How to calculate the anhydrous ammonia, from Kg to normal cubic metre in the gas state?

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How to calculate the anhydrous ammonia, from Kg to normal cubic metre in the gas state?

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Answer 1 · 2018-01-23T17:44:59

Presumably, you use the Ideal Gas Law....

Explanation:

Ammonia is a room temperature gas...and while its behaviour substantially departs from ideality, we may use the old Ideal Gas equation...

And we could specify a volume of $1 \cdot m^{3}$ $1*m^3$ , a pressure of $1 \cdot a t m$ $1*atm$ , and a temperature of $298 \cdot K$ $298*K$ ...

$n = \frac{P V}{R T} = \frac{1 \cdot a t m \times 1 \cdot m^{3} \times 1000 \cdot L \cdot m^{- 3}}{0.0821 \cdot \frac{L \cdot a t m}{K \cdot m o l} \times 298 \cdot K} = 40.9 \cdot m o l$ $n=(PV)/(RT)=(1*atmxx1*m^3xx1000*L*m^-3)/(0.0821*(L*atm)/(K*mol)xx298*K)=40.9*mol$ ...

And this represents a mass of $40.9 \cdot m o l \times 17.03 \cdot g \cdot m o l^{- 1} = 695 \cdot g$ $40.9*molxx17.03*g*mol^-1=695*g$

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How to calculate the anhydrous ammonia, from Kg to normal cubic metre in the gas state?

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