Answer :
we are going to use this formula:
Δ H = T * ΔS
when Δ H is the change in enthalpy
and T is the temperature in Kelvin = 100+273= 373 K
and ΔS is the change in entropy
but first, we need to get the value of ΔH:
ΔH = mass * molar mass per mole * enthalpy of vaporization
by substitution:
ΔH = 51.1 g * (1 mole/18g) * 40.67KJ/mole
= -115.5 KJ
we use negative sign because this is an exothermic reaction.
by substitution on the first formula, we will get the change of entropyΔS:
ΔS = ΔH / T
= -115.5 KJ / 373K
= 310 J/K
Δ H = T * ΔS
when Δ H is the change in enthalpy
and T is the temperature in Kelvin = 100+273= 373 K
and ΔS is the change in entropy
but first, we need to get the value of ΔH:
ΔH = mass * molar mass per mole * enthalpy of vaporization
by substitution:
ΔH = 51.1 g * (1 mole/18g) * 40.67KJ/mole
= -115.5 KJ
we use negative sign because this is an exothermic reaction.
by substitution on the first formula, we will get the change of entropyΔS:
ΔS = ΔH / T
= -115.5 KJ / 373K
= 310 J/K