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Equilibrium

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Q 1. The oxidation of {tex} \mathrm { SO } _ { 2 } {/tex} by {tex} \mathrm { O } _ { 2 } {/tex} to {tex} \mathrm { SO } _ { 3 } {/tex} is an exothermic reaction. The yield of {tex} \mathrm { SO } _ { 3 } {/tex} will be maximum if

temperature is increased and pressure is kept constant

temperature is reduced and pressure is increased

both temperature and pressure are increased

both temperature and pressure are reduced

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Q 2. For the reaction {tex} \mathrm { H } _ { 2 } ( \mathrm { g } ) + \mathrm { I } _ { 2 } ( \mathrm { g } ) \rightleftharpoons 2 \mathrm { HI } ( \mathrm { g } ) , {/tex} the equilibrium constant {tex} K _ { p } {/tex} changes with

total pressure

catalyst

the amounts of {tex} \mathrm { H } _ { 2 } {/tex} and {tex} \mathrm { I } _ { 2 } {/tex} present

temperature

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Q 3. One mole of {tex} \mathrm { N } _ { 2 } \mathrm { O } _ { 4 } ( \mathrm { g } ) {/tex} at {tex} 300 \mathrm { K } {/tex} is kept in a closed container under one atmosphere. It is heated to {tex} 600 \mathrm { K } {/tex} when {tex} 20 \% {/tex} by mass of {tex} \mathrm { N } _ { 2 } \mathrm { O } _ { 4 } ( \mathrm { g } ) {/tex} decomposes to {tex} \mathrm { NO } _ { 2 } ( \mathrm { g } ) {/tex}. The resultant pressure is

1.2 atm

2.4atm

2.0 atm

1.0 atm

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Q 4. Haber-Bosch process for the manufacture of {tex} \mathrm { NH } _ { 3 } {/tex} is based on the reaction

{tex} \mathrm { N } _ { 2 } ( \mathrm { g } ) + 3 \mathrm { H } _ { 2 } ( \mathrm { g } ) \stackrel { \text { catalyst } } { \rightleftharpoons } 2 \mathrm { NH } _ { 3 } ( \mathrm { g } ) ; \quad \Delta _ { \mathrm { r } } H ^ { \circ } = - 45.0 \mathrm { kJ } \mathrm { mol } ^ { - 1 } ; K _ { p } ^ { \circ } = 14 {/tex}

Which of the following information regarding the above reaction is correct?

On adding {tex} \mathrm { N } _ { 2 } , {/tex} the equilibrium is shifted to right side with an increase in entropy.

The equilibrium constant {tex} K _ { p } ^ { \circ } {/tex} increases with increase in temperature.

At equilibrium, {tex} 2 G _ { \mathrm { m } } \left( \mathrm { NH } _ { 3 } \right) = G _ { \mathrm { m }} ( \mathrm { N_2 } ) + 3 G _ { \mathrm { m } } \left( \mathrm { H } _ { 2 } \right) {/tex} where {tex} G _ { \mathrm { m } } {/tex} represents the molar Gibbs function of the species enclosed within the brackets.

The use of catalyst helps increasing the rate of forward reaction more than that of backward reaction thereby increasing the yield of {tex} \mathrm { NH } _ { 3 } {/tex}.

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Q 5. The {tex} \% {/tex} yield of ammonia as a function of time in the reaction {tex} \mathrm { N } _ { 2 } ( \mathrm { g } ) + 3 \mathrm { H } _ { 2 } ( \mathrm { g } ) \rightleftharpoons 2 \mathrm { NH } _ { 3 } ( \mathrm { g } ) ; \Delta H < 0 {/tex} at {tex} \left( P , T _ { 1 } \right) {/tex} is given below:

If this reaction is conducted at {tex} \left( P , T _ { 2 } \right) , {/tex} with {tex} T _ { 2 } /> T _ { 1 } , {/tex} the {tex} \% {/tex} yield of ammonia as a function of time is represented by

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Q 6.

A solution which is is treated with M sulphide ion. If

respectively, which one will

precipitate first?

On the basis of precipitation concept an electrolyte will be precipitated firstly whose ionic product is exceeded to its solubility product. In similar ionic conc. of cations, an electrolyte is precipitated firstly for which is lower. In these electrolytes

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Q 7.

Which of the following salts will not undergo hydrolysis in water?

Sodium sulphate

Ammonium sulphate

Aluminium sulphate

All the salts will hydrolyse

Salt of

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Q 8.

Precipitation starts when

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Q 9.

For the reversible reaction

at ^{ }when the partial pressure is measured in atmosphere. The corresponding value of

or

or

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Q 10.

For the system

_{ }for the reaction is

250

416

125

_{ }At

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Q 11.

The pH of a dilute solution of acetic acid was found to be 4.3. The addition of a small crystal of sodium acetate will cause pH to

Becomes less than 4.3

Become more than 4.3

Remain equal to 4.3

Unpredictable

Due to common ion

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Q 12.

The pH of a solution of weak base at neutralization with strong acid is 8.

None of there

At half neutralization,

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Q 13.

Auto-ionisation of liquid

With

Number of amide ions

602

301

200

100

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Q 14.

1 mol of _{ }in a litre container. If 50% of _{ } then the total number of

moles of gas at the equilibrium are

1.5

4.5

3

6

_{ }

Total moles

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Q 15.

pH signifies:

Puissance de hydrogen

All the above

pH stands for Fench word puissance de hydrogen which means power of hydrogen ions

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Q 16.

The

Unionized in the small intestine and in the stomach

Completely ionsed in the small intestine and in the stomach

Ionized in the stomach and almost unionized in the small intestine

Ionized in small intestine and almost unionized in the stomach

Aspirin is a weak acid ad its ionization is suppressed due to common ion effect in acidic medium, i.e., in stomach. Therefore, aspirin is unionized in stomach whereas in small intestine its pH is basic. So the ionization of aspirin increases, that is why it is completely ionized in small intestine

Therefore, ionization of aspirin increases

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Q 17.

Passing

CuS and HgS

MnS and CuS

MnS and NiS

NiS and HgS

In acidic medium,

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Q 18.

In the formation of nitric acid,

Low temperature

High temperature

Freezing point

All are favourable

The above equation shows that the reaction is endothermic. Endothermic reactions are forward in forward direction at high temperature

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Q 19.

The decomposition of _{ }and

_{ }

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Q 20.

Solubility of salt

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Q 21.

In 1L saturated solution of

3

5

7

9

It is a case of simultaneous solubility of salts with a common ion. Here solubility product of

Now for

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Q 22.

The conjugate acid of

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Q 23.

In alkaline solution, the following equilibrium exist

a. ^{ }equilibrium constant

b. ^{ }equilibrium constant

132

1.09

0.918

i.

ii.

The equation constant for the reaction,

iii.

Since eq. (iii) is obtained by reversing and adding equations (i) and (ii)

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Q 24.

If ammonia is added to pure water, the concentration of a chemical species already present will decrease. The species is

Due to common ion

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Q 25.

The equilibrium constant for a reaction

The chemical process resulting in the formation of C and D is

Exothermic

Endothermic

Unpredictable

None

Since

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