Equilibrium Test

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Equilibrium Test - 24

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Question 1
1 / -0

$$N_2 + 3H_2\rightleftharpoons 2NH_3$$ If temperature of following equilibrium reaction increase then -

A
Shift Right side

B
Shift left side

C
Unchanged

D
Nothing say.

Solution

As reaction is exothermic so an increasing temperature shifts to backward.
Question 2
1 / -0

The degree of dissociation of $$PCI_5(g)\rightleftharpoons PCI_3(g)+CI_2(g)$$ , decreases with increase in ______ at equilibrium?

A
temperature

B
volume

C
pressure

D
concentration

Solution

The degree of dissociation of $${\left [ PCl_5(g)\rightleftharpoons PCl_3(g)+Cl_2(g)\right ]}$$ , decreases with increase in pressure at equilibrium. When pressure is increased, the equilibrium will shift in the backward direction. This decreases the degree of dissociation.

Note: The number of moles of gaseous reactants are lower than the number of moles of gaseous products. When pressure is increased, the equilibrium will shift in the reverse direction so that there is decrease in the number of moles of gaseous species. This decreases the pressure and nullifies the effect of increase in the pressure. It is in accordance with Le Chatelier's principle.
Question 3
1 / -0

In a equilibrium reaction $$H_2(g) + I_2(g)\rightleftharpoons 2HI(g)$$
$$\Delta H =-3000 \:calories$$, which factor favours dissociation of HI :-

A
Low temp.

B
High Pressure

C
High temp.

D
Low pressure.

Solution

In a equilibrium reaction $$H_2(g) + I_2(g)\rightleftharpoons 2HI(g)$$
$$\Delta H =-3000 \:calories$$, High temp. favours dissociation of $$HI$$ . negative value of the enthalpy change indicates that the reverse reaction (dissociation of $$HI$$) is endothermic in nature.
At high temperature, the equilibrium will shift in the reverse direction so that more and more heat is absorbed during the reaction which nullifies the effect of high temperature.
Question 4
1 / -0

Determine $$[{OH}^{-}]$$ of a $$0.050\ M$$ solution of ammonia to which has been added sufficient $${NH}_{4}Cl$$ to make the total $$[{NH}_{4}^{+}]$$ equal to $$0.100 M$$. $$[{K}_{b({NH}_{3})}=1.8\times {10}^{-5}]$$

A
$$[{OH}^{-}]=9.0\times {10}^{-6}$$

B
$$[{OH}^{-}]=9.0\times {10}^{-8}$$

C
$$[{OH}^{-}]=9.0\times {10}^{-2}$$

D
$$[{OH}^{-}]=9.0\times {10}^{-9}$$

Solution

$${NH}_{4}Cl\longrightarrow {NH}_{4}^{+}+{Cl}^{-}$$
$${NH}_{4}OH\longrightarrow {NH}_{4}^{+}+{OH}^{-}$$
$${K}_{b}=\cfrac { \left[ { NH }_{ 4 }^{ + } \right] \left[ OH \right] }{ \left[ { NH }_{ 4 }OH \right] } $$
$$[{NH}_{4}^{+}]=$$ is due to salt because $${NH}_{4}OH$$ ionise less amount due to common ions effect
$$1.8\times {10}^{-5}=\cfrac{0.1\times [{OH}^{-}]}{0.05}$$
$$9\times {10}^{-6}=[{OH}^{-}]$$
Question 5
1 / -0

The ionic product of water ______ if a few drops of acid or base are added to it.

A
increases

B
decreases

C
remains the same

D
can not predict

Solution

The ionic product of water at a particular temperature is constant and has no effect of acid or base addition.
Question 6
1 / -0

In the presence of a common ion (incapable of forming complex ion), the solubility of salt _______ in solution.

A
increases

B
decreases

C
remains the same

D
cannot predict

Solution

$$AB \rightarrow A^+ + B^-$$
$$BC \rightarrow B^+ + C^-$$
Since $$B^+$$ is incapable of forming a complex salt it tends to decrease the solubility by Le-Chatelier's principle.
Question 7
1 / -0

Assertion: A solution of sodium acetate and ammonium acetate can act as a buffer.
Reason: A buffer solution consists of a mixture of a weak acid and its conjugate base or vice versa.

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

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

C
Assertion is true but Reason is false

D
Assertion is false but Reason is true

E
Both Assertion and Reason are false

Solution

A buffer is a solution that can resist pH change upon the addition of an acidic or basic components. It is able to neutralize small amounts of added acid or base, thus maintaining the pH of the solution relatively stable. A buffer must consist of a weak conjugate acid-base pair, meaning either a. a weak acid and its conjugate base, or b. a weak base and its conjugate acid. For example, the following could function as buffers when together in solution:
Acetic acid (weak organic acid w/ formula $$CH_3COOH$$) and a salt containing its conjugate base, the acetate anion ($$CH_3COO^-$$), such as sodium acetate ($$CH_3COONa$$)
Question 8
1 / -0

Assertion: A buffer has a definite pH value which changes, on keeping it or on diluting it.
Reason: A buffer solution is a mixture consisting of a weak acid and its conjugate base or vice versa.

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

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

C
Assertion is true but Reason is false

D
Assertion is false but Reason is true

Solution

A buffer solution is an aqueous solution consisting of a mixture of a weak acid and its conjugate base, or vice versa. Its pH changes very little when a small or moderate amount of strong acid or base is added to it and thus it is used to prevent changes in the pH of a solution. Buffer solutions are used as a means of keeping pH at a nearly constant value in a wide variety of chemical applications. Many life forms thrive only in a relatively small pH range so they utilize a buffer solution to maintain a constant pH. One example of a buffer solution found in nature is blood.
Question 9
1 / -0

Assertion: The buffer HCOOH/HCOONa will have pH lesser than 7.
Reason: Conjugate base of a weak acid is a strong base.

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

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

C
Assertion is true but Reason is false

D
Assertion is false but Reason is true

E
Both Assertion and Reason are false

Solution

The buffer HCOOH/HCOONa is an acidic buffer solution containing weak acid formic acid and its salt sodium formate with strong base NaOH.
It will have pH less than 7 as the solution will be acidic.
Question 10
1 / -0

Assertion: AgCl is less soluble in aqueous sodium chloride solution than in pure water.
Reason: AgCl dissociates completely and more rapidly than NaCl.

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

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

C
Assertion is true but Reason is false

D
Assertion is false but Reason is true

E
Both Assertion and Reason are false

Solution

$$AgCl \rightleftharpoons Ag^+ + Cl^-$$
$$NaCl \rightarrow Na^+ + Cl^-$$
Sodium chloride is a strong electrolyte and is completely dissociated. This increases the chloride ion concentration in solution and suppresses the ionization of $$AgCl$$. Hence, the solubility of $$AgCl$$ decreases.

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Equilibrium Test - 24

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Equilibrium Test - 24

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SHARING IS CARING

Question 1

Shift Right side

Shift left side

Unchanged

Nothing say.

Solution

Question 2

temperature

volume

pressure

concentration

Solution

Question 3

Low temp.

High Pressure

High temp.

Low pressure.

Solution

Question 4

$$[{OH}^{-}]=9.0\times {10}^{-6}$$

$$[{OH}^{-}]=9.0\times {10}^{-8}$$

$$[{OH}^{-}]=9.0\times {10}^{-2}$$

$$[{OH}^{-}]=9.0\times {10}^{-9}$$

Solution

Question 5

increases

decreases

remains the same

can not predict

Solution

Question 6

increases

decreases

remains the same

cannot predict

Solution

Question 7

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

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

Assertion is true but Reason is false

Assertion is false but Reason is true

Both Assertion and Reason are false

Solution

Question 8

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

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

Assertion is true but Reason is false

Assertion is false but Reason is true

Solution

Question 9

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

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

Assertion is true but Reason is false

Assertion is false but Reason is true

Both Assertion and Reason are false

Solution

Question 10

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

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

Assertion is true but Reason is false

Assertion is false but Reason is true

Both Assertion and Reason are false

Solution

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