# At 500 K, equilibrium constant, Kc, for the following reaction is 5. $\frac{1}{2}{\mathrm{H}}_{2}\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{I}}_{2}\left(\mathrm{g}\right)⇌\mathrm{HI}\left(\mathrm{g}\right)$ What would be the equilibrium constant Kc for the reaction? $2\mathrm{HI}\left(\mathrm{g}\right)⇌{\mathrm{H}}_{2}\left(\mathrm{g}\right)+{\mathrm{I}}_{2}\left(\mathrm{g}\right)$ 1.  0.04 2.  0.4 3.  25 4.  2.5

Subtopic:  Kp, Kc & Factors Affecting them |
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The addition of a small amount of argon at a constant volume will not affect the equilibrium of the following reaction:

 1 H2(g)+I2(g)⇌2HI(g) 2 PCl5(g)⇌ PCl3(g)+Cl2(g) 3 N2(g)+3H2(g)⇌2NH3(g) 4 The equilibrium will remain unaffected in all the three cases.

Subtopic:  Le Chatelier's principle |
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On increasing the pressure, the direction in which the gas phase reaction proceeds to re-establish equilibrium is predicted by applying Le-Chatelier's principle. Consider the reaction,

${\mathrm{N}}_{2}\left(\mathrm{g}\right)+3{\mathrm{H}}_{2}\left(\mathrm{g}\right)⇌2{\mathrm{NH}}_{3}\left(\mathrm{g}\right)$

Which of the following is correct, if the total pressure at which the equilibrium is established is increased without changing the temperature?

 1 K will remain the same. 2 K will decrease. 3 K will increase. 4 K will increase initially and then decrease, when pressure is very high.

Subtopic:  Le Chatelier's principle |
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Which of the following alternatives best describes the reaction A ⇌ B at its halfway point?
1. $$\Delta G^{\ominus}=0$$
2. $$\Delta G^{\ominus}>0$$
3. $$\Delta G^{\ominus}<0$$
4. $$\Delta G^{\ominus}=-RTlnK$$

Subtopic:  Kp, Kc & Factors Affecting them |
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${\mathrm{K}}_{\mathrm{a}}$ for ${\mathrm{CH}}_{3}\mathrm{COOH}$ is $1.8×{10}^{-5}$ and Kb for ${\mathrm{NH}}_{4}\mathrm{OH}$ is $1.8×{10}^{-5}$. The pH of ammonium acetate will be:

1. 7.005

2. 4.75

3. 7.0

4. Between 6 and 7

Subtopic:  Salt Hydrolysis & Titration |
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The value of the pH of $$0.01$$ $$\text{mol dm}^{-3}$$$$\text{CH}_3\text{COOH}$$ $$\left(K_a=1.74 \times 10^{-5}\right)$$  is:

 1 3.4 2 3.6 3 3.9 4 3
Subtopic:  pH calculation |
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Among the following solvents, silver chloride is most soluble in:

1.  solution

2.  solution

3. ${\mathrm{H}}_{2}\mathrm{O}$

4. Aqueous ammonia

Subtopic:  Common Ion Effect |
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The mixture that will produce a buffer solution when mixed in equal volumes is:

 1 0.1 mol dm-3 NH4OH and 0.1 mol dm-3 HCl 2 0.05 mol dm-3 NH4OH and 0.1 mol dm-3 HCl 3 0.1 mol dm-3 NH4OH and 0.05 mol dm-3 HCl 4 0.1 mol dm-3 CH3COONa and 0.1 mol dm-3 NaOH

Subtopic:  Buffer |
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Acidity of BF3 can be explained on the basis of:

1. Arrhenius concept

2. Bronsted Lowry concept

3. Lewis concept

4. Bronsted Lowry as well as Lewis concept

Subtopic:  Acids & Bases - Definitions & Classification |
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${\mathrm{K}}_{{\mathrm{a}}_{1}},$ ${\mathrm{K}}_{{\mathrm{a}}_{2}}$ $\mathrm{and}$ ${\mathrm{K}}_{{\mathrm{a}}_{3}}$ 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 ${\mathrm{K}}_{{\mathrm{a}}_{1}},$ ${\mathrm{K}}_{{\mathrm{a}}_{2}}$ $\mathrm{and}$ ${\mathrm{K}}_{{\mathrm{a}}_{3}}$ 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 |
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