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for the equation 6CO2(g)+6H2O(l)-->C6H12O6(aq) + 6O2(g), would the system being compressed mean that the volume decrease and pressure increases? As a result, since technically liquid isn't included in the equilibrium constant, shouldn't equilibrium favor the reactants??
I believe the "quick way" Dr. Lavelle described in class to determine which way the reaction shifts when the pressure increases only applies for moles of gas, not gas and aqueous solutions. The quick way is to see which side has fewer moles of gas and the reaction will proceed in that direction. Since there are 6 moles of gas on both sides of the reaction, no change is observed.
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