Given
Volume = 15.9 L
Temperature = 27.1 °C = (27.1+273.15) K = 300.25 K
Pressure = 2.20 atm
Using ideal gas equation
PV = nRT
R is universal gas constant = 0.08206 L atm/mol K
n is the no of moles
So
n = PV/RT
= (2.20 atm * 15.9L)/(0.08206 L atm/mol K * 300.25 K)
= 1.42 moles
1.42 moles of gas are contained inside the balloon
penalty 04 Question (4 points) See page 289 A balloon is filled to a volume of...
A balloon is filled to a volume of 20.7L at a temperature of 27.1ºC. If the pressure in the balloon is measured to be 2.20 atm, how many moles of gas are contained inside the balloon? Could you please solve this using the Ideal gas equation?
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