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Arsenic can be extracted from its ore (how it found in nature) by first reacting the ore with oxygen (called roasting) to form solid As4O6 which is then reduced using carbon in the following reaction:
1 As4O6 (s) + 6 C(s) <==> 1 As(s) + 6 C1O1 (g)
If I have the above chemical reaction in an equilibrium system and add a stress of adding in more carbon monoxide, what would LeChatelier's Principle says would happen (use the blank answer form below).
Here is link to notes on LeChaterlier's Principle, Equilibrium Notes 3 (Notes on LeChatelier's Principle)
Stress: __________________________________________(____________________)_
How rxn tries to remove stress: ___________________________________________(__________________)
Circle: Make more product or more reactant (fill in for pressure changes)__________________
Circle: Favoring: Forward rxn or Backward rxn: (fill in for temperature changes) _____________
Circle: Shift Equilibrium to: Left(more reactant) or Right (more product)