Question # 1

Addition of solid NaHCO₃in water causes ionization of NaCHO₃its K_a= 4.7 x 10^-1. Then this solution has character

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Acidic

Very weakly basic

Alkaline

Neutral

Ammonium carbonate when heated to 200°C gives a mixture of NH₃and CO₂vapour with a density of 13.0. What is the degree of dissociation of ammonia carbonate?

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3/2

1/2

2

1

The substance which increases rate of reaction but remains unchanged at the end of reaction is called :

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Catalyst.

Indicator.

Promoter.

Activator.

The optimum conditions of temperature and pressure to get maximum NH₃form N₂and H₂gases is

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2000°C and 10 atmosphere

0°C and 1 atmosphere

400°C and 200-300 atmosphere

200°C and 100 atmosphere

In exothermic reversible reaction increase in temperature shift the equilibrium to :

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Remains unchanged.

Product side.

Reactant side.

None of above.

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HF is stable and does not decompose even at 2000°C

HF is stable and slowly decomposes at 2000°C

HF is strong acid

HF produces equal moles of hydrogen and fluorine

The concentration of reactants is increased by x, then equilibrium constant K becomes

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ln K/x

K/x

K + x

K

In 1000 molecules of 0.001 M acetic acid the number of H⁺ions is 12.6, then its percentage of ionization is

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1.33%

1.26%

12.6

1%

A reaction is reversible because :

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Products are stable.

Reactants are reactive.

Products are reactive.

Reactants re stable.

In an exothermic reaction, a 10° rise in temperature will

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Decrease the value of equilibrium constant

Double the value of K_c

Not produce any change in K_c

Produce some increase in K_c

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High temperature and low pressure

Low temperature and high pressure

Low temperature and low pressure

High temperature and high pressure

Under what condition of temperature and pressure the formation of atomic hydrogen from molecular hydrogen will be favourd

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High temperature and high pressure

Low temperature and low pressure

High temperature and low pressure

:Low temperature and high pressure

The ionic product of H⁺ions and OH^-in water is called ionization constant of water Kw. The value of Kw at 25°C is

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0.11 x 10^-14

0.30 x 10^-14

1.0 x 10^-14

3 x 10^-14

The correct relation b/wK_{c and}K_{p is :}

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K_p = K_c[P/N] ^Δn

K_{c =}K_p(RT) ^Δn

K_{p =}K_c(RT) ^Δn

An aqueous solution is neutral when its

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pH = 14

pH = zero

pH = 7

Kw = 10^-7

Which statement about the following equilibrium in correct?

2SO_{2 (g)}+ O_2(g)---------------2sO_3(g)H= - 188.3 KJ mol-1

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T value of K_{p falls witha rise in temperate.}

The value of K_{p falls withincreasing pressure}

Adding V_2O₅catalyst increase the equilibrium yield of sulfur trioxide

The value of K_{p is equal to}K_p

K_bfor NH₄OH is 1.81 x 10^-5, then K_avalue of its conjugate base is

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1.81 x 10⁺⁵

1.81 x 10^-9

5.5 x 10^-9

5.5 x 10^-10

Chemical equilibrium involving reactants and products in more than one phase is called

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Static

Dynamic

Homogeneous

Heterogeneous

Extent to H₂ + L₂à2Hl can be increased by :

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Increasing temperature.

Increasing product.

Increasing pressure.

Adding a catalyst.

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Reaction occurs at STP

Reaction is exothermic

Reaction is endothermic

Number of moles of production and reactant are same

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Forward

Backward

Already in equilibrium

K_cis never less

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1

10

5

0.33

A chemical reaction is in equilibrium when

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Formation of product is minimum

Reactants are completely transformed into products

Rates of forward and backward reactions are equal

Equal amounts of reactants and products are present

Buffers having pH less than 7 are made

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Mixture of weak acid + salt of it with strong base

Mixture of weak acid + salt of it with weak base

Mixture of weak base + salt of it with strong acid

Mixture of weak base + salt of it with weak base

1 mole of N₂and 2 moles of H₂are allowed to react in a 1 dm³vessel. At equilibrium 0.8 mole of NH₃is formed. The concentration of H₂in the vessel is

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0.6 mole

0.8 mole

0.2 mole

0.4 mole

Units of Kw are

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Mole dm^-3

Mole²dm^-3

Mole²dm^-6

Mole²dm^-3

In a lime kiln, to get higher yield of CO₂, the measure that can be taken is

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To main high temperature

To pump out CO₂

To remove Cao

To add more CaCO₃

Reactions that proceed on both sides and never go to completion are called

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Irreversible reactions

Reversible reactions

Opposing reactions

Spontaneous reactions

The state of equilibrium refers to

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State of rest

Dynamic state

Stationary state

State of inertness

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At equilibrium there is no further change in the concentration of Hl

At equilibrium concentration of l₂remains constant

At equilibrium concentration of H₂remains unaltered

At equilibrium the rate of formation of Hl is equal to the rate of decomposition of Hl

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