Editing One LeChatelier's Principle Problem Homework
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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 As<sub>4</sub>O<sub>6</sub> which is then reduced using carbon in the following reaction:<br> <br> 1 As<sub>4</sub>O<sub>6 (s)</sub> + 6 C<sub>(s)</sub> <==> 1 As<sub>(s)</sub> + 6 C<sub>1</sub>O<sub>1 (g)</sub><br> <br> If I have the above chemical reaction in an equilibrium system and add a stress of <b>adding in more carbon monoxide</b>, what would <nowiki>LeChatelier's Principle </nowiki> says would happen (use the blank answer form below).<br> <br> Here is link to notes on <nowiki>LeChaterlier's Principle</nowiki>, [[Equilibrium Notes 3 (Notes on LeChatelier's Principle) ]] <br> <br> Stress: __________________________________________(____________________)_<br> <br> How rxn tries to remove stress: ___________________________________________(__________________)<br> <br> Circle: Make more product or more reactant (fill in for pressure changes)__________________<br> <br> Circle: Favoring: Forward rxn or Backward rxn: (fill in for temperature changes) _____________<br> <br> Circle: Shift Equilibrium to: Left(more reactant) or Right (more product)<br> <br> <br> <br> <br>
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