In which one of the following, does the given amount of chlorine exert the least pressure in a vessel of capacity $1 d m^{3}$ at $273 K$ ?

0.0355

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0.071

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6.023 \times 10^{21}

molecules

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0.02

mol

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Solution

The correct option is A $0.0355$ g
The ideal gas equation is:

$P V = n R T$

When $V$ and $T$ are the same,

$P \propto n$

Thus, when the number of moles, i.e., $n$ is least, it will exert the least pressure.

(a) $n = \frac{w t}{m o l . w t} = \frac{0.0355}{35.5} = 1 \times 10^{- 3} m o l$

(b) $n = \frac{0.071}{35.5} = 2 \times 10^{- 3} m o l$

(c) $n = \frac{n u m b e r o f m o l e c u l e s}{N_{A}}$

$= \frac{6.023 \times 10^{21}}{6.023 \times 10^{23}} = 0.01$ mol

(d) $n = 0.02$ mol

Thus, $0.0355$ g chlorine will exert the least pressure.

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In which one of the following, does the given amount of chlorine exert the least pressure in a vessel of capacity 1 dm3 at 273 K?

In which one of the following, does the given amount of chlorine exert the least pressure in a vessel of capacity $1 d m^{3}$ at $273 K$ ?