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Jina Kwon wrote:How does the gas law apply to chemical equilibrium?
The ideal gas law is PV = nrt. So, if you are given the pressures of a gas in a problem, and it asks you to find Kc, you can plug the pressure into PV = nRT, and solve for n/V (moles/volume, or molarity). Using this value, you can find Kc.
Similarly, if you are given the concentrations and it asks you to find Kp, plus the concentrations in instead of n/V (molarity) and solve for P. Using this value, you can find Kp.
I believe Prof. Lavelle mentioned it in class today. The gas law allows you to relate Pressure and Volume to concentration. You are then able to convert between partial pressures and concentration of a reactant in a reaction. [Conc.]=P/(RT)
Ronak Naik wrote:The gas law is an expression that relates P and V to concentration. Thus it allows you to convert between partial pressures and concentration of a reactant or product that is in equilibrium during a reaction.
When is it relevant to use this?
It allows us to convert between the partial pressure and molar concentration. the ideal gas law is PV=nRT. You then modify the equation so P=nRT/V and n/v is mol/L which is concentration. When you isolate that, p/RT=n/V which mean p/RT=concentration n. This means that partial pressure/ (gas constant * temp)= molar concentration
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