Organic Chemistry Question

Question

A sample of argon gas at a pressure of 0.894 atm and a temperature of 199 °C, occupies a volume of 853 mL. If the gas is heated at constant pressure until its volume is 998 mL, the temperature of the gas sample will be?

Answer 1

Using the Ideal Gas Law, I would first figure the moles at the lower volume measurement and then plug that into the T=PV/nR at the expanded volume, given a pressure that remains constant, giving us a Temperature of 544 Kelvin.

a) n=(.894 atm)(.853 L)(molxK)/(472.15K)(0.082057 Lxatm)=0.020 moles

b) Add into T=PV/nR

c) T=(0.894 atm)(.998L)(molxK)/(0.020 moles)(0.082057 Lxatm)=544 Kelvin