Hi, first timer here! i am facing some problems with chem
equilibrium/thermochemistry... the front page of my lecture notes
states that we are to 'show understanding that the position of
equilibrium is dependent on the standard Gibbs free energy change
of reaction' but nowhere in the lecture notes mention anything
about it... can you please explain how they are related?
Welcome, and feel free to post your H2 Chem qns here. Nonetheless,
do note that :
Tis the Age of the Internet
Google be thy Sword
Wikipedia be thy Shield
- BedokFunland JC
For general Chem conceptual qns like these, there are many
websites on the internet that you're encouraged to check out on
your own first (you know what they say about Singapore education
system spoonfeeding students with notes, until most Sg students
don't know or aren't used to taking the initiative to research out
and learn for themselves in self-directed lifelong learning).
The best type of questions to ask here, is when you have doubts
or disagreements with TYS or Prelim answers, and seek clarification
or a 2nd opinion. That's the best way I can help you guys here.
The relevant formula is ΔG = - R T ln Kc
Mathematically, JC students are expected to know that ln 1 = 0.
So if position of equilibrium lies on the LHS, Kc < 1, then ΔG
> 0, hence the forward reaction is not thermodynamically
feasible (under standard conditions and molarities), the backward
reaction is.
Conversely, if position of equilibrium lies on the RHS, Kc >
1, then ΔG < 0, hence the forward reaction is thermodynamically
feasible (under standard conditions and molarities), the backward
reaction isn't.