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The variation of pressure with volume of the gas at different temperatures can be graphically represented as shown in Fig. 5.3.
On the basis of this graph answer the following questions.
1. How will the volume of a gas change if its pressure is increased at constant temperature?
2. At a constant pressure, how will the volume of a gas change if the temperature is increased from 200K to 400K?
The variation of pressure with volume of the gas at different temperatures can be graphically represented as shown in Fig. 5.3.
On the basis of this graph answer the following questions.
1. How will the volume of a gas change if its pressure is increased at constant temperature?
2. At a constant pressure, how will the volume of a gas change if the temperature is increased from 200K to 400K?
This is a short answer type question as classified in NCERT Exemplar
1. According to Boyle's law,
Pressure of a gas is inversely proportional to volume of gas at constant temperature. So, the volume decreases with increase in pressure at constant temperature.
2. According to Charles's
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Explain the effect of increasing the temperature of a liquid, on intermolecular forces operating between its particles, what will happen to the viscosity of a liquid if its temperature is increased?
Explain the effect of increasing the temperature of a liquid, on intermolecular forces operating between its particles, what will happen to the viscosity of a liquid if its temperature is increased?
This is a short answer type question as classified in NCERT Exemplar
The increase in temperature increases the kinetic energy of the molecules which decreases the intermolecular forces operating between its particles and hence, the viscosity of a liquid decreases. So, the viscosity of a liquid
Upvote Viscosity of a liquid arises due to strong intermolecular forces existing between the molecules. Stronger the intermolecular forces, greater is the viscosity. Name the intermolecular forces existing in the following liquids and arrange them in the increasing order of their viscosities. Also give reason for the assigned order in one line.
Water, hexane (CH3CH2CH2CH2CH2CH3), glycerine (CH2OH CH(OH) CH2OH) .
Viscosity of a liquid arises due to strong intermolecular forces existing between the molecules. Stronger the intermolecular forces, greater is the viscosity. Name the intermolecular forces existing in the following liquids and arrange them in the increasing order of their viscosities. Also give reason for the assigned order in one line.
Water, hexane (CH3CH2CH2CH2CH2CH3), glycerine (CH2OH CH(OH) CH2OH) .
This is a short answer type question as classified in NCERT Exemplar
Hexane is a nonpolar molecule which has london force between the molecules, which is a weak force.
Water and glycerine have O atoms which is an electronegative atom that forms H bonding between the molecules along w
Upvote Name two phenomena that can be explained on the basis of surface tension.
Name two phenomena that can be explained on the basis of surface tension.
This is a short answer type question as classified in NCERT Exemplar
The two phenomena that can be explained on the basis of surface tension are:
1. Spherical shape of rain droplets.
2. Capillary action due to which the liquid in capillary rises and falls.
Upvote The relation between pressure exerted by an ideal gas (pideal) and observed pressure (preal) is given by the equation:
If pressure is taken in Nm-2, number of moles in mol and volume in m3, Calculate the unit of 'a'.
What will be the unit of 'a' when pressure is in atmosphere and volume in dm3?
The relation between pressure exerted by an ideal gas (pideal) and observed pressure (preal) is given by the equation:
If pressure is taken in Nm-2, number of moles in mol and volume in m3, Calculate the unit of 'a'.
What will be the unit of 'a' when pressure is in atmosphere and volume in dm3?
This is a short answer type question as classified in NCERT Exemplar
Unit of ‘P’ = N m-2
Unit of ‘a’ = N m-2 X (m3)2 / (mol)2
= N-m4 mol-2
Unit of ‘a’ when pressure is in atm, and volume in dm3
Unit of ‘P’ = atm
Unit of ‘a’
Upvote For real gases the relation between p, V and T is given by van der Waals equation:
where 'a' and are van der Waals constants, 'nb' is approximately equal to the total volume of the molecules of a gas.
'a' is the measure of magnitude of intermolecular attraction.
I. Arrange the following gases in the increasing order of 'b'. Give reason. O2, CO2, H2, He
II. Arrange the following gases in the decreasing order of magnitude of ‘a’. Give reason. CH4, O2, H2.
For real gases the relation between p, V and T is given by van der Waals equation:
where 'a' and are van der Waals constants, 'nb' is approximately equal to the total volume of the molecules of a gas.
'a' is the measure of magnitude of intermolecular attraction.
I. Arrange the following gases in the increasing order of 'b'. Give reason. O2, CO2, H2, He
II. Arrange the following gases in the decreasing order of magnitude of ‘a’. Give reason. CH4, O2, H2.
This is a short answer type question as classified in NCERT Exemplar
I.The increasing order of ‘b’ of the given gases is:
H2 < He < O2 < CO2
Volume of a gas is proportional to the size of the molecule.
II.The decreasing order of magnitude of ‘a’ of the given molecule is:
CH4 > O2
Upvote The critical temperature (Tc) and critical pressure ( pc) of CO2 are 30.98°C and 73 atm respectively. Can CO2 (g) be liquefied at 32°C and 80 atm pressure?
The critical temperature (Tc) and critical pressure ( pc) of CO2 are 30.98°C and 73 atm respectively. Can CO2 (g) be liquefied at 32°C and 80 atm pressure?
This is a short answer type question as classified in NCERT Exemplar
The CO2 gas cannot be liquified at the 32°C and 80 atm pressure as the given temperature and pressure are above critical temperature (Tc) and critical pressure (pc) which are 30.98°C and 73 atm respectively.
Upvote Compressibility factor, Z, of a gas is given as Z=
(i) What is the value of Z for an ideal gas?
(ii) For real gas what will be the effect on value of Z above Boyle’s temperature?
Compressibility factor, Z, of a gas is given as Z=
(i) What is the value of Z for an ideal gas?
(ii) For real gas what will be the effect on value of Z above Boyle’s temperature?
This is a short answer type question as classified in NCERT Exemplar
(i) The value of Z for an ideal gas is 1.
(ii) For real gas, the value of Z > 1 above Boyle's temperature
Upvote One of the assumptions of kinetic theory of gases is that there is no force of attraction between the molecules of a gas. State and explain the evidence that shows that the assumption is not applicable for real gases.
One of the assumptions of kinetic theory of gases is that there is no force of attraction between the molecules of a gas. State and explain the evidence that shows that the assumption is not applicable for real gases.
This is a short answer type question as classified in NCERT Exemplar
The assumption of kinetic theory of gases that there is no force of attraction between the molecules of a gas is applicable for real gases. The evidence for this is that the real gas can be liquified at high pressure and low t
Upvote Name two intermolecular forces that exist between HF molecules in liquid state.
Name two intermolecular forces that exist between HF molecules in liquid state.
This is a short answer type question as classified in NCERT Exemplar
The two intermolecular forces that exist between HF molecules in liquid state are hydrogen bonding (as F is a highly electronegative atom) and dipole-dipole interaction (as HF is a polar molecule).
Upvote