Browse by Stream
QnA
Home
QnA
Go To Your Study Dashboard

Get Answers to all your Questions

header-bg qa
  • Home
  • Engineering
  • Help me solve this 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 )

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)

best_answer

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.

Posted by

prateek

View full answer

JEE Main high-scoring chapters and topics

Study 40% syllabus and score up to 100% marks in JEE

Similar Questions

Trending Articles/News

anam-khan

JEE Main 2024 Topper: Farmer’s son Gajare Nilkrishna says ‘keep questioning until you understand’
anam-khan

NIT Puducherry Cut-off 2024: Computer Science and Engineering had highest closing rank last year
anam-khan

What after JEE Main results 2024? All you need to know about JEE Adv, CSAB, JoSAA counselling

Latest Question