Chemistry: What mass of neon gas is required to fill a 5.00-L container to a pressure of 1.02 atm at 25 °C?

Depends how many pickles you would like on a sandwich (sorry had to)...

What mass of neon gas is required to fill a 5.00-L

krystalhurst97

02.02.2022

m=4.21g

Explanation:

Hello,

In this case, by using the ideal gas equation:

PV=nRT

We can compute the mass of neon gas at the given conditions by firstly computing the moles and also considering the temperature in kelvins (298K):

$n=\frac{PV}{RT}=\frac{1.02atm*5.00L}{0.082\frac{atm*L}{mol*K}*298K}\\ \\n=0.209mol$

Finally, by using the atomic mass of neon gas (20.18g/mol) we compute the required mass to fill the 5.00-L container:

$m=0.209mol*\frac{20.18g}{1mol}\\ \\m=4.21g$

Best regards.

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