A 1.18 L sample of gas at 759 mm Hg pressure is expanded until its volume is 2.06 L. What will be the pressure in the expanded gas sample (at constant temperature)?

434.77 mmHg

Explanation:

Data obtained from the question include:

V1 (initial volume) = 1.18 L

P1 (initial pressure) = 759 mmHg

V2 (final volume) = 2.06 L

P2 (final pressure) =?

The Boyle's law equation P1V1 = P2V2, will be use to obtain the final pressure of the gas since the temperature is constant. So, applying the Boyle's law equation, the final pressure is obtained as shown below:

P1V1 = P2V2

759 x 1.18 = P2 x 2.06

Divide both side by 2.06

P2 = (759 x 1.18)/2.06

P2 = 434.77 mmHg

Therefore, the final pressure of the gas is 434.77 mmHg

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.