A sample of 4.59 L of CO2 gas has a pressure of 7.56 atm. What volume (in Liters) would the gas occupy if the pressure was reduced to 2.57 atm and the temperature raised from 25.0oC to 39.0oC?

The answer to your question is V = 14.44 L

Explanation:

Data

Conditions 1                            Conditions 2

V1 = 4.69 L                               V2 = ?

P1 = 7.56 atm                           P2 = 2.57 atm

T1 = 25°C                                  T2 = 39°C

Process

1.- Convert the temperature to °K

T1 = 25 + 273 = 298°K

T2 = 39 + 273 = 312 °K

2.- Find V2 using the combined gas law

     (P1V1)/T1 = (P2V2)/T2

solve for V2

     V2 = (P1V1T2) / (T1P2)

substitution

     V2 = (7.56 x 4.69 x 312) / (298 x 2.57)

Simplify

     V2 = 11062.39 / 765.86

Result

     V2 = 14.44 L

the electronic configuration of an atom with eight electrons is 1s²2s²2p⁴. the orbital diagrams are shown in the figure.

as per the hunds rule:

1. electrons tend to avoid being in the same orbital as per as practicable.

2. electrons in different orbitals of the same energy will have their spin parallel.

this can be illustrated from the multiplicity of the orbitals of the atom. as there are four electrons in the p orbital and p orbital has 3 sub-shells. the electrons can be fed in different ways as shown in the figure but the correct orbital diagram will be as per the hunds rule.