Number 115 Chapter 11 HW

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805132275
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Joined: Fri Sep 28, 2018 12:26 am

Number 115 Chapter 11 HW

Postby 805132275 » Wed Jan 16, 2019 12:51 pm

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??

Helen Zhao 1F
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Joined: Fri Sep 28, 2018 12:20 am

Re: Number 115 Chapter 11 HW

Postby Helen Zhao 1F » Wed Jan 16, 2019 1:50 pm

But because there is an equal number moles of gases on each side of the reaction, compressing the system should have little to no effect.

Melissa Bu 1B
Posts: 36
Joined: Fri Sep 28, 2018 12:19 am

Re: Number 115 Chapter 11 HW

Postby Melissa Bu 1B » Wed Jan 16, 2019 2:34 pm

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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