Equilibrium Test

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Equilibrium Test - 46

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Weekly Quiz Competition

Question 1
1 / -0

$$Ag_3 PO_4$$ would be least soluble at 25$$^o$$C in

A
0.1 M $$AgNO_3$$

B
0.1 M $$HNO_3$$

C
pure water

D
0.1 M $$Na_3PO_4$$

E
solubility in (a), (b), (c) or (d) is not different

Solution

$$Ag_3 PO_4$$ is a weak electrolyte and $$AgNO_3$$ is a strong electrolyte containing common ion $$(Ag^+ion)$$. Thus common ion effect is observed and the solubility of $$Ag_3 PO_4$$ is suppressed.
Hence, $$Ag_3 PO_4$$ is least soluble in 0.1M $$AgNO_3$$.
Question 2
1 / -0

Equilibrium constant for the given reaction is $$K = 10^{20}$$ at temperature $$300 K$$
$$A(s) + 2B (aq.) \rightleftharpoons 2C (s) + D(aq.)$$; $$K= 10^{20}$$
The equilibrium concentration of B starting with a mixture of $$1 mol/lit$$ of A and $$1/3 mol/lit$$ of B at $$300 K$$ is ________.

A
$$~ 4.71\times 10^{-11}$$

B
$$~ 2 \times 10^{-10}$$

C
$$~ 2 \times 10^{-11}$$

D
$$~ 10^{-10}$$

Solution

$$A(s) + 2B (aq) \rightleftharpoons 2C(s) + D(aq)$$

Initially 1 $$\dfrac{1}{3}$$ 0 0

At eq. $$1 - x$$ $$\dfrac{1}{3} -x$$ $$2x$$ $$x$$
$$\dfrac{2}{3}$$ $$\approx a$$ $$\dfrac{2}{3}$$ $$\dfrac{1}{3}$$

Since, $$x \approx \dfrac{1}{3}$$ ( As $$B$$ gets nearly completely consumed)

Now,
$$K_c=\dfrac{[C]^2[D]}{[A][B]^2}$$

$$\displaystyle 10^{20}= \dfrac{\dfrac{2^2\times1}{3^2\times3}}{\dfrac{2}{3}\times[B]^2}$$ $$\Rightarrow$$ $$10^{20} = \dfrac{\dfrac{2}{9}}{a^2}$$ $$\Rightarrow$$ $$a^2 = \displaystyle \dfrac{2}{9 \times 10^{20}} = \dfrac{2\times 10^{-20}}{9} $$

$$\therefore a= 4.71 \times 10^{-11}$$

Hence, the correct option is $$(A)$$
Question 3
1 / -0

The value of K for a reaction can be changed by changing :

A
temperature

B
pressure

C
volume

D
all of the above

Solution

The value of equilibrium constant can be altered by varying the temperature.

The variation of K with temperature is given by van't Hoff equation.
Hence option A is correct.
Question 4
1 / -0

The degree of dissociation of $$PCl_{5}(g)\rightleftharpoons PCl_{3}(g)+Cl_{2}(g)$$, ___________ with increase in pressure at equilibrium.

A
increases

B
decreases

C
first increases and then decreases

D
first decreases and then increases

Solution

With an increase in the pressure, the equilibrium will shift in the direction in which there is decrease in the number of moles so as to nullify the effect of increased pressure. The number of moles of the reactant is less than the total number of moles of the product. Hence, the equilibrium will shift in the backward direction. This will suppress the dissociation.
Question 5
1 / -0

Assertion(A): In the dissociation of $$PCl_{5}$$ at constant pressure and temperature addition of helium at equilibrum increases the dissociation of $$PCl_{5}$$.
Reason(R): Helium removes $$Cl_{2}$$ from the field of action.

A
Both Assertion and Reason are true and Reason is correct explanation of Assertion.

B
Both Assertion and Reason are true but Reason is not correct explanation of Assertion.

C
Assertion is true but Reason is false.

D
Both Assertion and Reason are false.

Solution

When inert gas such as helium is added at constant pressure, the equilibrium will shift in the direction in which there is increase in the number of moles of gases. Thus the equilibrium for the dissociation of $$PCl_5$$ will shift to right as the number of moles increases from 1 to 2.
Question 6
1 / -0

Ammonia is a weak base that reacts with water according to the equation $$NH_{3}(aq)+H_{2}O(l)\rightleftharpoons NH_{4}^{+}+OH^{-}(aq)$$. Will any of the following increase the percent of ammonia that is converted to the ammonium ion in water?

A
Addition of $$NaOH$$.

B
Addition of $$HCl$$.

C
Addition of $$NH_{4}Cl$$.

D
None of the above.

Solution

Whn HCl is added, the hydrogen ions will neutralize hydroxide ions to form water. The equilibrium will shift in the forward direction so that more hydroxide ions are obtained. This will increase the percentage of ammonia that is converted to ammonium ions in water.
Question 7
1 / -0

Introduction of inert gas at constant volume to a gaseous reaction at equilibrium, results in formation of :

A
same amount of product

B
more quantity of product

C
less quantity of product

D
no product

Solution

When an inert gas is added to the equilibrium gaseous mixture at constant volume, the total number of moles of the reaction mixture are unaffected. Hence, there is no impact on the value of the equilibrium constant. Hence, the concentration of products is not affected.
Question 8
1 / -0

$$N_{2}+O_{2}$$$$\rightleftharpoons$$ $$2NO-Heat$$

The forward reaction would be favoured by:

A
high temperature

B
low temperature

C
high and low temperature

D
constant temperature

Solution

The reaction is endothermic. Heat is absorbed during the reaction. When the temperature is raised, the forward reaction will be favoured so that the absorbed heat will nullify the effect of increased heat. So, the forward reaction will be favoured by high temperature.

Hence, the correct option is $$A$$
Question 9
1 / -0

Given that $$K_w$$ for water is $$10^{-13}M^2$$ at $$2^oC$$, compute the sum of $$p{OH}$$ and $$p{H}$$ for a neutral aqueous solution at $$2^oC$$?

A
$$7.0$$

B
$$13.30$$

C
$$14.0$$

D
$$13.0$$

Solution

As we know,
$$K_w = [H^+][OH^-];\quad pH+pOH = -logK_w = 13$$.
Question 10
1 / -0

Which of the following is a buffer solution?

A
$$500\space mL$$ of $$0.1\space N\space CH_3COOH + 500\space mL$$ of $$0.1\space N\space NaOH$$

B
$$500\space mL$$ of $$0.1\space N\space CH_3COOH + 500\space mL$$ of $$0.1\space N\space HCl$$

C
$$500\space mL$$ of $$0.1\space N\space CH_3COOH + 500\space mL$$ of $$0.2\space N\space NaOH$$

D
$$500\space mL$$ of $$0.2\space N\space CH_3COOH + 500\space mL$$ of $$0.1\space N\space NaOH$$

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Equilibrium Test - 46

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Equilibrium Test - 46

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Question 1

0.1 M $$AgNO_3$$

0.1 M $$HNO_3$$

pure water

0.1 M $$Na_3PO_4$$

solubility in (a), (b), (c) or (d) is not different

Solution

Question 2

$$~ 4.71\times 10^{-11}$$

$$~ 2 \times 10^{-10}$$

$$~ 2 \times 10^{-11}$$

$$~ 10^{-10}$$

Solution

Question 3

temperature

pressure

volume

all of the above

Solution

Question 4

increases

decreases

first increases and then decreases

first decreases and then increases

Solution

Question 5

Both Assertion and Reason are true and Reason is correct explanation of Assertion.

Both Assertion and Reason are true but Reason is not correct explanation of Assertion.

Assertion is true but Reason is false.

Both Assertion and Reason are false.

Solution

Question 6

Addition of $$NaOH$$.

Addition of $$HCl$$.

Addition of $$NH_{4}Cl$$.

None of the above.

Solution

Question 7

same amount of product

more quantity of product

less quantity of product

no product

Solution

Question 8

high temperature

low temperature

high and low temperature

constant temperature

Solution

Question 9

$$7.0$$

$$13.30$$

$$14.0$$

$$13.0$$

Solution

Question 10

$$500\space mL$$ of $$0.1\space N\space CH_3COOH + 500\space mL$$ of $$0.1\space N\space NaOH$$

$$500\space mL$$ of $$0.1\space N\space CH_3COOH + 500\space mL$$ of $$0.1\space N\space HCl$$

$$500\space mL$$ of $$0.1\space N\space CH_3COOH + 500\space mL$$ of $$0.2\space N\space NaOH$$

$$500\space mL$$ of $$0.2\space N\space CH_3COOH + 500\space mL$$ of $$0.1\space N\space NaOH$$

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