Equilibrium Test

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Equilibrium Test - 51

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Weekly Quiz Competition

Question 1
1 / -0

How can be equilibrium concentration of $$Ag^+$$ can be reduced in a solution of $$Na^+, Cl^+, Ag^+$$ and $$NO_3$$, in contact with solid $$AgCl$$. $$Na^+ (aq) + Cl (aq) + Ag^+ (aq) + NO_3(aq)\rightleftharpoons AgCl (s) + Na^+ (aq) + NO_3 (aq) \Delta H = 65.9 kJ$$ ?

A
Add $$NaCl$$ in the solution.

B
Some other salt that produces $$Cl^+$$ in the solution.

C
Cool the solution

D
All of the above

Solution

$$Na^+ (aq) + Cl^ (aq) + Ag^+ (aq) + NO_3^ (aq)\rightleftharpoons AgCl (s) + Na^+ (aq) + NO_3^ (aq) \Delta H = 65.9 kJ$$
As we know,
To increase product, we have to add reactant (or common ion) so by adding $$Cl^+$$ $$(NaCl)$$ product increases.
Also as this is an exothermic reaction so it will be favoured by losing heat.
Question 2
1 / -0

Consider the equilibria:

1. $$\displaystyle Hb(aq)+4O_{2}(g)\rightleftharpoons Hb(O_{2})_{4}(aq);\ \ \ K_{c_{1}}$$
2. $$\displaystyle Hb(aq)+4CO(g)\rightleftharpoons Hb(CO)_{4}(aq);\ \ \ K_{c_{2}}$$

(Hb) = Haemoglobin in Blood)

Identify the correct statement.

A
at higher altitudes, equilibria 1 shifts towards right

B
carbon monoxide poisoning makes the face of affected person look plate

C
$$\displaystyle K_{C_{1}}> K_{C_{2}}$$

D
people living on hills have more haemoglobin in their body than people living on plains

Solution

As one climbs higher away from the mean sea level, the atmospheric concentration decreases, and therefore the amount of oxygen available proportionately decreases. In an effort to take in as much oxygen is available to us, the human body increases the number of RBCs in the system, which also would reflect in a higher haemoglobin count for such people.

Hence, people living on hills have more haemoglobin in their body than people living on plains.

So, option D is correct.
Question 3
1 / -0

For the equilibrium reaction, $${H}_{2}O(l)\rightleftharpoons {H}_{2}O(g)$$, what happens, if pressure is increased.

A
More water evaporates.

B
Equilibrium shift in backward direction.

C
No effect on equilibrium.

D
None of the above

Solution

For the equilibrium reaction, $${H}_{2}O(l)\rightleftharpoons {H}_{2}O(g)$$, if pressure is increased, equilibrium shift in backward direction. The reaction is accompanied by increase in the number of moles of gaseous species from 0 to 1. Hence, the increase in pressure will try to decrease the number of moles by shifting the equilibrium in backward direction.
Question 4
1 / -0

At $${60}^{o}C$$, pure water has $$[{H}_{3}{O}^{+}]={10}^{-6.7}mol/lit$$.What is the value of $${K}_{W}$$ at $${60}^{o}C$$ :-

A
$${10}^{-6}$$

B
$${10}^{-12}$$

C
$${10}^{-67}$$

D
$${10}^{-13.4}$$

Solution

In pure water, $$[H_3O^{+}]= [OH^{-}]$$

$$K_w = [H_3O^+][OH^-]$$

As given, $$[{H}_{3}{O}^{+}]={10}^{-6.7}mol/lit$$

So, $$K_w = {10}^{-6.7}\times{10}^{-6.7} = {10}^{-13.4}$$
Question 5
1 / -0

A buffer solution can be prepared from a mixture of:

(i) Sodium acetate and acetic acid in water
(ii) Sodium acetate and hydrochloric acid in water
(iii) Ammonia and ammonium chloride in water
(iv) Ammonia and sodium hydroxide in water

A
(i), (ii)

B
(ii), (iii)

C
(iii), (iv)

D
(i), (iii)

Solution

An acidic buffer solution consists of a weak acid (such as acetic acid) and its salt (such as sodium acetate) with a strong base (such as $$NaOH$$).

A buffer solution can be prepared from a mixture of:
(i) Sodium acetate and acetic acid in water
(ii) Sodium acetate and hydrochloric acid in water

Hydrochloric acid will partly neutralize sodium acetate to form acetic acid.
Hence, the option $$A$$ is the correct answer.
Question 6
1 / -0

Which one of the following statements is not correct?

A
The pH of $$1.0 \times {10}^{-8} M\ HCl$$ is less than $$7$$

B
The ionic product of water at $$25^0C$$ is $$1.0 \times {10}^{-14}\ {mol}^{2} {L}^{-2}$$

C
$${Cl}^{-}$$ is a Lewis acid

D
Bronsted-Lowry theory cannot explain the acidic character of $$Al{Cl}_{3}$$

Solution

$$Cl^-$$ is not a Lewis acid. It is a Lewis base. Lewis acid is a chemical species that reacts with a Lewis base to form a Lewis adduct. A Lewis base, then, is any species that donates a pair of electrons to a Lewis acid to form a Lewis adduct.

For example, $$OH^−$$ and $$NH_3$$ are Lewis bases, because they can donate a lone pair of electrons.
Question 7
1 / -0

On increasing temperature, the equilibrium constant of exothermic and endothermic reactions __________ and ________ respectively:

A
increases and decreases

B
decreases and increases

C
increases and increases

D
decreases and decreases

Solution

Exothermic Reactions
If $$K_c$$ decreases with an increase in temperature, the reaction shifts to the left.
If $$K_c$$ increases with a decreases in temperature, the reaction to shifts to the right.
Endothermic Reactions
If $$K_c$$ increases with an increase in temperature, the reaction to shifts to the right.
If $$K_c$$ decreases with a decrease in temperature, the reaction to shifts to the left.
Question 8
1 / -0

The gaseous reaction $$A+B \rightleftharpoons 2C+D+Q$$ is most favoured at :

A
low temperature and high pressure

B
high temperature and high pressure

C
high temperature and low pressure

D
low temperature and low pressure

Solution

The gaseous reaction $$\displaystyle A+B \rightleftharpoons 2C+D+Q $$ is most favoured at low temperature and low pressure.

Since heat Q is on the products side, the reaction is exothermic in nature.

At low temperature, the equilibrium shifts to products so that more heat is produced which nullifies the effect of low temperature.

The difference between the number of moles of gaseous products and the number of moles of gaseous reactants $$\displaystyle \Delta n = 2 + 1 - 1 + 1 = 1 > 0 $$

At low pressure, the reaction will shift in forward direction so that more and more products are produced which increases the total number of moles and total pressure. This nullifies the effect of low pressure.

Hence the correct option is D.
Question 9
1 / -0

Which one of the following is not a buffer solution?

A
$$0.8M\ {H}_{2}S+0.8MKHS$$

B
$$2\ M\ {C}_{6}{H}_{5}{NH}_{2}+2M\ {C}_{6}{H}_{5}\overset { + }{ N } {H}_{3}{Br}$$

C
$$3\ M\ {H}_{2}{CO}_{3}+3M\ KH{CO}_{3}$$

D
$$0.05\ M\ KCl{O}_{4}+0.05M\ HCl{O}_{4}$$

Solution

A solution that resists change in pH value upon addition of small amount of strong acid or base (less than 1 %) or when solution is diluted is called buffer solution.

Basic buffer solution : A basic buffer solution consists of a mixture of a weak base and its salt with strong acid. The best known example is a mixture of $$NH_4OH$$ and $$NH_4 Cl.$$

Acidic buffer solution : An acidic buffer solution consists of solution of a weak acid and its salt with strong base. The best known example is a mixture of solution of acetic acid and its salt with strong base.($$CH_3COONa)$$

So D is not a buffer solution.
Question 10
1 / -0

If pressure increases then its effect on given equilibrium
$$C(s) + H_2O(g) \rightleftharpoons CO(g) + H_2 (g)$$
It is shifted in:

A
forward direction

B
backward direction

C
no effect

D
none of these

Solution

$$C_{(s)} + H_2O_{(g)} \rightleftharpoons CO_{(g)} + H_{2(g)}$$
According to Le-Chatelier's principle, the reactions in which number of moles of gaseous reactions are less than number of gaseous moles of products, such reactions are favored at low pressure.
$$\therefore$$ The equilibrium will shift in backward direction at high pressure.

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Equilibrium Test - 51

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Equilibrium Test - 51

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Question 1

Add $$NaCl$$ in the solution.

Some other salt that produces $$Cl^+$$ in the solution.

Cool the solution

All of the above

Solution

Question 2

at higher altitudes, equilibria 1 shifts towards right

carbon monoxide poisoning makes the face of affected person look plate

$$\displaystyle K_{C_{1}}> K_{C_{2}}$$

people living on hills have more haemoglobin in their body than people living on plains

Solution

Question 3

More water evaporates.

Equilibrium shift in backward direction.

No effect on equilibrium.

None of the above

Solution

Question 4

$${10}^{-6}$$

$${10}^{-12}$$

$${10}^{-67}$$

$${10}^{-13.4}$$

Solution

Question 5

(i), (ii)

(ii), (iii)

(iii), (iv)

(i), (iii)

Solution

Question 6

The pH of $$1.0 \times {10}^{-8} M\ HCl$$ is less than $$7$$

The ionic product of water at $$25^0C$$ is $$1.0 \times {10}^{-14}\ {mol}^{2} {L}^{-2}$$

$${Cl}^{-}$$ is a Lewis acid

Bronsted-Lowry theory cannot explain the acidic character of $$Al{Cl}_{3}$$

Solution

Question 7

increases and decreases

decreases and increases

increases and increases

decreases and decreases

Solution

Question 8

low temperature and high pressure

high temperature and high pressure

high temperature and low pressure

low temperature and low pressure

Solution

Question 9

$$0.8M\ {H}_{2}S+0.8MKHS$$

$$2\ M\ {C}_{6}{H}_{5}{NH}_{2}+2M\ {C}_{6}{H}_{5}\overset { + }{ N } {H}_{3}{Br}$$

$$3\ M\ {H}_{2}{CO}_{3}+3M\ KH{CO}_{3}$$

$$0.05\ M\ KCl{O}_{4}+0.05M\ HCl{O}_{4}$$

Solution

Question 10

forward direction

backward direction

no effect

none of these

Solution

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