le chateliers question

[mgdent]

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The balanced equation is:

light + H202 (g) ---> H20 (l) + 1/2 02 (g)

When you increase the pressure, you shift to LESS moles. In this case there is 1 mole of H202 on the left and 1/2 mole of 02 on the right.. Just to make sure, you dont count the H20 because it is not a gas, right? Therefore, you would shift to the right? Thanks.

 

[Lethstang]

u r correct sir

 

[cm8a12321]

The balanced equation is:

light + H202 (g) ---> H20 (l) + 1/2 02 (g)

When you increase the pressure, you shift to LESS moles. In this case there is 1 mole of H202 on the left and 1/2 mole of 02 on the right.. Just to make sure, you dont count the H20 because it is not a gas, right? Therefore, you would shift to the right? Thanks.

For Avogadro's principle, he says that Volume is directly proportional to the number of moles

For Boyle's Law, P is indirectly proportional to Volume.

Thus, when you increase pressure, it also decrease volume and the number of moles.

So, it will favor the side with the fewer number of moles, which in this case is the right (water is ignored because of pure state).

 

[chromosome21]

For Avogadro's principle, he says that Volume is directly proportional to the number of moles

For Boyle's Law, P is indirectly proportional to Volume.

Thus, when you increase pressure, it also decrease volume and the number of moles.

So, it will favor the side with the fewer number of moles, which in this case is the right (water is ignored because of pure state).

pressure increases then volume decreases.. but it does NOT decrease the # of moles. Here, you are talking about gas laws, but the question is related to "equilibrium". Gas law cannot describe why the equilibrium here favors less # of moles.

Increasing pressure will decrease volume and it'll have an effect on equilibrium only if the moles of products and reactants are not the same. Here, we have 1 mole of H2O2 and half mole of O2. So the pressure will make changes to equilibrium.

OP is correct here. When you increase the pressure, you shift to LESS # of moles. and When you decrease the pressure, you shift to MORE # of moles. This is true only with gases. Pressure won't have any obvious effect on solids and liquids.

 

[txlonghorn]

The way you have the equation written, la chatlier's principle does not apply. It will only apply to reversible reactions. Also, I think it applied to electrochemical rxns that are irreversible.