At what temperature (in K) does the following reaction become spontaneous, if Δ𝐻∘ = 311.1 kJ/mol and Δ𝑆∘ = 707.3 J/mol*K?
Question
At what temperature (in K) does the following reaction become spontaneous, if and ?
Solution
The reaction becomes spontaneous when ΔG° < 0. The formula for ΔG° is ΔG° = ΔH° - TΔS°.
To find the temperature at which the reaction becomes spontaneous, we set ΔG° = 0 and solve for T:
0 = ΔH° - TΔS° T = ΔH° / ΔS°
Substituting the given values:
T = (311.1 kJ/mol) / (707.3 J/mol*K)
Note that we need to convert kJ to J because the units must match. 1 kJ = 1000 J, so:
T = (311.1 * 1000 J/mol) / (707.3 J/mol*K) T = 439.9 K
So, the reaction becomes spontaneous at a temperature of approximately 440 K.
Similar Questions
At what temperature (in K) does the following reaction become spontaneous, if Δ𝐻∘ = 311.1 kJ/mol and Δ𝑆∘ = 707.3 J/mol*K?
At which temperature would a reaction with H = -92 kJ/mol, S = -0.199 kJ/(molK) be spontaneous?A.400 KB.500 KC.600 KD.700 KSUBMITarrow_backPREVIOUS
For a reaction, H = 198 kJ. For which value of TS is the reaction spontaneous?A.0 kJB.396 kJC.-198 kJD.198 kJ
For the reaction PCl5(g) → PCl3(g) + Cl2(g) at298 K, Keq = 1.87 × 10-7, what is ΔrG ° and isthe reaction spontaneous?
This reaction is spontaneous except below −22.°C but proceeds at a slower rate below 165.°C.
Upgrade your grade with Knowee
Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.