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vampirchik [111]
3 years ago
5

A sample of an unknown compound is vaporized at 150.°C . The gas produced has a volume of 960.mL at a pressure of 1.00atm , and

it weighs 0.941g . Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound.
Chemistry
1 answer:
IrinaK [193]3 years ago
6 0

Answer:

34.02 g.

Explanation:

Hello!

In this case, since the gas behaves ideally, we can use the following equation to compute the moles at the specified conditions:

PV=nRT\\\\n=\frac{1.00atm*0.960L}{0.08206\frac{atm*L}{mol*K}*(150+273)K} =0.0277mol\\\\

Now, since the molar mass of a compound is computed by dividing the mass over mass, we obtain the following molar mass:

MM=\frac{0.941g}{0.0277mol} \\\\MM=34.02g/mol

So probably, the gas may be H₂S.

Best regards!

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3 Ca²⁺(aq) + 2 PO₄³⁻(aq) ⇄ Ca₃(PO₄)₂(s)

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