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6CO2 + 6H2O-----> C6H12O6 + 6O2. I don't understand why compressing the system has, according to the book, little to no effect on the shift towards reactants or products. I thought that since pressure was being increased, the products are favored because there are fewer molecules on the product side.
Change in pressure does not change K. In this case, even though more pressure may be on the reactants, the reaction will eventually reach equilibrium again and balance out. Refer to page 129 in the course reader.
Since H2O is a liquid, you would not consider its moles when determining the effect the compression would have. Thus, the number of moles on the products and reactants side would be almost identical. So there would not really be an effect. Hope this helped!
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