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Dalton's Law of Partial Pressures

A cylinder co...

Question

A cylinder contain hydrogen gas at pressure of $249 k P a$ and temperature $2 7^{o}$ C its density is:
$(R = 8.3 J m o l^{- 1} k^{- 1})$

0.1 kg / m^{- 3}

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0.2 kg / m^{- 3}

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0.02 kg / m^{- 3}

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0.5 kg / m^{- 3}

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Solution

We can express, an ideal gas equation as,
$P M = d e n s i t y \times R T$
Given Data:
Temprature in kelvin will be, $= 27 + 273 = 300 K$
Molar mass of hydrogen, $= 2 \times 1 0^{- 3} k g$
Pressure, $= 249 k P a$
Gas constant, $(R = 8.3 J m o l^{- 1} k^{- 1})$
Step 1: Density of gas:
$P M = d e n s i t y \times R T$
$d e n s i t y = \frac{P M}{R T}$ $d e n s i t y = \frac{249 \times 10^{3} \times 2 \times 10^{- 3}}{8.3 \times 300} = 0.2 k g m^{- 3}$

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