Answer: 0.0238 moles
Explanation: Convert pressure from torr to atm:
598 torr ÷ 760 torr/atm = 0.789 atm
Convert temperature from Celsius to Kelvin:
139.2°C + 273.15 = 412.35 K
Use the ideal gas law equation to calculate the number of moles of gas:
PV = nRT
n = (PV) / (RT)
where P = 0.789 atm, V is the volume of the container (unknown), R = 0.0821 Latm/molK (the ideal gas constant), and T = 412.35 K
n = (0.789 atm * V) / (0.0821 Latm/molK * 412.35 K)
If we assume the container has a volume of 1 liter, we can solve for n:
n = (0.789 atm * 1 L) / (0.0821 Latm/molK * 412.35 K)
n = 0.0238 mol
Therefore, if the container has a volume of 1 liter, there are 0.0238 moles of gas in the container at a pressure of 598 torr and a temperature of 139.2°C.