Question # 1

Decomposition of H2O is

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Endothermic reaction

Nuclear reaction

Exothermic reaction

Zero nuclear reaction

The enthalpies of all elements in their standard states are

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Unity

always +ve

always -ve

zero

For an endothermic reaction, enthalpy of reactants

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Is smaller than that of the products

Is greater than that of the products

Must be greater or smaller than that of the products

Is equal to that of the products

Enthalpy of neutralization (∆H°n) per mole of H2SO4/ Ba(OH)2 is

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+57.4 kJmol-1

-114.8 kJmol-1

-57.4 kJmol-1

Change in enthalpy (∆H) of a system can be calculated by

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∆H=∆E - PV

ΔH =ΔE +q

∆H = ∆E - q

∆Η = ΔΕ + P∆V

The enthalpy of formation of a compound is

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Positive

Either positive or negative

Negative

None

The change in enthalpy when one mole of a substance is dissolved in a specified quantity of solvent at a given temperature is called

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Heat of reaction

Heat of solvation

Heat of combustion

Heat of solvent

The change in enthalpy of a system when one mole of the substance is completely burnt in excess of air or oxygen is called

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Heat of reaction

Heat of formation

Heat of atomization

Heat of combustion

If an endothermic reaction is allowed to take place very rapidly in air, the temperature of the surrounding air will

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Remains constant

Increase

Decrease

Either increase or decrease

One Joule is equivalent to

A state function which describes together the internal energy and product of pressure and volume is called

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Enthalpy

internal energy

Work

Kinetic energy

Which of the following enthalpy change always have a negative value

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∆Hf

∆H sol

∆Hc

∆Hat

Hess's law is analogous to

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Law of heat summation

law of increasing entropy

Law of heat exchange

Ist law of thermodynamics

The net heat change in a chemical reaction is the same whether it is brought about in two or more different ways in one or several steps.it is known as

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Henry's law

Hess's law

joule's law

Law of conservation of energy

Enthalpy of neutralization of strong acids and strong bases have same values because

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Neutralization leads to the formation of salt and water

Acids always give rise to H+ and bases always furnish OH-

Strong acids and bases are ionic substances

The net change involves the combination of H and OH ions to form water

Enthalpy of formation of one mole of ionic compound form gaseous ion under standard condition is called

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Gibb's energy

Bond energy

Lattice energy

Choose from the followings the correct statement about Born Haber cycle

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Born Haber cycle is different from Hess's law

The energy changes in a cyclic process is not zero

The lattice energy of crystalline substances can be calculated easily

None

According to Hess's law, the enthalpy change for a reaction

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Depends on path

Independent of the path

The sum of ∆E and ∆H

None of these

If internal energy of the system is increased

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Change in state of the system may occur

Temperature of the system may rise

Chemical reaction may take place

All of these

In order to determine ∆H (latt) of ionic compound which is correct relationship

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∆H latt. = ∆Hf - ∆Hx

∆H latt. = ∆Ha + ∆Hv

∆H latt. = ∆Hf + ∆Hx

∆H latt. = ∆Hf - ∆H sol.

ΔH° represent the enthalpy change at

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0°C and 1 atm pressure

25°Cand 1atm

0K and I atm pressure

25°C and 2 atm pressure

Which of the following has positive value of enthalpy

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Neutralisation

Atomization

combustion

All of the above

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