If 10-4 dm3 of water is introduced into a flask at 300 K, how many moles of water are in the vapour phase when equilibrium is established?

( Given : Vapour pressure of H2O at 300 K is 3170 Pa ;R =  8.314  JK-1 mol-1 )

  • Option 1)

    1.27 × 10-3 mol

  • Option 2)

    5.56 × 10-3 mol

  • Option 3)

    1.5 × 10-2 mol

  • Option 4)

    4.46 × 10-2 mol

 

Answers (1)

As we learnt in

Ideal Gas Law -

PV=nRT

- wherein

P - Pressure

V - Volume

n - No. of Moles

R - Gas Constant

T - Temperature

 

 PV = nRT

3170\times 10^{-4}=n\times 8.314\times 300

n=\frac{0.3170}{8.314\times 300}=1.27\times 10^{-4}

Corrrect option is 1.

 


Option 1)

1.27 × 10-3 mol

This is the correct option.

Option 2)

5.56 × 10-3 mol

This is an incorrect option.

Option 3)

1.5 × 10-2 mol

This is an incorrect option.

Option 4)

4.46 × 10-2 mol

This is an incorrect option.

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