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
Question
Solution 1
The spontaneity of a reaction can be determined using the Gibbs Free Energy equation:
ΔG = ΔH - TΔS
Where: ΔG is the change in Gibbs Free Energy ΔH is the change in enthalpy T is the temperature in Kelvin ΔS is the change in entropy
For a reaction to be spontaneous, ΔG must be less than 0.
Given Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI
Similar Questions
Question 1 of 30What is the temperature in kelvins of 23oC?A.-250 KB.6279 KC.11.9 KD.296 KSUBMITarrow_backPREVIOUS
At what temperature (in K) does the following reaction become spontaneous, if Δ𝐻∘ = 311.1 kJ/mol and Δ𝑆∘ = 707.3 J/mol*K?
What is the value for G at 1000 K if H = -220 kJ/mol and S = -0.05 kJ/(molK)?A.-270 kJB.-220 kJC.780 kJD.-170 kJ
What is the value for G at 1000 K if H = -220 kJ/mol and S = -0.05 kJ/(molK)?A.-270 kJB.-170 kJC.-220 kJD.780 kJSUBMITarrow_backPREVIOUS
If 3 moles of a compound use 12 J of energy in a reaction, what is the Hreaction in kJ/mol?A.-4 kJ/molB.4 kJ/molC.-0.004 kJ/molD.0.004 kJ/mol
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.