The number of moles of the Helium gas at STP and RTP are 0.0197mol and 0.018mol respectively.
What is Ideal Gas Law?
The Ideal gas law or general gas equation emphasizes on the state or behavior of a hypothetical ideal gas. It states that "the pressure multiplied by volume is equal to moles multiply by the universal gas constant multiply by temperature.
It is expressed as;
PV = nRT
Where P is pressure, V is volume, n is the amount of substance, T is temperature and R is the ideal gas constant ( 0.08206 Latm/molK )
Given that;
- Volume of the Helium gas V = 440.8 mL = (440.8/1000)L = 0.4408L
At STP
- Temperature T = 273.15K
- Pressure P = 1.0atm
At RTP
- Temperature T = 298.15K
- Pressure P = 1.0atm
The number of moles at standard temperature and pressure STP
PV = nRT
n = PV / RT
n = ( 1.0atm × 0.4408L ) / ( 0.08206Latm/molK × 273.15K )
n = ( 0.4408Latm ) / ( 22.41Latm/mol )
n = 0.0197mol
Therefore, at standard temperature and pressure STP, the number of moles of the Helium gas is 0.0197mol.
The number of moles at room temperature and pressure RTP
PV = nRT
n = PV / RT
n = ( 1.0atm × 0.4408L ) / ( 0.08206Latm/molK × 298.15K)
n = ( 0.4408Latm ) / ( 24.466Latm/mol )
n = 0.018mol
Therefore, at room temperature and pressure RTP, the number of moles of the Helium gas is 0.018mol.
The number of moles of the Helium gas at STP and RTP are 0.0197mol and 0.018mol respectively.
Learn more about Ideal Gas Law here: brainly.com/question/4147359
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