Over 344.76 K the forward reaction will be spontaneous
calculation
ΔG = ΔH° -TΔs
if ΔG =0
therefore 0 =ΔH°-TΔs
ΔH° = TΔs
divide both side by Δs
T = ΔH°/Δs
convert 34.2 kj into j
that is 1 kj = 1000 j
34.2 kj =? j
by cross multiplication
=[34.2 kj x 1000j / 1 kj] = 34200 j
T is therefore = 34200 j÷99.2 j/k =344.76 k
if T is greater than 344.76 k the forward reaction will be spontaneous
The calculation of temperature is done as follows:
T = ΔH°/ΔS°
= 34.2 kJ/mol / 99.2 × 10⁻³ kJ/molK
= 345 K
Since, ΔS° and ΔH° comes out to be positive for the given reaction. Hence, the given reaction is spontaneous at higher temperature and non spontaneous at lower temperature. Thus, it can be said that above 345 K, the given reaction will become spontaneous.
