When the temperature of a rigid hollow sphere containing 685 L of helium gas is held at 621 K, the pressure of the gas is 1.89 x 10^3 kPa. How many moles of the helium does the sphere contain? Please explain how you got the answer.
You have to use the equation PV=nRT. P=pressure (in this case 1.89x10^3 kPa which equals 18.35677 atm) 1V=volume (in this case 685L) n=moles (in this case the unknown) R=gas constant (0.08206 (L atm)/(mol K)) T=temperature (in this case 621 K) with the given information you can rewrite the ideal gas law equation as n=PV/RT. n=(18.35677atm x 685L)/(0.08206atmL/molK x 621K) n=246.8 moles
