At constant pressure and 25^0C , a sample of gas occupies 4.5lit. at what temperature will the gas occupy 9.0lit.

Final temperature = 149 K

Explanation:

Given data:

Initial temperature = 25°C (25+273 = 298 K)

Initial volume = 4.5 L

Final temperature = ?

Final volume = 9.0 L

Solution:

The given problem will be solve through the Charles Law.

According to this law, The volume of given amount of a gas is directly proportional to its temperature at constant number of moles and pressure.

Mathematical expression:

V₁/T₁ = V₂/T₂

V₁ = Initial volume

T₁ = Initial temperature

V₂ = Final volume  

T₂ = Final temperature

Now we will put the values in formula.

V₁/T₁ = V₂/T₂

T₂ = T₁V₂/V₁  

T₂ = 4.5 L × 298 K / 9.0 L

T₂ = 1341 L K / 9.0L

T₂ = 149 K

c is having 4 valence electrons and is bonded to three hydrogens and one sulphur atom, therefore, the number of bond pair is equal to four. as all the valence electrons are used in forming the bonds so, there is no lone pair left on carbon.

s is having 6 valence electrons and is bonded to one other sulfur atom and one carbon atom, therefore, the number of bond pair is equal to 2. as only two valence electrons are used in forming the bonds so, four electrons are left. therefore, two lone pairs are present on s.