Question # 1

The oxidation of SO2 to SO3 is exothermic reaction. The yield of SO3 will be maximum if

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Temperature is increased and pressure is kept constant

Temperature is reduced and pressure is increased

Both temperature and pressure are increased

Which of the following is a base according to lowery Bronsted concept?

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I-1

HCl

H3O+

NH4+1

In a given system, water and ice are in equilibrium, if the pressure is applied to the above system then

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Morc ice is formed

Amount of ice and water will remain the same

more ice is melted

both A and B

If the concentration of salt is greater than the acid in buffer solution, then the

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pH = pKa

pH = pKb

pH > pKa

pH < pKb

lonization of KCIO3. is suppressed by

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Increasing temperatuse

adding KCl

adding NaNO3

Decreasing temperature

The solubility product of AgCl is
2.0 x 10(-10) mol2 dm(-6). The maximum concentration Ag+ ions in the solution is:

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1.41 × 10(-5) mol. dm(-3)

1.41 × 10(-10) mol. dm(-3)

2.0 × 10(-10) mol. dm(-3)

4.0 × 10(-20) mol. dm(-3)

If the temperature is inereased of following reaction, then will go in N2 +3H2 <---------> .2NH3, ∆H= -Ve

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Forward direction

Reverse direction

Remain constant

Cannot be predicted

Correct relationship b/w Kc and Kp can be written as

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Kp=, Kc(R)∆n

Kc=Kp (RT)∆n

Kp.= Kc.(RT)∆n

Kp=Kc (R/N)∆n

If Kc value is small then equilibrium position will shift

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Towards left

Remains unchanged

Towards right

lt is always constant value

In the reaction A2 (g) + 4B2 (g) <-----------> 2AB4 (g) such that ∆H < 0, the formation of AB4(g) will be favoured at

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Low temperature and high pressure

Low temperature and low pressure

High temperature and low pressure

High temperature and high pressure

For the reaction H2(g) +I2 (g) <---------> 2Hl(g). The equilibrium constant changes with

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Total pressure

Catalyst

Concentration of H2 and I2

Temperature

Consider the reaction

PCI5 (g) <---------> PCl3 (g) +Cl2 (g) in a closed container at equilibrium. At a fixed temperature, what will be the effect of adding more PCl5 on the equilibrium constant

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It increases

It remains unaffected

It decreases

Can't be predicted without Ki

If the volume term is present in denominator of Kc expression, then which one is correct

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Increase in pressure will shift the reaction backward

Increase in pressure will shift the reaction forward direction

Decrease in volume will shift the reaction forward direction

Reaction will not effected

What will be the pH of 1.0 mol dm-3 of NH4OH, which is 1% dissociated

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2

12

0

2.7

The pH of ideal buffer is

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10

7

Less than 7

0

Buffer action can be explained by except

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Common ion effect

Le-Chatelier's principle

Law of mass action

Solubility product

At equilibrium, the concentration of reactants and products are

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Constant

Maximum

Different

Equal

Buffer solutions are used in except

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Clinical analysis

Nutrition

Soil science

Qualitative analysis

The pH of neutral water is 6.8 then the temperature of H2O is

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25°C

More than 25°C

less than 25 C°

Not predicted

Which one increases by common ion effect except?

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Crystallization

Solubility

Association of ions

All of these

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