Turn on thread page Beta
    • Thread Starter
    Offline

    8
    ReputationRep:
    i don't understand how to do this question

    A 5.0 L container is filled with 8.8 g of CO(g) and 2.00 g of H2(g). The temperature is 47 oC. Calculate the partial pressure of H2 and the total pressure of the gas mixture.
    • Community Assistant
    • Study Helper
    Offline

    17
    ReputationRep:
    Community Assistant
    Study Helper
    (Original post by qatarownz)
    i don't understand how to do this question

    A 5.0 L container is filled with 8.8 g of CO(g) and 2.00 g of H2(g). The temperature is 47 oC. Calculate the partial pressure of H2 and the total pressure of the gas mixture.
    Do you know the definition of partial pressure?
    • Thread Starter
    Offline

    8
    ReputationRep:
    (Original post by charco)
    Do you know the definition of partial pressure?
    it means the total pressure when summed together
    Offline

    1
    ReputationRep:
    (Original post by qatarownz)
    i don't understand how to do this question

    A 5.0 L container is filled with 8.8 g of CO(g) and 2.00 g of H2(g). The temperature is 47 oC. Calculate the partial pressure of H2 and the total pressure of the gas mixture.
    By using this law .. You have the volume , mass and temrature . find number of moles from the mass then you can culculate partial pressure .
    The total pressure is the sum of partial pressure of gases in mixture .
    Name:  Capture+_2016-11-12-09-25-56.png
Views: 157
Size:  76.4 KB
    • Thread Starter
    Offline

    8
    ReputationRep:
    this what I got



    Moles of CO= 8.8 g/28.008 g/mol= 0.314
    Moles of H2= 2 g/2.0156 g/mol= 0.992

    P(CO)= nRT/V = [(0.314)(0.08206)(47+273.15)]/5.0= 1.65 atm

    P(H2)= nRT/V = [(0.992)(0.08206)(47+273.15)]/5.0= 5.21 atm

    Partial Pressure of H2 = 0.992/(0.314+ 0.992) = 0.76

    0.76*5.21 = 3.96 atm

    Pressure Total = 1.65 + 5.21 = 6.86 atm








    Offline

    1
    ReputationRep:
    (Original post by qatarownz)
    this what I got


    [/color][/font]
    [/color][/color]
    [/color][/color]
    [/color][/font]
    [/color][/color]
    [/color][/font]
    [/color][/color]
    [/color][/font]
    [/color][/color]
    [/color][/font]
    [/color][/color]
    [/color][/font]
    [/color][/color]
    [/color][/font]






    I think its correct
    • Community Assistant
    • Study Helper
    Offline

    17
    ReputationRep:
    Community Assistant
    Study Helper
    (Original post by qatarownz)
    this what I got
    A 5.0 L container is filled with 8.8 g of CO(g) and 2.00 g of H2(g). The temperature is 47ºC. Calculate the partial pressure of H2 and the total pressure of the gas mixture.

    The partial pressure of a gas is the pressure that it would exert if it were on its own.
    It can be calculated by the mole fraction x the total pressure.

    So deal with each gas on its own:

    CO(g) 8.8g = 8.8/28 mol = 0.314

    P = nRT/V = 0.314 x 8.314 x 320/5 = 167.2 kPa

    H2(g, 2g = 2/2 mol = 1 mol

    P = nRT/V =1 x 8.314 x 320/5 = 532.1 kPa

    Total pressure = 699.3 kPa

    If you want the answer in atmospheres divide by 101.3 = 6.90 atm


    You are correct (the slight difference results from my use of rounded Mr values)
 
 
 
Reply
Submit reply
Turn on thread page Beta
Updated: November 12, 2016
The home of Results and Clearing

3,702

people online now

1,567,000

students helped last year

University open days

  1. Bournemouth University
    Clearing Open Day Undergraduate
    Fri, 17 Aug '18
  2. University of Bolton
    Undergraduate Open Day Undergraduate
    Fri, 17 Aug '18
  3. Bishop Grosseteste University
    All Courses Undergraduate
    Fri, 17 Aug '18
Poll
A-level students - how do you feel about your results?

The Student Room, Get Revising and Marked by Teachers are trading names of The Student Room Group Ltd.

Register Number: 04666380 (England and Wales), VAT No. 806 8067 22 Registered Office: International House, Queens Road, Brighton, BN1 3XE

Write a reply...
Reply
Hide
Reputation gems: You get these gems as you gain rep from other members for making good contributions and giving helpful advice.