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Chemistry Question on States of matter

If 10−4 dm310^{-4}\, dm^3 of water is introduced into a 1.0 dm31.0\, dm^3 flask to 300 K300\, K, how many moles of water are in the vapour phase when equilibrium is established ? (Given : Vapour pressure of H2OH_2O at 300 K300\, K is 3170 Pa; R=8.314 J K−1 mol−13170\, Pa ;\, R = 8.314 \,J \,K^{-1}\, mol^{-1})

A

5.56×10−3 mol5.56 \times 10^{-3}\, mol

B

1.53×10−2 mol1.53 \times 10^{-2}\, mol

C

4.46×10−2 mol4.46 \times 10^{-2}\, mol

D

1.27×10−3 mol1.27 \times 10^{-3}\, mol

Answer

1.27×10−3 mol1.27 \times 10^{-3}\, mol

Explanation

Solution

n=PVRTn = \frac{PV}{RT} =128×10−5= 128 \times 10^{-5} moles =3170×10−5atm×1L0.0821L atm k−1 mol−1×300K≈1.27×10−3 mol= \frac{3170 \times 10^{-5} atm \times 1L}{0.0821L\, atm\, k^{-1}\, mol^{-1}\times 300K} \approx 1.27 \times 10^{-3} \,mol