1. The problem statement, all variables and given/known data What is the pressure inside a $50.0$ L container holding $105.0$ kg of argon gas at $20^\circ$ C? 2. Relevant equations Ideal Gas Law: PV=nRT 3. The attempt at a solution From the ideal gas law, I get [itex] P=\frac{nRT}{V}=\frac{\frac{105.0\times 10^3g}{36g/mol}\times 0.08214\frac{L\cdot atm}{mol\cdot K}\times 293^\circ K}{50.0 L}=25258atm [/itex] which seems much too large. Am I doing something wrong?
Nope! Your answer is quite reasonable, and it seems like nothing looks wrong in your setup of P= nRT/V and all the units match, your value for R is correct and you've converted C to K. Unless you made a calculating mistake, everything looks correct to me.
Oh wow, thanks! It's hard to believe the massive pressure inside, which was why I was skeptical. Thanks again.
On second glance, your molar mass for Argon seems to be off, also, you've made a calculation error. Try again and tell me what you got. (I've worked it out this time).
By looking at the problem you've presented it should look like this: P = [(105000/39.95)(0.08214)(293)]/(50) P = 1265.1 atm P = 1.27 x 10^3 atm I've left out the units for simplicity, but you should write them in yourself.