Chemistry Chapter 7 Mock Test

Question 1 of 45

15 moles of H₂ and 5.2 moles of l₂ are mixed and allowed to attain equilibrium at 500°c The concentration of HI is found to be 10 moles at equilibrium. Find the equilibrium constant for the formation of HI.

15
25
50
100

Question 2 of 45

Statement 1: Unit of \(K_{c} =L^{2} mol^{-2}\) for the reaction \(N_{2}(g)+3H_{2}(g) \leftrightharpoons 2NH_{3}(g)\).

Statement 2: Equilibrium constant \(K_{c} = \frac{[NH_{3}^{2}]}{[N_{2}][H_{2}]^{3}}\) for the reaction \(N_{2}(g) + 3H_{2}(g) \leftrightharpoons 2NH_{3}(g).\)

Both Statement 1 and Statement 2 are true but Statement 2 is not the correct explanation of Statement 1
Both Statement 1 and Statement 2 are true and the Statement 2 is correct explanation of the Statement 1
This Statement 1 is true, but the Statement 2 is false
Both Statement 1 and Statement 2 are false

Question 3 of 45

The value of K_pwill be equal to K_cin which of the following equation?

\(2SO_{2}+O_{2} \leftrightharpoons 2SO_{3}\)
\(2NH_{3} \leftrightharpoons N_{2}+3H_{2}\)
\(PCl_{5} \leftrightharpoons PCl_{3}+Cl_{2}\)
\(H_{2}+l_{2} \leftrightharpoons 2HI\)

Question 4 of 45

Find the equilibrium constant for the following gaseous reaction \(H_{2}+I_{2} \leftrightharpoons 2HI.\)

\(K_{p}=1/K_{c}\)
\(K_{p}=K_{c}\)
\(K_{p} \textless K_{c}\)
\(K_{p}>K_{c}\)

Question 5 of 45

2 moles of PCl₅ were heated in a closed vessel of 2 litre capacity. At equilibrium, 40% of PCl₅ is dissociated into PCl₃ and Cl₂. What is the value of equilibrium constant?

5.3
2.66
0.53
0.266

Question 6 of 45

Statement 1 : Colour of the mixture turns to pink from deep blue for a reaction, \(Co(H_{2}O)_{6(aq)}^{2+}+4Cl_{(aq)}^{-} \leftrightharpoons CoCl_{4(aq)}^{2-}+6H_{2}O_{(l)}\)after cooling a freezing mixture.

Statement 2 : Reaction is endothermic so on cooling, the reaction moves to backward direction.

Both statement 1 and statement 2 are true and the statement 2 is the correct explanation of the statement 1
Both statement 1 and statement 2 are true but statement 2 is not the correct explanation of the statement 1
Statement 1 is true but statement 2 is false
The statement 1 and statement 2 both are false

Question 7 of 45

What is the correct explanation of the effect of catalyst on the velocity in a reversible reaction?

It decreases the velocity of backward reaction
It provides a new reaction path of low activation energy
It increases the kinetic energy of reacting molecules
It displaces the equilibrium state on right side

Question 8 of 45

What does the K becomes if concentration of reactants is increased by ‘x’?

K
K+X
K/X
In (K/X)

Question 9 of 45

Equilibrium is attained by the reaction when the free energy change accompanying it is

negative and small
negative and large
zero
positive and large

Question 10 of 45

HI was heated in a closed tube at 440°c till equilibrium is obtained. At this temperature 22% of HI was dissociated. What will be the equilibrium constant for this dissociation?

0.0199
0.0796
0.282
1.99

Question 11 of 45

Reactant ‘A’ decomposes 10% in 1 hour, 20% in 2 hour and 30% in 3 hour in a reaction. What is the unit of rate constant of this reaction?

\( litre^{2}mol^{-2} s^{-1}\)
\( litre mol^{-1} s^{-1}\)
[mathjax] [latex] mol litre^{-1} s^{-1}[/latex]
\(s^{-1}\)

Question 12 of 45

For which of the following reactions K_p is greater than K_c?

\(2SO_3 \leftrightharpoons O_2+2SO_2 \)
\(PCl_3+Cl_2\leftrightharpoons PCl_5\)
\( H_2+l_2 \leftrightharpoons 2HI\)
\( N_2+3H_2 \leftrightharpoons 2NH_3\)

Question 13 of 45

K_p is less than K_c in which of the following equilibria?

\(N_2+O_2 \leftrightharpoons 2NO\)
\(2SO_2+O_2 \leftrightharpoons 2SO_3\)
\( 2HI \leftrightharpoons H_2+I_2 \)
\( N_2 O_4 \leftrightharpoons 2NO_2\)

Question 14 of 45

\( \Delta \) G°(HI,g) = + 1.7 kJ. The equilibrium constant at 25°C for 2Hl(g)\( \leftrightharpoons \) H₂(g) + l₂(g) is

24.0
3.9
2.0
0.5

Question 15 of 45

56 g of nitrogen and 8 g hydrogen gas are heated in a closed vessel. At equilibrium 34 g of ammonia are present. What are the equilibrium no. of moles of nitrogen, hydrogen and ammonia respectively?

2, 1, 2
1,1,2
2, 2, 1
1,2,2

Question 16 of 45

In which of the following reaction, yield of product will increase with increase in pressure?

\(CO_{(g)} + 3H_{2(g)} \leftrightharpoons CH_{4(g)} + H_{2}O_{(g)}\)
\(H_{2}O_{(g)} + C_{(s)} \leftrightharpoons CO_{(g)} + H_{2(g)}\)
\(H_{2}O_{(g)} + CO_{(g)} \leftrightharpoons CO_{2(g)} + H_{2(g)}\)
\(H_{2(g)}+l_{2(g)} \leftrightharpoons 2HI_{(g)}\)

Question 17 of 45

If for \(H_{2(g)} + \frac{1}{2}S_{2(s)} \leftrightharpoons H_{2}S_{(g)} and H_{2(g)} + Br_{2(g)} \leftrightharpoons 2HBr_{(g)}.\)The reaction\(Br_{2(g)} + H_{2}S_{(g)} \leftrightharpoons 2HBr_{(g)}+ \frac{1}{2}S_{2(s)}\) would have equilibrium constant ________ where \(K_{1} and K_{2}\) are the equilibrium constants respectively.

\(K_{2}^{2} / K_{1}\)
\(K_{2} / K_{1}\)
\(K_{1} / K_{2}\)
\(K_{1} \times K_{1}\)

Question 18 of 45

For reaction \(PCl_{5}(g) \leftrightharpoons PCl_{3}(g) + Cl_{2}(g),\)

\(K_{p}=K_{c}(RT)^{2}\)
\(K_{p}=K_{c}(RT)\)
\(K_{p}=K_{c}(RT)^{-1}\)
\(K_{p}=K_{c}\)

Question 19 of 45

5 moles of SO₂ and 5 moles of O₂ are allowed to react to form SO₃ in a closed vessel. At the equilibrium stage 60% of SO₂ is used up. Find the total number of moles of SO₂, O₂ and SO₃ in the vessel now.

3.9
8.5
10.0
10.5

Question 20 of 45

Statement 1: Catalyst affects the final state of the Equlibrium.

Statement 2: It enables the system to attain a new equilibrium state by complexing with the reagents.

Both Statement 1 and Statement 2 are true but Statement 2 is not the correct explanation of Statement 1
Both Statement 1 and Statement 2 are true and the Statement 2 is correct explanation of the Statement 1
Both Statement 1 and Statement 2 are false
This Statement 1 is false but the Statement 2 is true

Question 21 of 45

The formation of HX will be favoured by _____ in the gaseous equilibrium \(H_{2} X_{2}+heat \leftrightharpoons 2HX\)

high temperature and low pressure
high pressure and low temperature
low temperature and low pressure
high temperature and high pressure

Question 22 of 45

In Haber process 30 litres of dihydrogen and 30 litres of dinitrogen were taken for reaction which yielded only 50% of the expected product. The composition of gaseous mixture under the aforesaid condition in the end will be:

20 litres ammonia, 10 litres nitrogen, 30 litres hydrogen
10 litres ammonia, 25 litres nitrogen, 15 litres hydrogen
20 litres ammonia, 20 litres nitrogen, 20 litres hydrogen
20 litres ammonia, 25 litres nitrogen, 15 litres hydrogen

Question 23 of 45

The information that can be obtained on the basis of Le-chatelier’s principle is:

Question 24 of 45

Increasing the temperature of an equilibrium system

favours the endothermic reaction only
favours the exothermic reaction only
favours both the exothermic and endothermic reactions
favours neither the exothermic nor endothermic reactions

Question 25 of 45

Value of K_c will be equal to which of the following for reaction, \(2A(g) \leftrightharpoons 3C(g) + D(s)\)?

\(K_{p}/RT\)
\(K_{p}(RT)\)
\(=K_{p}\)
None of these

Question 26 of 45

One mole of \(SO_{3}\) was placed in a litre reaction vessel at a certain temperature. The following equilibrium was established \(2SO_{3} \leftrightharpoons 2SO_{2}+O_{2}\). At equilibrium 0.6 moles of \(SO_{2}\) were formed. What will be the equilibrium constant of the reaction?

0.675
0.54
0.35
0.36

Question 27 of 45

What is the equilibrium constant K for the system \( 2A(g) + B(g) \leftrightharpoons 3C(g)?\)

\( \frac {[C]^{3}} {[A]^{2}\times[B]} \)
\( \frac {[3C]}{[2A]\times[B]}\)
\( \frac {[A]^{2}\times[B]} {[C]^{3}} \)
\( \frac {[2A]\times[B]}{[3C]} \)

Question 28 of 45

Statement 1: Addition of a small amount of sodium acetate to a dilute solution of acetic acid does not affect the pH value.

Statement 2: Buffer solutions have a definite pH value.

Both Statement 1 and Statement 2 are true but Statement 2 is not the correct explanation of Statement 1
Both Statement 1 and Statement 2 are true and the Statement 2 is correct explanation of the Statement 1
This Statement 1 is true, but the Statement 2 is false
This Statement 1 is false but the Statement 2 is true

Question 29 of 45

Statement 1: The pH of 10 M HCI aqueous solution is less than 1.

Statement 2: The pH is -ve logarithm of H⁺ concentration.

Both Statement 1 and Statement 2 are true but Statement 2 is not the correct explanation of Statement 1
Both Statement 1 and Statement 2 are true and the Statement 2 is correct explanation of the Statement 1
This Statement 1 is true, but the Statement 2 is false
Both Statement 1 and Statement 2 are false

Question 30 of 45

Statement 1 : For the reverse reaction, equilibrium constant is the inverse of the equilibrium constant for the reaction in the forward direction.

Statement 2 : Equilibrium constant depends upon the way in which the reaction is written.

Both statement 1 and statement 2 are true and the statement 2 is the correct explanation of the statement 1
Both statement 1 and statement 2 are true but statement 2 is not the correct explanation of the statement 1
Statement 1 is true but statement 2 is false
The statement 1 and statement 2 both are false

Question 31 of 45

The equilibrium constant changes with _____ for the reaction\(H_2(g)+ l_2(g) \leftrightharpoons 2HI(g) \)

temperature
the amounts of \( H_2 and l_2\) taken
catalyst
total pressure

Question 32 of 45

For the reaction \(C(s) + CO_{2}(g) \leftrightharpoons 2CO(g)\), the partial pressure of \(CO_{2}\) and CO are 2.0 and 4.0 atm respectively at equilibrium. What is the \(K_{p}\) for the reaction?

32.0
8.0
4.0
0.5

Question 33 of 45

Under conditions of constant _________ \(\Delta G = 0\) for a system in equilibrium.

pressure and volume
energy and volume
temperature and volume
temperature and pressure

Question 34 of 45

Statement 1 : Effect of temperature of K_c or K_p depends on enthalpy

Statement 2 : Increase in temperature shifts the equilibrium in exothermic direction while decrease in the temperature shifts the equilibrium position in endothermic direction.

Both statement 1 and statement 2 are true and the statement 2 is the correct explanation of the statement 1
Both statement 1 and statement 2 are true but statement 2 is not the correct explanation of the statement 1
Statement 1 is true but statement 2 is false
The statement 1 and statement 2 both are false

Question 35 of 45

The equilibrium reactions in which the equilibrium would shift to the right if total pressure is increased is:

\(N_{2}O_{4} \leftrightharpoons 2NO\)
\(H_{2}+Cl_{2} \leftrightharpoons 2HCl\)
\(H_{2} + I_{2} \leftrightharpoons 2HI\)
\(N_{2} + 3H_{2} \leftrightharpoons 2NH_{3}\)

Question 36 of 45

The standard state Gibbs free energy change for the given isomerization reaction \(cis-2-pentene \leftrightharpoons trans -2 -pentene\) is -3.67 kJ/mol at 400 K. What happens if more trans-2-pentene is added to the reaction vessel?

Additional trans-2-pentene is formed
Equilibrium remains unaffected
Equilibrium is shifted in the forward direction
More cis -2-pentene is formed

Question 37 of 45

Following gaseous reaction is undergoing in a vessel \(C_{2}H_{4}+H_{2} \leftrightharpoons C_{2}H_{6}: \Delta H=-32.7 Kcal\), Which of the following will increase the equilibrium concentration of \(C_{2}H_{6}\)?

By reducing temperature
By increase of temperature
By removing some hydrogen
By adding some [latex]C_{2}H_{6}[/latex]

Question 38 of 45

in the chemical reaction \(N_{2}+3H_{2} \rightarrow 2NH_{3}\) the product increases by ________ .

increasing pressure
increasing temperature
increasing temperature and pressure both
decreasing temperature and pressure both

Question 39 of 45

Consider the reaction \(A_{2(g)} + B_{2(g)} \leftrightharpoons 2AB_{(g)} ; \Delta H= + ve\)

It occurs at high pressure and high temperature
It occurs at high temperature
It occurs at 1000 pressure
Unaffected by pressure

Question 40 of 45

Gaseous reaction \(A + B \leftrightharpoons 2C + D ; + Q\) is most favoured at which of the following?

Low- temperature and low pressure
High temperature and low pressure
High temperature and high pressure
Low temperature and high pressure

Question 41 of 45

Sodium sulphate dissolves in water with evolution of heat. Consider a saturated solution of sodium sulphate. According to Le-Chatelier principle, if the temperature is raised, then

solution concentration will remain unchanged
the solution will become supersaturated
some solid will precipitate out from the solution
more solid will dissolve

Question 42 of 45

If the equilibrium concentration of A is doubled in the equilibrium \(AB \leftrightharpoons A + B\). the equilibrium concentration of B would become:

half
twice
\(1/4 ^{th}\)
\(1/8 ^{th}\)

Question 43 of 45

The equilibrium constant of the reaction \(H_{2}(g)+I_{2}(g) \leftrightharpoons 2HI\) is 64. What will be the value of the equilibrium constant if volume of the container is reduced to one fourth of its original volume?

128
64
32
16

Question 44 of 45

All reactions that possess chemical disintegration is_____ .

reversible or irreversible and endothermic or exothermic
exothermic
reversible and endothermic
reversible

Question 45 of 45

The following equation gives the exothermic formation of \(ClF_{3}\).

\(Cl_{2(g)}+3F_{2(g)} \leftrightharpoons 2ClF_{3(g)} ; \Delta H= – 329 kj\)

Which of the following will increase the quantity of \(ClF_{3}\) in an equilibrium mixture of \(Cl_{2}, F_{2}\) and \(ClF_{3}?\)

Adding \(F_{2}\)
Increasing the volume of the container
Removing [latex]Cl_{2}[/latex]
Increasing the temperature

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