Question

a given mass of Sulphur dioxide occupies 500 ml at 47 degree Celsius .To what temperature must the gas be heated to change the volume to 650 ml? assume that the pressure of the gas remains constant​

Answer 1

Answer:

Gaseous state

· Intermolecular forces versus Thermal Energy

· The gaseous state

· The gas laws

· Kinetic Molecular Model of gas

· Real Gases

· Liquefaction of gases and Crirical Point

· The liquid state

· Solids

· Intermolecular Forces

INTERMOLECULAR FORCES

The intermolecular forces are those of attraction and repulsion between interacting particles (atoms and molecules). This term does not include the electrostatic forces that exist between the two oppositely charged ions and the forces that hold atoms of a molecule together i.e., covalent bonds.

Attractive intermolecular forces are known as van der Waals forces. Van der Waals forces vary considerably in magnitude and include dispersion or London forces , dipole-dipole forces, and dipole-induced dipole forces. A particularly strong type of dipole-dipole interaction is hydrogen bonding.

Attractive forces between an ion and a dipole are known as ion-dipole forces and these are not van der Waals forces.

Dispersion Forces or London Forces

Atoms and nonpolar molecules are electrically symmetrical and have no dipole moment because their electronic charge cloud is symmetrically distributed. But a dipole may develop momentarily even in such atoms and molecules. This can be understood as follows. Suppose we have two atoms ‘A’ and ‘B’ in a close vicinity of each other.

Symmetrical distribution of electronic charge cloud

It may so happen that momentarily electronic charge distribution in one of the atoms, say ‘A’ , becomes unsymmetrical i.e., the charge cloud is more on one side than the other (Fig b and c)

Answer 2

The gas must be heated to 246 K to change the volume to 650 ml.

Explanation:

Charles' Law: This law states that volume is directly proportional to the temperature of the gas at constant pressure and number of moles.

$V\propto T$     (At constant pressure and number of moles)

${V_1\times T_1}={V_2\times T_2}$

where,

$V_1$ = initial volume of gas = 500 ml

$V_2$ = final volume of gas = 650 ml

$T_1$ = initial temperature of gas = $47^0c=(47+273)K=320K$

$T_2$ = final temperature of gas = ?

Putting the values:

${500\times 320}={650\times T_2}$

$T_2=246K$

Learn More about Charle's law

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