b(NH_3) = \frac{K_w}{K_a(NH_4^+)} = \frac{1.0 \times 10^{-14}}{5.6 \times 10^{-10}} = 1.79 \times 10^{-5}$.

Q13

What is the pH of a 0.10 M solution of sodium acetate ($CH_3COONa$) at $25^\circ\text{C}$? ($K_a \text{ of } CH_3COOH = 1.8 \times 10^{-5}$, $K_w = 1.0 \times 10^{-14}$)

(A)

5.13

(B)

7.00

(C)

8.87

(D)

9.37

View Correct Answer & Detailed Solution

✓ Correct Option: (C)

Explanation:Sodium acetate is a salt of a weak acid and strong base. Its pH formula is $\text{pH} = 7 + \frac{1}{2}\text{p}K_a + \frac{1}{2}\log C$. Here $\text{p}K_a = -\log(1.8 \times 10^{-5}) = 4.74$, $\log C = \log(0.1) = -1$. $\text{pH} = 7 + 2.37 - 0.50 = 8.87$.

Q14

An acidic buffer contains $0.20m CH_3COOH$ and $0.20m CH_3COONa$ ($\text{p}K_a = 4.74$).
What will be the resulting pH of the solution if $0.05m HCl$ is added (assuming negligible volume change)?

(A)

4.96

(B)

4.74

(C)

4.52

(D)

4.22

View Correct Answer & Detailed Solution

✓ Correct Option: (C)

Explanation:Adding $0.05m HCl$ converts 0.05 M of $CH_3COO^-$ into $CH_3COOH$. New concentrations: $[CH_3COOH] = 0.20 + 0.05 = 0.25m$, $[CH_3COO^-] = 0.20 - 0.05 = 0.15m$. By Henderson-Hasselbalch equation: $\text{pH} = 4.74 + \log\left(\frac{0.15}{0.25}\right) = 4.74 + \log(0.60) = 4.74 - 0.22 = 4.52$.

Q15

A basic buffer solution contains $0.10m NH_3$ and $0.10m NH_4Cl$. Given $K_b$ of $NH_3 = 1.8 \times 10^{-5}$ ($\text{p}K_b = 4.74$), what is the pH of this buffer at $25^\circ\text{C}$?

(A)

4.74

(B)

7.00

(C)

9.26

(D)

11.52

View Correct Answer & Detailed Solution

✓ Correct Option: (C)

Explanation:Using Henderson-Hasselbalch equation for basic buffer: $\text{pOH} = \text{p}K_b + \log\left(\frac{[\text{salt}]}{[\text{base}]}\right) = 4.74 + \log\left(\frac{0.10}{0.10}\right) = 4.74$. $\text{pH} = 14 - \text{pOH} = 14 - 4.74 = 9.26$.

Q16

The molar solubility of calcium fluoride ($CaF_2$) in pure water at 298 K is $2.0 \times 10^{-4}\text{ mol L}^{-1}$. What is its solubility product ($K_{sp}$)?

(A)

$4.0 \times 10^{-8}$

(B)

$8.0 \times 10^{-12}$

(C)

$3.2 \times 10^{-11}$

(D)

$1.6 \times 10^{-11}$

View Correct Answer & Detailed Solution

✓ Correct Option: (C)

Explanation:Dissociation: $CaF_2(s) \rightleftharpoons Ca^{2+} + 2F^-$. If solubility is $S$: $[Ca^{2+}] = S$, $[F^-] = 2S$. $K_{sp} = [Ca^{2+}][F^-]^2 = S(2S)^2 = 4S^3$. Substituting $S = 2.0 \times 10^{-4}m$: $K_{sp} = 4 \times (2.0 \times 10^{-4})^3 = 4 \times 8.0 \times 10^{-12} = 3.2 \times 10^{-11}$.

Q17

The solubility product $K_{sp}$ of silver chloride (AgCl) is $1.8 \times 10^{-10}$. What is its molar solubility in a $0.10m NaCl$ solution?

(A)

$1.34 \times 10^{-5}m$

(B)

$1.80 \times 10^{-9}m$

(C)

$1.80 \times 10^{-11}m$

(D)

$3.24 \times 10^{-10}m$

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation:Due to complete dissociation of NaCl, $[Cl^-] \approx 0.10m$ (common ion effect). $K_{sp} = [Ag^+][Cl^-] \implies 1.8 \times 10^{-10} = S' \times 0.10 \implies S' = 1.8 \times 10^{-9}m$.

Q18

Equal volumes of $0.002m CaCl_2$ solution and $0.004m Na_2SO_4$ solution are mixed. Given $K_{sp}(CaSO_4) = 2.4 \times 10^{-5}$, will a precipitate of $CaSO_4$ form?

(A)

Yes, because $Q_{sp} > K_{sp}$.

(B)

No, because $Q_{sp} < K_{sp}$.

(C)

Yes, because $Q_{sp} = K_{sp}$.

(D)

Precipitation depends solely on solution temperature.

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation:After mixing equal volumes, concentrations are halved: $[Ca^{2+}] = 0.001m$, $[SO_4^{2-}] = 0.002m$. Ionic product $Q_{sp} = [Ca^{2+}][SO_4^{2-}] = (10^{-3}) \times (2 \times 10^{-3}) = 2.0 \times 10^{-6}$. Since $Q_{sp} (2.0 \times 10^{-6}) < K_{sp} (2.4 \times 10^{-5})$, no precipitation occurs.

Q19

Consider the following four chemical species:
(i) $BF_3$, (ii) $NH_3$, (iii) $AlCl_3$, (iv) $H_2O$
Which of the following options correctly classifies these species as Lewis acids or Lewis bases?

(A)

Lewis acids: (i) & (iii); Lewis bases: (ii) & (iv)

(B)

Lewis acids: (ii) & (iv); Lewis bases: (i) & (iii)

(C)

All four are Lewis acids

(D)

All four are Lewis bases

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation:$BF_3$ and $AlCl_3$ are electron-deficient molecules with incomplete octets capable of accepting electron pairs (Lewis acids). $NH_3$ and $H_2O$ possess lone pairs of electrons available for donation (Lewis bases).

Q20

For the gas-phase dissociation $N_2O_4(g) \rightleftharpoons 2NO_2(g)$, the theoretical vapor density of $N_2O_4$ is $D = 46$. At a specific temperature, the observed vapor density $d$ of the equilibrium mixture is found to be 30.67.
What is the degree of dissociation ($\alpha$) of $N_2O_4$?

(A)

0.25

(B)

0.33

(C)

0.50

(D)

0.75

View Correct Answer & Detailed Solution

✓ Correct Option: (C)

Explanation:For a dissociation reaction producing $n$ moles of gaseous product per mole of reactant ($n = 2$ for $N_2O_4 \rightarrow 2NO_2$), degree of dissociation is $\alpha = \frac{D - d}{(n - 1)d}$. Substituting values: $\alpha = \frac{46 - 30.67}{(2 - 1) \times 30.67} = \frac{15.33}{30.67} = 0.50$.

Grade 11 : Chemistry - Equilibrium (Set 3)

Grade 11 : Chemistry - Equilibrium (Set 3)— Questions & Detailed Solutions

An ice-water system is maintained at 273 K and 1 atm in a closed insulated cylinder fitted with a frictionless piston.
Which of the following statements correctly describes what happens when the external pressure on the system is increased?

For the gas-phase reaction $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$ at 700 K, if $K_c = 3.0 \times 10^2\text{ L mol}^{-1}$, what is the value of $K_p$ in $\text{atm}^{-1}$? (Use $R = 0.0821\text{ L atm K}^{-1}\text{mol}^{-1}$)

A 2.0 L rigid vessel initially contains 0.4 mol of gas $A$ and 0.8 mol of gas $B$. They react according to the equation: $A(g) + 2B(g) \rightleftharpoons C(g)$. At equilibrium, 0.2 mol of gas $C$ is present.
What is the equilibrium constant $K_c$ for this reaction?

For the gaseous equilibrium system $PCl_5(g) \rightleftharpoons PCl_3(g) + Cl_2(g)$, what is the effect of adding an inert gas like Helium at constant pressure?

For the reaction $A(g) + B(g) \rightleftharpoons 2C(g)$, the equilibrium constant $K_c$ is 16. At a given instant, a reaction vessel contains $[A] = 0.5m$, $[B] = 0.5m$, and $[C] = 4.0m$.
Which statement correctly describes the state and direction of the reaction system?

Which of the following species acts as a Brønsted-Lowry base but NOT as an Arrhenius base in aqueous medium?

What is the conjugate base of the hydrogenphosphate ion, $HPO_4^{2-}$?

Equal volumes of $0.02m HCl$ solution and $0.04m HNO_3$ solution are mixed together. What is the pH of the resulting mixture? (Given: $\log_{10} 3 \approx 0.48$)

A 0.10 M aqueous solution of a weak monobasic acid HA has an ionization constant $K_a = 1.0 \times 10^{-5}$. What is the pH of this solution?

If the degree of dissociation of a 0.01 M monobasic weak acid solution is 0.05 (5%), what is its acid dissociation constant $K_a$?

Given that the acid dissociation constant $K_a$ for the ammonium ion ($NH_4^+$) is $5.6 \times 10^{-10}$ at $25^\circ\text{C}$, what is the base dissociation constant $K_b$ for $NH_3$? ($K_w = 1.0 \times 10^{-14}$)

What is the pH of a 0.10 M solution of sodium acetate ($CH_3COONa$) at $25^\circ\text{C}$? ($K_a \text{ of } CH_3COOH = 1.8 \times 10^{-5}$, $K_w = 1.0 \times 10^{-14}$)

An acidic buffer contains $0.20m CH_3COOH$ and $0.20m CH_3COONa$ ($\text{p}K_a = 4.74$).
What will be the resulting pH of the solution if $0.05m HCl$ is added (assuming negligible volume change)?

A basic buffer solution contains $0.10m NH_3$ and $0.10m NH_4Cl$. Given $K_b$ of $NH_3 = 1.8 \times 10^{-5}$ ($\text{p}K_b = 4.74$), what is the pH of this buffer at $25^\circ\text{C}$?

The molar solubility of calcium fluoride ($CaF_2$) in pure water at 298 K is $2.0 \times 10^{-4}\text{ mol L}^{-1}$. What is its solubility product ($K_{sp}$)?

The solubility product $K_{sp}$ of silver chloride (AgCl) is $1.8 \times 10^{-10}$. What is its molar solubility in a $0.10m NaCl$ solution?

Equal volumes of $0.002m CaCl_2$ solution and $0.004m Na_2SO_4$ solution are mixed. Given $K_{sp}(CaSO_4) = 2.4 \times 10^{-5}$, will a precipitate of $CaSO_4$ form?

Consider the following four chemical species:
(i) $BF_3$, (ii) $NH_3$, (iii) $AlCl_3$, (iv) $H_2O$
Which of the following options correctly classifies these species as Lewis acids or Lewis bases?

For the gas-phase dissociation $N_2O_4(g) \rightleftharpoons 2NO_2(g)$, the theoretical vapor density of $N_2O_4$ is $D = 46$. At a specific temperature, the observed vapor density $d$ of the equilibrium mixture is found to be 30.67.
What is the degree of dissociation ($\alpha$) of $N_2O_4$?

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Grade 11 : Chemistry - Equilibrium (Set 3)

Grade 11 : Chemistry - Equilibrium (Set 3)— Questions & Detailed Solutions

An ice-water system is maintained at 273 K and 1 atm in a closed insulated cylinder fitted with a frictionless piston.Which of the following statements correctly describes what happens when the external pressure on the system is increased?

For the gas-phase reaction $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$ at 700 K, if $K_c = 3.0 \times 10^2\text{ L mol}^{-1}$, what is the value of $K_p$ in $\text{atm}^{-1}$? (Use $R = 0.0821\text{ L atm K}^{-1}\text{mol}^{-1}$)

A 2.0 L rigid vessel initially contains 0.4 mol of gas $A$ and 0.8 mol of gas $B$. They react according to the equation: $A(g) + 2B(g) \rightleftharpoons C(g)$. At equilibrium, 0.2 mol of gas $C$ is present.What is the equilibrium constant $K_c$ for this reaction?

For the gaseous equilibrium system $PCl_5(g) \rightleftharpoons PCl_3(g) + Cl_2(g)$, what is the effect of adding an inert gas like Helium at constant pressure?

For the reaction $A(g) + B(g) \rightleftharpoons 2C(g)$, the equilibrium constant $K_c$ is 16. At a given instant, a reaction vessel contains $[A] = 0.5m$, $[B] = 0.5m$, and $[C] = 4.0m$.Which statement correctly describes the state and direction of the reaction system?

Which of the following species acts as a Brønsted-Lowry base but NOT as an Arrhenius base in aqueous medium?

What is the conjugate base of the hydrogenphosphate ion, $HPO_4^{2-}$?

Equal volumes of $0.02m HCl$ solution and $0.04m HNO_3$ solution are mixed together. What is the pH of the resulting mixture? (Given: $\log_{10} 3 \approx 0.48$)

A 0.10 M aqueous solution of a weak monobasic acid HA has an ionization constant $K_a = 1.0 \times 10^{-5}$. What is the pH of this solution?

If the degree of dissociation of a 0.01 M monobasic weak acid solution is 0.05 (5%), what is its acid dissociation constant $K_a$?

Given that the acid dissociation constant $K_a$ for the ammonium ion ($NH_4^+$) is $5.6 \times 10^{-10}$ at $25^\circ\text{C}$, what is the base dissociation constant $K_b$ for $NH_3$? ($K_w = 1.0 \times 10^{-14}$)

What is the pH of a 0.10 M solution of sodium acetate ($CH_3COONa$) at $25^\circ\text{C}$? ($K_a \text{ of } CH_3COOH = 1.8 \times 10^{-5}$, $K_w = 1.0 \times 10^{-14}$)

An acidic buffer contains $0.20m CH_3COOH$ and $0.20m CH_3COONa$ ($\text{p}K_a = 4.74$).What will be the resulting pH of the solution if $0.05m HCl$ is added (assuming negligible volume change)?

A basic buffer solution contains $0.10m NH_3$ and $0.10m NH_4Cl$. Given $K_b$ of $NH_3 = 1.8 \times 10^{-5}$ ($\text{p}K_b = 4.74$), what is the pH of this buffer at $25^\circ\text{C}$?

The molar solubility of calcium fluoride ($CaF_2$) in pure water at 298 K is $2.0 \times 10^{-4}\text{ mol L}^{-1}$. What is its solubility product ($K_{sp}$)?

The solubility product $K_{sp}$ of silver chloride (AgCl) is $1.8 \times 10^{-10}$. What is its molar solubility in a $0.10m NaCl$ solution?

Equal volumes of $0.002m CaCl_2$ solution and $0.004m Na_2SO_4$ solution are mixed. Given $K_{sp}(CaSO_4) = 2.4 \times 10^{-5}$, will a precipitate of $CaSO_4$ form?

Consider the following four chemical species:(i) $BF_3$, (ii) $NH_3$, (iii) $AlCl_3$, (iv) $H_2O$Which of the following options correctly classifies these species as Lewis acids or Lewis bases?

For the gas-phase dissociation $N_2O_4(g) \rightleftharpoons 2NO_2(g)$, the theoretical vapor density of $N_2O_4$ is $D = 46$. At a specific temperature, the observed vapor density $d$ of the equilibrium mixture is found to be 30.67.What is the degree of dissociation ($\alpha$) of $N_2O_4$?

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An ice-water system is maintained at 273 K and 1 atm in a closed insulated cylinder fitted with a frictionless piston.
Which of the following statements correctly describes what happens when the external pressure on the system is increased?

A 2.0 L rigid vessel initially contains 0.4 mol of gas $A$ and 0.8 mol of gas $B$. They react according to the equation: $A(g) + 2B(g) \rightleftharpoons C(g)$. At equilibrium, 0.2 mol of gas $C$ is present.
What is the equilibrium constant $K_c$ for this reaction?

For the reaction $A(g) + B(g) \rightleftharpoons 2C(g)$, the equilibrium constant $K_c$ is 16. At a given instant, a reaction vessel contains $[A] = 0.5m$, $[B] = 0.5m$, and $[C] = 4.0m$.
Which statement correctly describes the state and direction of the reaction system?

An acidic buffer contains $0.20m CH_3COOH$ and $0.20m CH_3COONa$ ($\text{p}K_a = 4.74$).
What will be the resulting pH of the solution if $0.05m HCl$ is added (assuming negligible volume change)?

Consider the following four chemical species:
(i) $BF_3$, (ii) $NH_3$, (iii) $AlCl_3$, (iv) $H_2O$
Which of the following options correctly classifies these species as Lewis acids or Lewis bases?

For the gas-phase dissociation $N_2O_4(g) \rightleftharpoons 2NO_2(g)$, the theoretical vapor density of $N_2O_4$ is $D = 46$. At a specific temperature, the observed vapor density $d$ of the equilibrium mixture is found to be 30.67.
What is the degree of dissociation ($\alpha$) of $N_2O_4$?