H₂S
<h3>Further explanation</h3>
Given
ΔH fusion and ΔH vaporization of different substances
Required
The substance absorbs 58.16 kJ of energy when 3.11 mol vaporizes
Solution
We can use the formula :

Q=heat/energy absorbed
n = moles
The heat absorbed : 58.16 kJ
moles = 3.11
so ΔH vaporization :

The correct substance which has ΔH vaporization = 18.7 kj / mol is H₂S
(H₂S from the data above has ΔH fusion = 2.37 kj / mol and ΔH vaporization = 18.7 kj / mol)
They must have opposite spins
Answer:
The activation energy is 164.02 kJ/mol
Explanation:
Log (k2/k1) = Ea/2.303R × [1/T1 - 1/T2]
k1 = 8.9×10^-4 s^-1
k2 = 9.83×10^-3 s^-1
R = 8.314 J/mol.K
T1 = 540 K
T2 = 578 K
Log (9.83×10^-3/8.9×10^-4) = Ea/2.303×8.314 × [1/540 - 1/578]
1.043 = 6.359×10^-6Ea
Ea = 1.043/6.359×10^-6 = 164020 J/mol = 164020/1000 = 164.02 kJ/mol
Thick cloud covering on earths surface would have a warming effect also known as the "Green House Effect"