How many grams of fluorine gas will exert a pressure of 1.54 atm in a 3.2-liter container at 40 °C?

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How many grams of fluorine gas will exert a pressure of 1.54 atm in a 3.2-liter container at 40 °C?

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Answer 1 · 2017-05-08T12:26:03

You MUST know that elemental fluorine is the gaseous $F_{2}$ $F_2$ molecule.

Explanation:

And in fact all the elemental gases, save for the Noble Gases, are bimolecular species. Is this true?

And we use the Ideal Gas Equation:

$P V = n R T = \frac{mass}{molar mass} \times R T$ $PV=nRT="mass"/"molar mass"xxRT$

And thus $mass = \frac{P V \times molar mass}{R T}$ $"mass"=(PVxx"molar mass")/(RT)$

And we plugs in the numbers:

$\frac{1.54 \cdot a t m \times 3.2 \cdot L \times 38.0 \cdot g \cdot m o l^{- 1}}{0.0821 \cdot \frac{L \cdot a t m}{K \cdot m o l} \times 313.1 \cdot K} =$ $(1.54*atmxx3.2*Lxx38.0*g*mol^-1)/(0.0821*(L*atm)/(K*mol)xx313.1*K)=$

$7.29 \cdot g$ $7.29*g$ .

Remember what I said with regard to the so-called molecularity of elemental gases. And fluorine gas, the most reactive substance on the Periodic Table, is not to be handled without special precautions.

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How many grams of fluorine gas will exert a pressure of 1.54 atm in a 3.2-liter container at 40 °C?

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