Unformatted text preview: o C), its internal pressure is 1.06 atm. Determine the number of moles of helium in the balloon, and the mass of helium needed to inflate the balloon to these values. Solution: We find the number of moles of helium in the balloon from the ideal gas equation. PV = nRT → n = PV/RT n =( (1.06atm)*(1.013E5Pa)*((4/3)* π *(.22m)^3))/((8.314J/mol*K)*293K) = 1.97mol 1.97mol*(4g/1mol H 2 ) = 7.86g...
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This note was uploaded on 11/19/2010 for the course LECTURE 1 taught by Professor Yildiz during the Fall '10 term at Berkeley.
- Fall '10