States of Matter Test

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States of Matter Test - 1

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Weekly Quiz Competition

Question 1
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Dalton’s Law of Partial Pressures states that the total pressure exerted by the mixture of non-reactive gases is equal to the

A
sum of the partial pressures of individual gases

B
average of the partial pressures of individual gases

C
maximum of the partial pressures of individual gases

D
difference of the partial pressures of individual gases

Solution

Explanation:

The question is based on the statement of Dalton Law of Partial pressures for Gases which states that total pressure exerted by mixture of non reacting gases is equal to the sum of partialpressure of individual gases.
Question 2
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Increase in kinetic energy can overcome intermolecular forces of attraction. How will the viscosity of liquid be affected by the increase in temperature?

A
Decrease

B
Increase

C
No effect

D
No regular pattern will be followed

Solution

Explanation:

Viscosity decreases as Temperature increases.
Question 3
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Avogadro law states that

A
equal volumes of all gases under the similar conditions of temperature and pressure contain equal number of molecules

B
equal volumes of all gases under the same conditions of temperature contain equal number of molecules

C
equal volumes of all gases under the same conditions of temperature and pressure contain different number of molecules

D
equal volumes of all gases under the same conditions of temperature and pressure contain equal number of molecules

Solution

Explanation:

Equal volumes of all gases under the same conditions of temperature and pressure contain equal number of molecules. This is Avagadros Law.
Question 4
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Gay Lussac’s law states that at constant volume, pressure of a fixed amount of a gas

A
directly proportional to square of absolute temperature

B
constant irrespective of its absolute temperature

C
varies directly with the temperature

D
varies inversely with the temperature

Solution

Explanation:

P α T (at constant V).
Question 5
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Gases have much lower density than the solids and liquids because ?

A
Gases contain lower specific enthalpy than solids.

B
Distance between the molecules is small compared to solids.

C
Gases do not have intermolecular forces that attract each molecule to another.

D
Thermal energy overcomes on the attractive intermolecular forces.

Solution

Explanation:

In gases, molecules are far apart from each other, thermal energy which is a measure of freeness of motion is thus very high resulting in a very large volume for the same mass(compared to solid and liquid). Hence there density is lowest.
Question 6
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Three states of matter are the result of?

A
Balance between vanderwaals forces and the London forces.

B
Balance between intermolecular forces and the thermal energy of the molecules

C
Balance between intermolecular forces and the intramolecular bonding energy of the molecules

D
Balance between Hydrogen bonding forces and the London forces.

Solution

Explanation:

Three states of matter are the result of balance between intermolecular forces and the thermal energy of the molecules. These two factors differentiate them from each other. For understanding, The strongest intermolecular forces are in solid then in liquid and weakest in gases.
Question 7
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The average Kinetic energy and Thermal energy are proportional to the

A
Absolute Temperature

B
Specific Heat

C
Pressure

D
Volume

Solution

Explanation:

The average KE and Thermal energy are proportional to absolute Temperature.

The kinetic energy is the amount of motion in the atoms and molecules of a substance. The moleculess of the gas gain energy as the temperature increases as there is more motion of the molecules. As the temperature decreases the motion lessens until at absolute zero all motion (kinetic energy) stops.
Question 8
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The intermolecular force primarily responsible for the condensed states of nonpolar substances is the

A
ion-dipole forces

B
dipole-dipole attraction

C
dispersion force (or London force)

D
hydrogen bond

Solution

Explanation:

The intermolecular force primarily responsible for the condensed states of nonpolar substances is the dispersion force (or London force).
Question 9
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Which of the following statements about Hydrogen bond incorrect?

A
In hydrogen bonding H atom becomes partially positive and is attracted to the more negative F atom.

B
In hydrogen bonding H atom becomes partially positive and is attracted to the more negative O atom.

C
In hydrogen bonding H atom becomes partially negative and is attracted to the more positive N atom.

D
In hydrogen bonding H atom becomes partially positive and is attracted to the more negative N atom.

Solution

Explanation:

Hydrogen atom covalently bonded to highly electronegative atom such as N,O experience electrostatic field of another highly electronegative atom due to which a partial positive charge is developed on H atom.
Question 10
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Physical behavior of the states differs greatly even though chemical behavior of the three states is identical because

A
chemical properties depend on non bonding forces whereas physical properties depend on intermolecular bonding forces

B
chemical properties depend on intramolecular bonding forces whereas physical properties depend on intermolecular nonbonding forces

C
chemical properties depend on intermolecular non bonding forces whereas physical properties depend on intermolecular bonding forces

D
chemical properties depend on covalent bonding forces whereas physical properties depend on energy supplied

Solution

Explanation:

chemical properties depend on intramolecular bonding forces whereas physical properties depend on intermolecular nonbonding forces

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States of Matter Test - 1

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States of Matter Test - 1

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Question 1

sum of the partial pressures of individual gases

average of the partial pressures of individual gases

maximum of the partial pressures of individual gases

difference of the partial pressures of individual gases

Solution

Question 2

Decrease

Increase

No effect

No regular pattern will be followed

Solution

Question 3

equal volumes of all gases under the similar conditions of temperature and pressure contain equal number of molecules

equal volumes of all gases under the same conditions of temperature contain equal number of molecules

equal volumes of all gases under the same conditions of temperature and pressure contain different number of molecules

equal volumes of all gases under the same conditions of temperature and pressure contain equal number of molecules

Solution

Question 4

directly proportional to square of absolute temperature

constant irrespective of its absolute temperature

varies directly with the temperature

varies inversely with the temperature

Solution

Question 5

Gases contain lower specific enthalpy than solids.

Distance between the molecules is small compared to solids.

Gases do not have intermolecular forces that attract each molecule to another.

Thermal energy overcomes on the attractive intermolecular forces.

Solution

Question 6

Balance between vanderwaals forces and the London forces.

Balance between intermolecular forces and the thermal energy of the molecules

Balance between intermolecular forces and the intramolecular bonding energy of the molecules

Balance between Hydrogen bonding forces and the London forces.

Solution

Question 7

Absolute Temperature

Specific Heat

Pressure

Volume

Solution

Question 8

ion-dipole forces

dipole-dipole attraction

dispersion force (or London force)

hydrogen bond

Solution

Question 9

In hydrogen bonding H atom becomes partially positive and is attracted to the more negative F atom.

In hydrogen bonding H atom becomes partially positive and is attracted to the more negative O atom.

In hydrogen bonding H atom becomes partially negative and is attracted to the more positive N atom.

In hydrogen bonding H atom becomes partially positive and is attracted to the more negative N atom.

Solution

Question 10

chemical properties depend on non bonding forces whereas physical properties depend on intermolecular bonding forces

chemical properties depend on intramolecular bonding forces whereas physical properties depend on intermolecular nonbonding forces

chemical properties depend on intermolecular non bonding forces whereas physical properties depend on intermolecular bonding forces

chemical properties depend on covalent bonding forces whereas physical properties depend on energy supplied

Solution

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