0.07 mol sample of octane, c^6h^18 absorbed 3.5 x 10^3 j of energy. calculate the temp increase of octane if the molar heat capacity of octane is 254.0 j/k* mol

n = number of moles of sample of octane = 0.07 mol

Q = energy absorbed by a sample of octane = 3.5 x 10³ J

c = molar heat capacity of octane = 254.0 J/K* mol

ΔT = increase in temperature of octane = ?

Heat absorbed is given as

Q = n c ΔT

inserting the values

3.5 x 10³ J = (0.07 mol) (254.0 J/K* mol) ΔT

ΔT = (3.5 x 10³ )/((0.07) (254.0))

ΔT = 196.85 K

hence increase in temperature comes out to be 196.85 K

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.