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
Solution 1
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 Knowee AI StudyGPT is a powerful AI-powered study tool designed to help you to solve study prob
Knowee AI StudyGPT is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI StudyGPT is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI StudyGPT is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI StudyGPT is a powerful AI-powered study tool designed to help you to solv
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?
Calculate the Gibbs free energy change (in kJ/mol) when Δ𝐻∘ = 910.1 kJ/mol, Δ𝑆∘ = 744.1 J/mol*K, and T = 261.3 K.
What is the ΔG° at room temperature of the reaction 2CO+O2→2CO2, if ΔH°=-128.3 kJ and ΔS°= - 159.5 J/K ?*- 80. 769 kJ80. 769 kJ- 175.831 kJ- 124.313 kJ
At 298 K, H0 = -314 kJ/mol and S0 = -0.372 kJ/(K•mol). What is the Gibbs free energy of the reaction?A.-425 kJB.0.393 kJC.34,900 kJD.-203 kJ
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