Increasing Pressure

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Increasing Pressure

Postby Sophia_Kiessling_2L » Fri Jan 25, 2019 11:01 am

For the homework question 5J.5 (7th edition), part E asks "if there is a change in overall pressure, what is the change in equilibria?" for the reaction Cl2 (g) ⇄ 2Cl (g). The answer book says that reactants are favored but why is that?

Jerome Mercado 2J
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Re: Increasing Pressure

Postby Jerome Mercado 2J » Fri Jan 25, 2019 11:43 am

Reactants are only favored when pressure increases equilibrium shifts to the side where there is less moles. This is Le Chatelier's Principle. When pressure decreases it would do the opposite: equilibrium would shift to the side where there is more moles.

Sean Reyes 1J
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Re: Increasing Pressure

Postby Sean Reyes 1J » Fri Jan 25, 2019 5:54 pm

We can use the amount of moles on each side of the reaction to justify this.
Because there is one mole of Cl2 on the reactants side and 2 moles of Cl in the products side, and increase in the pressure (through reduction of volume) would favor the reaction that produces less moles of gas, in this case the reverse reaction

Karina Jiayu Xu 4E
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Joined: Fri Sep 28, 2018 12:29 am

Re: Increasing Pressure

Postby Karina Jiayu Xu 4E » Fri Jan 25, 2019 9:53 pm

an increase in pressure would shift the reaction towards the side with less moles.

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