How many grams of fluorine gas will exert a pressure of 134 atm in a 3.2-liter container at 40°C?

Question

How many grams of fluorine gas will exert a pressure of 134 atm in a 3.2-liter container at 40°C?

1 Answer

Impact of this question

1702 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2017-05-11T21:23:42

It will have to be a stout container.

Explanation:

We use the Ideal Gas equation:

$Mass = \frac{P V}{R T} \times 38.00 \cdot g \cdot m o l^{- 1}$ $"Mass"=(PV)/(RT)xx38.00*g*mol^-1$

$= \frac{134 \cdot a t m \times 3.2 \cdot L}{0.0821 \cdot \frac{L \cdot a t m}{K \cdot m o l} \times 313 \cdot K} = 16.7 \cdot m o l \times 38.00 \cdot g \cdot m o l^{- 1} = 635 \cdot g$ $=(134*atmxx3.2*L)/(0.0821*(L*atm)/(K*mol)xx313*K)=16.7*molxx38.00*g*mol^-1=635*g$

Why did I use $38.00 \cdot g \cdot m o l^{- 1}$ $38.00*g*mol^-1$ for fluorine gas and not $19.00 \cdot g \cdot m o l^{- 1}$ $19.00*g*mol^-1$ ?

Science

Math

Humanities

... and beyond

How many grams of fluorine gas will exert a pressure of 134 atm in a 3.2-liter container at 40°C?

1 Answer

Explanation:

Related questions

Impact of this question