Ok, so I'm doing this homework online and I THINK I'm doing it correctly, but I'm getting incorrect answers. 1. The problem statement, all variables and given/known data 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? 2. Relevant equations p=(nRT)/V and p(f)/T(f)= p(i)/T(i) 3. 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.