Match the following equilibria with the corresponding condition.

A. LiquidVapour 1. Saturated solution
B. SolidLiquid 2. Boiling point
C. SolidVapour 3. Sublimation point
D. Solute (s)Solute (solution) 4. Melting point
5. Unsaturated solution

Codes

A B C D
1. 2 4 3 1
2. 1 2 3 5
3. 5 4 3 2
4. 4 5 3 2
Subtopic:  Introduction To Equilibrium |
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In the reaction, N2O4  2NO2α is that part of N2O4 which dissociates. The number of moles at equilibrium will be:

1. 1-α2

2. 3α

3. α

4. 1+α

Subtopic:  Introduction To Equilibrium |
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I2(s) + 5F2(g)  2IF5(g) 

The equilibrium constant Kc expression for the above mentioned reaction is:

1. KC= IF52F25
2. KC= IF52F25I2
3. KC =F25I2IF22
4.  KC =F25IF52

Subtopic:  Introduction To Equilibrium |
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Ka1, Ka2 and Ka3 are the respective ionisation constants for the following reactions.
\(\mathrm{H}_2 \mathrm{~S} \rightleftharpoons \mathrm{H}^{+}+\mathrm{HS}^{-}\)
\(\mathrm{HS}^{-} \rightleftharpoons \mathrm{H}^{+}+\mathrm{S}^{2-}\)
\(\mathrm{H}_2 \mathrm{~S} \rightleftharpoons 2 \mathrm{H}^{+}+\mathrm{S}^{2-}\)
The correct relationship between Ka1, Ka2 and Ka3 is:

1. \(\mathrm{K}_{\mathrm{a}_3}=\mathrm{K}_{\mathrm{a}_1} \times \mathrm{K}_{\mathrm{a}_2} \) 2. \(\mathrm{K}_{\mathrm{a}_3}=\mathrm{K}_{\mathrm{a}_1}+\mathrm{K}_{\mathrm{a}_2} \)
3. \(K_{a_3}=K_{a_1}-K_{a_2} \) 4. \(\mathrm{K}_{\mathrm{a}_3}=\mathrm{K}_{\mathrm{a}_1} / \mathrm{K}_{\mathrm{a}_2}\)
Subtopic:  Introduction To Equilibrium |
 80%
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If the molar concentration of SnCl4 is 1.5 × 10-3 mol L–1, the concentration of chloride ions will be:

1. 3.0 x 10-3 2. 6.0 x 10-3
3. 0.3 x 10-3 4. 0.6 x 10-6
Subtopic:  Introduction To Equilibrium |
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Reaction quotient for the reaction, N2(g)+3H2(g)2NH3(g) is given by , Q = [NH3]2[N2][H2]3 .The reaction will proceed from right to left if Kc value is:

1. Q<Kc  2. Q=0
3. Q>Kc  4. Q=Kc 
Subtopic:  Introduction To Equilibrium |
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An incorrect statement about equilibrium among the following is:

1. Equilibrium is possible only in a closed system at a given temperature.
2. All measurable properties of the system remain constant.
3. All the physical processes stop at equilibrium.
4. The opposing processes occur at the same rate and there is a dynamic but stable condition.
Subtopic:  Introduction To Equilibrium |
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For a reaction, 2NO (g) + Br2 (g)  2NOBr (g)

When 0.087 mol of NO and 0.0437 mol of Br2 are mixed in a closed container at a constant temperature, 0.0518 mol of NOBr is obtained at equilibrium. The concentration of NO and Br2 at equilibrium will be:

1. NO = 0.0352 mol; Br2= 0.0178 mol

2. NO = 0.352 mol; Br2= 0.178 mol

3. NO = 0.0634 mol; Br2= 0.0596 mol

4. NO = 0.634 mol; Br2= 0.596 mol

Subtopic:  Introduction To Equilibrium |
 70%
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In the reaction A(g) + 2B(g) ⇌ 2C(g) + D(g), the initial concentration of B is twice that of A and, at equilibrium, the concentrations of A and D are equal. The value of the equilibrium constant will be:

1. 4 2. 16
3. 2 4. 1
Subtopic:  Introduction To Equilibrium |
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Which of the following is an example of a reversible reaction?
1. \(\small{KNO_3(aq) + NaCl(aq) \rightleftharpoons KCl(aq) + NaNO_3(aq)}\)
2. \(\small{2Na(s) + H_2O(l) \rightleftharpoons 2NaOH(aq) + H_2(g)}\)
3. \(\small{AgNO_3(aq) + NaCl(aq) \rightleftharpoons AgCl(s) + NaNO_3(aq)}\)
4. \(\small{Pb{(NO_3)}_2(aq) + 2NaI(aq) \rightleftharpoons PbI_2(s) + 2NaNO_3(aq)}\)

Subtopic:  Introduction To Equilibrium |
 59%
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