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Postby JChen_2I » 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?

Kaitlyn Ang 1J
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Re: 5.61b

Postby Kaitlyn Ang 1J » 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.

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Re: 5.61b

Postby 305385703 » 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.

Noe BM 1J
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Re: 5.61b

Postby Noe BM 1J » 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.

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