If $10^{-4} \ dm^3$ of water is introduced into a $1.0 \ dm^3$ flask at $300 \ K,$ how many moles of water are in the vapour phase when equilibrium is established? (Given: Vapour pressure of $H_2O$ at $300 \ K$ is $3170 \ Pa;$ $R = 8.314 \ J \ K^{-1} \ mol^{-1}$)
- A$5.56 \times 10^{-3} \ mol$
- B$1.53 \times 10^{-2} \ mol$
- C$4.46 \times 10^{-2} \ mol$
- D$1.27 \times 10^{-3} \ mol$
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