increasing pressure, what happens to concentration?

[Josephine Lu 4L]

Why is it that when we increase pressure, the reaction favors the side with less moles of gas?

[Julia Go 2L]

According to Le Chatelier's Principle, a change in pressure will result in an attempt to restore equilibrium by creating more or less moles of gas. For example, if the pressure in a system increases, the equilibrium will shift to favor the side of the reaction that involves fewer moles of gas. Similarly, if the the pressure decreases, the production of additional moles of gas will be favored. A system will try to minimize the disturbance.

[Selina Bellin 2B]

increasing pressure will make the reaction go in the direction where there are LESS moles

[Lopez_Melissa-Dis4E]

According to Le Chatelier's Principle, if you increase the pressure the reaction will go towards the side with less moles.

[Krista Mercado 1B]

Increasing pressure will cause the reaction to proceed towards the side with less moles of gas.

[Hannah Pham 1D]

Take volume into account. The reaction will favor the side with fewer moles.

[Jeannine 1I]

You can imagine that when pressure increases, the gas molecules on both sides of the reaction move faster, and are therefore more likely to bump into each other. The side with more moles of gas will have more molecules that bump into each other, which will drive the reaction to shift towards the side with less moles.

I hope that helps! I'm more of a visual learner myself, so imagining what things would look like helps me understand it better(:

[Xingzheng Sun 2K]

When pressure is increased, the reaction wants to do something to reduce the effects. Lowering the number of molecules can decrease the pressure which reduce the effect.

[Tony Chung 2I]

Le Chatelier's Principle for pressure: if the pressure increases, the reaction will proceed towards the side with less moles of gas. if the pressure is decreased, the reaction will proceed towards the side with more moles of gas.

[jlinwashington1B]

when pressure increases, the reaction is attracted to the side with fewer moles.

[Sarah_Kang_2K]

When pressure increases, the gaseous molecules on both sides of the reaction increasingly collide with each other. In order to alleviate/compensate for these increased collisions, the reaction favors the side with the less number of moles of gaseous molecules.