When to use PV=nRT

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When to use PV=nRT

Postby Shanzey » Sun Jan 19, 2020 8:53 pm

How do we know when to use the PV=nRT equation? Do we just use it to calculate initial concentration for pressure before creating our ICE table? Were there any homework questions that showed us an example of when/how to use it? Also, do the units for pressure (bars vs. atm) matter when using this equation, or can we use either?

Ariana Iranmahboub1G
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Re: When to use PV=nRT

Postby Ariana Iranmahboub1G » Sun Jan 19, 2020 8:55 pm

It’s often used to convert partial pressure to the molarity or vice versa. It can also be used to understand the effect volume, moles, and temperature will be affected by a change in pressure. In terms of whether to use arm or bar, you units should be the same units you are using for your R constant.
Last edited by Ariana Iranmahboub1G on Sun Jan 19, 2020 10:18 pm, edited 1 time in total.

Janet Nguy 2C
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Re: When to use PV=nRT

Postby Janet Nguy 2C » Sun Jan 19, 2020 9:00 pm

pV = nRT is used to convert between concentrations and partial pressures. Basically it means that you can express K for gases as either their molar concentrations or their partial pressures.

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Re: When to use PV=nRT

Postby CalvinTNguyen2D » Sun Jan 19, 2020 9:10 pm

Ideal gas law is used to convert individual concentrations into partial pressures, and vise-versa. It's useful for expressing K in either Kc (concentration) or Kp (partial pressure).

Kimberly Koo 2I
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Re: When to use PV=nRT

Postby Kimberly Koo 2I » Sun Jan 19, 2020 9:11 pm

Since PV=nRT can be converted into the equation P=(n/V)RT and R is a constant, we can convert from partial pressures to concentration to find K and vice versa

Ruth Glauber 1C
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Re: When to use PV=nRT

Postby Ruth Glauber 1C » Sun Jan 19, 2020 11:41 pm

Does anyone have an example they could walk through?

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