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I think the purpose is just based on the context of the problem. The problem could give the initial concentration of a gas but then ask you to find the partial pressure at equilibrium or something that requires you to be able to convert one to another when the substance is a gas.
We move elements of the equation around to solve for P and the concentration so we can convert the partial pressure of a gas to its concentration. Being able to do so will be helpful when we deal with heterogenous equilibria.
If there were, would that be a problem? Assuming the gas constant R was given in the correct units and the temperature was specified, I would think there would be enough information to solve a problem even if both partial pressures and concentrations were part of the information provided.
Matt Sanruk 2H wrote:Ok I see, but there won't be any problems that give both concentration and pressure for different elements right?
manipulating the ideal gas law equation gives us a way to convert either partial pressure to concentration or vice versa. so, even if a problem provides values both ways, we should be able to convert them all to the same units.
Matt Sanruk 2H wrote:What was the purpose of changing the equation to equal P or the concentration? Will this be further manipulated when we deal with equilibrium?
The purpose of manipulating PV=nRT is purely to acquire the information that is asked for in the problem, as well as to understand certain concepts. Solving for concentration (n/V) can help understand how changing temperature has on that concentration.
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