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Angelina_Jolie [31]
2 years ago
5

The gaseous product of a reaction is collected in a 25.0L container at 27.0 C. The pressure in the container is 3.0atm and the g

as has a mass of 96.0g. What is the molar mass of the gas?
Chemistry
1 answer:
NeX [460]2 years ago
4 0

Answer: The molar mass of the gas is 31.6 g/mol

Explanation:

According to ideal gas equation:

PV=nRT

P = pressure of gas = 3.0 atm

V = Volume of gas = 25.0 L

n = number of moles  = ?

R = gas constant =0.0821Latm/Kmol

T =temperature =27.0^0C=(27.0+273)K=300K

n=\frac{PV}{RT}

n=\frac{3.0atm\times 25.0L}{0.0821 L atm/K mol\times 300K}=3.04moles

Moles =\frac{\text {given mass}}{\text {Molar mass}}

3.04=\frac{96.0g}{\text {Molar mass}}

{\text {Molar mass}}=31.6g/mol

The molar mass of the gas is 31.6 g/mol

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Answer:

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Explanation:

The mole fraction of BaCl₂ (X) is calculated as follows:

X = moles BaCl₂/total moles of solution

Given:

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We have to convert the mass of water to moles, by using the molecular weight of water (Mw):

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moles of water = mass of water/Mw of water = 850.0 g/(18 g/mol) = 47.2 mol

The total moles of the solution is given by the addition of the moles of solute (BaCl₂) and the moles of solvent (water):

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X = 0.400 mol/47.6 mol = 0.0084

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