answersLogoWhite

0

The given information is not sufficient to answer this question.

You can use the Ideal Gas Law to find out though, expressed mathematically as:

PV=nRT

Where:

P=Pressure (in mmHg)

V=Volume (in Liters)

n=number of moles of gas

R=62.36367 L·mmHg·K−1·mol−1 (Ignore the jargon at the end just know that solving the equation for P will give an answer in the unit mmHg,)

T= Temperature (in Kelvin) (room temperature in Kelivin is 293 K)

You would already need to know V and n to begin with in order to be able to do this equation, however for the sake of example (exactly) one liter and .0094 mole of Argon would be:

P(1)=(.0094)(62.36367)(293)

P= 170 mmHg

One mole or 39.948 grams of Argon would be at a pressure of

P(1)=(1)(62.36367)(293)

P= 18300 mmHg which is 24 times the pressure of Earth's atmosphere.

User Avatar

Wiki User

16y ago

Still curious? Ask our experts.

Chat with our AI personalities

FranFran
I've made my fair share of mistakes, and if I can help you avoid a few, I'd sure like to try.
Chat with Fran
TaigaTaiga
Every great hero faces trials, and you—yes, YOU—are no exception!
Chat with Taiga
EzraEzra
Faith is not about having all the answers, but learning to ask the right questions.
Chat with Ezra
More answers

Argon at room temperature (approximately 20°C) typically exerts a pressure of around 1 atmosphere (atm), which is equivalent to about 101.3 kilopascals (kPa) or 14.7 pounds per square inch (psi).

User Avatar

AnswerBot

10mo ago
User Avatar

Add your answer:

Earn +20 pts
Q: What pressure is argon at room temperature?
Write your answer...
Submit
Still have questions?
magnify glass
imp