Using Ideal Gas Law to find P, V, or T

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SUMMARY

The discussion centers on applying the Ideal Gas Law to determine the final pressure of argon gas in a specified scenario. The user correctly identifies the initial conditions: 0.290 mol of argon gas in a 40.0 cm³ container at 60.0°C, using the equation p=(nRT)/V. The initial pressure calculated was 2.01x107 atm, but the user later realizes that the pressure should be expressed in Pascals, leading to a final pressure of 3.46x104 Pa after conversion. The key takeaway is the importance of unit consistency when applying the Ideal Gas Law.

PREREQUISITES
  • Understanding of the Ideal Gas Law (p=(nRT)/V)
  • Knowledge of unit conversions, particularly between atm and Pa
  • Familiarity with temperature conversion from Celsius to Kelvin
  • Basic skills in algebra for manipulating equations
NEXT STEPS
  • Study the Ideal Gas Law applications in different scenarios
  • Learn about unit conversions between various pressure units (atm, Pa, kPa)
  • Explore the implications of isochoric processes in thermodynamics
  • Investigate the significance of the ideal gas constant (R) and its units
USEFUL FOR

This discussion is beneficial for students studying chemistry or physics, particularly those focusing on gas laws, as well as educators seeking to clarify concepts related to the Ideal Gas Law and unit conversions.

Samurai Weck
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Ok, so I'm doing this homework online and I THINK I'm doing it correctly, but I'm getting incorrect answers.

Homework Statement



0.290 mol of argon gas is admitted to an evacuated 40.0 cm^3 container at 60.0 degrees C. The gas then undergoes an isochoric heating to a temperature of 300 degrees C.

What is the final pressure of the gas?

Homework Equations



p=(nRT)/V and p(f)/T(f)= p(i)/T(i)

The Attempt at a Solution



Okay, so I need to find p(i).
n=.290 mol
V=40 cm^3 = 40cm^3(1m/100 cm)^3 = 4x10^-5 m^3
T= 60.0 degrees C = 60 C + 273 = 333 K
R= the ideal gas constant which is 8.31 J/mol K

Therefore,
p(i)= (.290 mol * 8.31 J/mol K * 333 K)/ (4x10^-5 m^3)
p(i) = 2.01x10^7 atm

Now that I know p(i), i can then solve for the temperature increase to find p(f)

p(f) = p(i)T(f)/T(i)
p(f) = (2.01x10^7 atm * 573 K)/ 333 K = 34586486 atm = 3.46x10^7 atm

They want the answer in kPa, and converting atm to kPa online yielded 3.50x10^10.

I'm completely clueless as to what I'm doing wrong. There are two other problems asking for either p or V which seem to have the same basis. If I can figure out what I'm doing wrong here, I should be able to understand why I'm doing the rest wrong. Thank you.
 
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Ah, disregard my question. I was mistaken when I thought that pressure in p=nRT comes out in atm. It actually is in Pa and you have to change 3.46x10^7 to 3.46x10^4.
 

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