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A Helium gas in a tube with a volume of 9.583 L under pressure of 4.972 atm at 31.8 c
How many moles of Helium gas is in the tube

1.9 mol
0.019 mol
18.24 mol
0.525 mol

Sagot :

1.905 moles of Helium gas are in the tube. Hence, option A is correct.

What is an ideal gas equation?

The ideal gas law (PV = nRT) relates the macroscopic properties of ideal gases. An ideal gas is a gas in which the particles (a) do not attract or repel one another and (b) take up no space (have no volume).

Calculate the moles of the gas using the gas law,

PV=nRT, where n is the moles and R is the gas constant. Then divide the given mass by the number of moles to get molar mass.

Given data:

P= 4.972 atm

V= 9.583 L

n=?

R= [tex]0.082057338 \;L \;atm \;K^{-1}mol^{-1}[/tex]

T=31.8 +273= 304.8 K

Putting value in the given equation:

[tex]\frac{PV}{RT}[/tex]=n

n= [tex]\frac{4.972 \;atm\; X \;9.583 \;L}{0.082057338 \;L \;atm \;K^{-1}mol^{-1} X 304.8}[/tex]

Moles = 1.905 moles

1.905 moles of Helium gas are in the tube. Hence, option A is correct.

Learn more about the ideal gas here:

https://brainly.com/question/27691721

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