THERMOCHEMISTRY - Free Energy
12 important questions on THERMOCHEMISTRY - Free Energy
Is this reaction spontaneous or non spontaneous?
- ΔG < 0
Is this reaction spontaneous or non spontaneous?
- ΔG = 0
- Reaction is at its equilibrium
- has balanced forward and reverse reactions
What happens when:
- ΔH = positive (endo)
- ΔS = positive (more random)
- ΔG = negative (spontaneous)
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How to find at what temperature a reaction is spontaneous?
- Use the Gibbs Free Energy formula
- Find the enthalpy
- ΔHo = npΔHf o ∑ ( p) − nrΔHf o ∑ (r)
- Find the entropy
- ΔSo = np So ∑ (p) − nrSo ∑ (r)
- Know that ΔG < 0 when spontaneous
- Plug in formula
- ΔH − TΔS < 0
- find your Temperature!
T/F You can you measure absolute G
T/F do all elements in their standard state have e ΔG°f = 0?
What is the standard state: 1 bar or 1atm pressure?
- 1 M for aqueous solutions
- At a specified temperature (298K)
What are the two ways to determine ΔG?
- Use equation: ΔGo = ΔHo − TΔSo
- Though you must determine Use ΔH and ΔS
- Use tabulated ΔG values in the CDS
- ΔG = nG(products) - nG(reactants)
How to calculate free energy (G) when T is not 298K?
- Use : ΔGº = ΔHº − TΔSº
- Find the ΔHº and ΔSº
- ASSUME THAT ΔHº and ΔSº are NOT temperature dependent
- Determine G using new temperature
- *** YOU CANNOT USE THE ΔG IN THE TABLES
What is the equation for a non standard free energy?
- Q is the reaction quotient
- ΔG is the non standard
- ΔGº is the standard
- RT ln Q is the correction factor
What is the temperature dependence of K?
- You can plot lnK vs 1/T
What are the four possibilities with different signs of ΔH and ΔS?
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