Which Actions Increase N2 Concentration in Water?

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SUMMARY

The discussion centers on actions that increase the concentration of nitrogen gas (N2) in water within a closed rigid container at equilibrium. The correct answer to the posed question is (C) injecting more N2(g) into the container. Shaking the container (I) does not affect the concentration since equilibrium is already established, and raising the temperature (II) decreases gas solubility according to Henry's law. Therefore, only the injection of additional N2(g) increases its concentration in the water.

PREREQUISITES
  • Understanding of Henry's law and its implications on gas solubility.
  • Familiarity with Le Chatelier's principle and its application to equilibrium systems.
  • Knowledge of the effects of temperature on gas solubility in liquids.
  • Basic concepts of chemical equilibrium in closed systems.
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  • Study Henry's law and its mathematical formulation for gas solubility.
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  • Examine the relationship between temperature and gas solubility in various liquids.
  • Explore the dynamics of gas behavior in closed systems and equilibrium shifts.
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Homework Statement


A closed rigid container contains distilled water
and N_{2}(g) at equilibrium. Actions that would
inctease the concentration of N_{2}(g) in the
water include which of the following?
I. Shaking the container vigorously
II. Raising the temperature of the water
III. Injecting more N_{2}(g) into the container
(A) I only
(B) II only
(C) III only
(D) I and II only
(E) I, II, and III


Homework Equations


- Henry's law states that more pressure means more solubility but don't know if that works here.
- We could try Le chatelier's principle


The Attempt at a Solution


To be honest I'm not very sure what the question is asking. The answer happens to be choice (C) but I can't figure my way around it. When I answered it initially, I wrote down A but no clue why it should be C. Is the question asking about the solubility of nitrogen gas in the water, or something else? Surely if you add gas, the concentration of the gas must increase even if equilibrium tries to consume some of it, the net change of the gas's concentration will still be positive right? So I know that III is definitely true, but I can't seem to work out I and II. I feels right, since shaking it should increase pressure?

I appreciate any help on this question. Thanks!

BiP
 
Physics news on Phys.org
Shaking can speed up reaching equilibrium, but you are told you already are at the equilibrium, so shaking doesn't matter.

Solubility of gases lowers with temperature.
 

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