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Posted: Fri Jan 10, 2020 11:27 am
6CO2(g) + 6H2O(l)->C6H12O6(aq) + 6O2(g) is at equilibrium
How comes when you compress this system, there will be little to no effect on the system? Would the reaction not shift to the formation of reactants because there's less moles?
Posted: Fri Jan 10, 2020 11:29 am
I think that since you’re compressing the entire system, both the pressure of the reactants and products are increasing by the same amount, so in a sense, the ratios aren’t changing so there is little/no effect on the system.
Posted: Sat Jan 11, 2020 3:50 pm
On both sides of the reaction, there are 6 moles of gas, so changing the pressure will not affect the equilibrium.
Posted: Sun Jan 12, 2020 1:12 pm
You only take into account the gases, that's why when compressing the system there's no effect on the equilibrium since there is the same amount of moles of gas on both sides of the reaction.