Equilibrium Test

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Equilibrium Test - 73

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Weekly Quiz Competition

Question 1
1 / -0

In which of the following reactions, an increase in volume of the container will favour the formation of products?

A
$$2NO_2 (g) \rightleftharpoons 2NO (g) + O_2 (g)$$

B
$$4NH_3(g) + 5O_2(g) \rightleftharpoons 4NO (g) + 6H_2O (l)$$

C
$$3O_2 (g) \rightleftharpoons 2O_3 (g)$$

D
$$H_2(g) + I_2 (g) \rightleftharpoons 2HI (g)$$

Solution

On increasing the volume of container there will be decrease in pressure since pressure is inversely proportional to volume. According to Le Chatelier's principle the reaction will proceed in that direction where there is increase in pressure. So correct option is $$A$$ since it has more gaseous species in products .
Question 2
1 / -0

For the chemical reaction $$3X(g) + Y(g) \rightleftharpoons X_{3}Y(g)$$ the amount $$X_{3}Y$$ at equilibrium is affected by

A
temperature and pressure

B
temperature only

C
pressure only

D
temperature, pressure and catalyst

Solution

$$3X \left ( g \right )+ Y\left ( g \right )\rightarrow X_{3}Y\left ( g \right )$$

$$\Delta n=1-4=-3$$

From the above reaction, we can see there is a change in mole during the reaction. So an increase in pressure will favour forward the reaction.

Also, the equilibrium constant $$K_{p}$$ changes with temperature and catalyst has no effect on the $$K_{p}$$.

Hence pressure and temperature affect the equilibrium condition.
Question 3
1 / -0

$$K_a$$ value for the acid $$HA$$ is $$1\times 10^{-6}$$. The value of $$K$$ for $$A^- +H_3O^+ \to HA +H_2O$$ is

A
$$1\times 10^{-6}$$

B
$$1\times 10^{12}$$

C
$$1\times 10^{-12}$$

D
$$1\times 10^{6}$$

Solution
Question 4
1 / -0

Aqueous solution of $$HNO_3, KOH, CH_3COOH$$ and $$CH_3COONa$$ of identical concentration are provided. The pair(s) of solution which forms buffer upon mixing is (are)

A
$$HNO_3$$ and $$CH_3COOH$$

B
$$KOH$$ and $$CH_3COONa$$

C
$$HNO_3$$ and $$CH_3COONa$$

D
$$CH_3COOH$$ and $$CH_3COONa$$

Solution

A buffer solution is an aqueous solution consisting of a mixture of a weak acid and its conjugate base or a weak base and its conjugate acid.

Of all options, only in option "D", there is a pair of a weak acid and salt of its conjugate base.

Hence, Option "D" is the correct answer.
Question 5
1 / -0

The hydrogen ion concentration of a slightly acidic water solution can be represented by

A
$$10^{-pOH}$$

B
$$14 - pOH$$

C
$$\dfrac{K_w}{pOH}$$

D
$$10^{-(14-pOH)}$$

Solution

$$pH = - \log [H^+]$$

or, $$[H^+] = 10^{-pH}$$

$$\because pH + pOH = 14$$

$$\therefore pH = 14 - pOH$$

Thus, $$[H^+] = 10^{-(14-pOH)}$$
Question 6
1 / -0

When $$NH_4Cl$$ is added to $$NH_4OH$$ solution, the dissociation of ammonium hydroxide is reduced. It is due to:

A
Common ion effect

B
Hydrolysis

C
Oxidation

D
Reduction

Solution

Due to common ion effect.

This effect is known as common ion effect.
Question 7
1 / -0

Pure $$NaCl$$ is prepared by saturating a cold saturated solution of common salt in water with $$HCl$$ gas. The principle used is

A
Le Chatelier principle

B
Displacement law

C
Common ion effect

D
Fractional distillation

Solution

Pure NaCl is prepared by saturating a cold saturated solution of common salt in water with HCl gas and is based on the $$\text{common ion effect.}$$
HCl is a strong electrolyte and provides an ion $$(Cl^-)$$ that is common to that provided by the weak electrolyte. Thus, the ionization of weak electrolytes is suppressed.
Question 8
1 / -0

Out of the following which pair of solutions is not a buffer solution?

A
$$NH_{4}Cl+NH_{4}OH$$

B
$$NaCl+NaOH$$

C
$$Na_{2}HPO_{4}+Na_{3}PO_{4}$$

D
$$CH_{3}COOH+CH_{3}COONa$$

Solution

Buffer solution is combination of weak acid and conjugate base. $$NaCl$$ is a salt and $$NaOH$$ is the base.
Question 9
1 / -0

$$K_{a1},K_{a2}$$ and $$K_{a3}$$ are the respective ionisation constants for the following reactions:
$$H_{2}S\leftrightharpoons H^{+}+HS^{-}$$
$$HS^{-}\leftrightharpoons H^{+}+S^{2-}$$
$$H_{2}S\leftrightharpoons 2H^{+}+S^{2-}$$
The correct relationship between $$K_{a1},K_{a2}$$ and $$K_{a3}$$ is,

A
$$K_{a3}=K_{a1}\times K_{a2}$$

B
$$K_{a3}=K_{a1}+K_{a2}$$

C
$$K_{a3}=K_{a1}-K_{a2}$$

D
$$K_{a3}=K_{a1}/K_{a2}$$

Solution

$$K_{a1}=\frac{[H^{+}][HS^{-}]}{[H_{2}S]}, K_{a2}=\frac{[H^{+}][S^{2-}]}{[HS^{-}]},K_{a3}=\frac{[H^{+}][S^{2-}]}{[H_{2}S]}$$,
For dibasic acid, $$K_{a3}=K_{a1}*K_{a2}$$
Question 10
1 / -0

What will be the ionisation constant of formic acid if its 0.01 M solution is 14.5% ionised?

A
$$2.1 \times 10^{-4}$$

B
14.5

C
0.145

D
$$1.45 \times 10^{-4}$$

Solution

$$K_a = c \alpha^{2}$$

$$\alpha = \dfrac{14.5} {100} = 0.145$$

$$K_a = 0.01 \times (0.145)^{2} = 2.1 \times 10^{-4}$$

Option A is correct.

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Equilibrium Test - 73

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Equilibrium Test - 73

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Question 1

$$2NO_2 (g) \rightleftharpoons 2NO (g) + O_2 (g)$$

$$4NH_3(g) + 5O_2(g) \rightleftharpoons 4NO (g) + 6H_2O (l)$$

$$3O_2 (g) \rightleftharpoons 2O_3 (g)$$

$$H_2(g) + I_2 (g) \rightleftharpoons 2HI (g)$$

Solution

Question 2

temperature and pressure

temperature only

pressure only

temperature, pressure and catalyst

Solution

Question 3

$$1\times 10^{-6}$$

$$1\times 10^{12}$$

$$1\times 10^{-12}$$

$$1\times 10^{6}$$

Solution

Question 4

$$HNO_3$$ and $$CH_3COOH$$

$$KOH$$ and $$CH_3COONa$$

$$HNO_3$$ and $$CH_3COONa$$

$$CH_3COOH$$ and $$CH_3COONa$$

Solution

Question 5

$$10^{-pOH}$$

$$14 - pOH$$

$$\dfrac{K_w}{pOH}$$

$$10^{-(14-pOH)}$$

Solution

Question 6

Common ion effect

Hydrolysis

Oxidation

Reduction

Solution

Question 7

Le Chatelier principle

Displacement law

Common ion effect

Fractional distillation

Solution

Question 8

$$NH_{4}Cl+NH_{4}OH$$

$$NaCl+NaOH$$

$$Na_{2}HPO_{4}+Na_{3}PO_{4}$$

$$CH_{3}COOH+CH_{3}COONa$$

Solution

Question 9

$$K_{a3}=K_{a1}\times K_{a2}$$

$$K_{a3}=K_{a1}+K_{a2}$$

$$K_{a3}=K_{a1}-K_{a2}$$

$$K_{a3}=K_{a1}/K_{a2}$$

Solution

Question 10

$$2.1 \times 10^{-4}$$

14.5

0.145

$$1.45 \times 10^{-4}$$

Solution

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