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A mixture of 0.224 g of H2, 1.06 g of N2, and 0.834 g of Ar is stored in a closed container at STP. Find the volume (in L) of the container, assuming that the gases exhibit ideal behavior.

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Answer: The volume of given container is 3.83 L.

Step-by-step explanation:

Given: Mass of
H_(2) = 0.224 g

Mass of
N_(2) = 1.06 g

Mass of Ar = 0.834 g

Since, moles is the mass of a substance divided by its molar mass. Therefore, moles of given substances present in the mixture are as follows.

Moles of
H_(2) are:


Moles = (mass)/(molar mass)\\= (0.224 g)/(2 g/mol)\\= 0.112 mol

Moles of
N_(2) are:


Moles = (mass)/(molar mass)\\= (1.06 g)/(28 g/mol)\\= 0.038 mol

Moles of Ar are:


Moles = (mass)/(molar mass)\\= (0.834 g)/(40 g/mol)\\= 0.021 mol

Total moles = (0.112 + 0.038 + 0.021) mol = 0.171 mol

Now, using ideal gas equation the volume is calculated as follows.

PV = nRT

where,

P = pressure

V = volume

n = no. of moles

R = gas constant = 0.0821 L atm/mol K

T = temperature

Substitute the values into above formula as follows.


V = (nRT)/(P)\\= (0.171 mol * 0.0821 L atm/mol K * 273 K)/(1 atm)\\= 3.83 L

Thus, we can conclude that the volume of given container is 3.83 L.

User Alno
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