Chemistry

A gas occupies a volume of .350 L at a temperature of 18.0 degrees Celsius and a pressure of 980.0 torr. What will be the volume of this gas at standard conditions? Please explain how to do it.

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1. p v = n R T
n and R the same

so
P1 V1/T1 = P2 V2/T2

T1 = 18 + 273
T2 = 273

P1 = 980 Torr
P2 = 760 Torr

V1 = .35
V2 = ?

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posted by Damon
2. Why are n and R the same? Isn't n the mol's and R the ideal gas constant?

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posted by Linda
3. Damon used PV = nRT. n isn't known at the conditions listed. Using those conditions allows the evaluation of n. Then that value of n is used in another PV = nRT calculation to solve for the volume at the new conditions.

You can avoid that problem if you use
(P1V1/T1) = (P2V2/T2) and just one calculation.
To answer your question, yes, n is mols and R is constant. The P1V1/T1 = P2V2/T2 avoids the use of both n and R although they are used inherently (perhaps intrinsically is a better word).

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posted by DrBob222
4. Okay, I understand that part, but if I use P1V1=P2V2, what happens to the temperature that they gave me? What do I do with it?

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posted by Linda
5. I don't see a P1V1 = P2V2.
I see a (P1V1/T1) = (P2V2/T2) so the T is taken into account.

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posted by DrBob222
6. Oh okay, my bad, and thank you for your help

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posted by Linda

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