Question

At 30°C , 500cm^3 of H_2 at 0.52 atm pressure and 1 dm^3 of N_2 at 0.78 atm pressure are transferred into a 1500 cm^3 flask. Calculate the total pressure of the mixture of gases

Answer 1

help! plzz!! ;(

Answer 2

Dalton's Law !!!

Answer 3

how to do this ? help plz!! ...why there are 3 volumes given ? :/

Answer 4

http://www.chm.davidson.edu/vce/gaslaws/daltonslaw.html

Answer 5

i know that

Answer 6

i cannot understand the question

Answer 7

i have solved numericals related to dalton's law but this one is confusing me

Answer 8

you would add both Poxygen + Pnitrogen = Ptotal I would assume

Answer 9

Find the pressure Hydrogen would have in the 1500[cm^3] volume

\[p_1V_1=p_2V_2\\p_2=p_1\frac{V_1}{V_2}\]

Answer 10

then why temperature and volumes are given ? there must be some reason

Answer 11

and similarly find the same for the nitrogen, then add these pressures together

Answer 12

Temperature is the same for both of the gases, so don't worry about it. You can find the moles of gas used from the pressures and volumes given

Answer 13

what is the V1 ....for hydrogen and nitrogen ?

Answer 14

You are given a final volume use that to figure out the new pressure of both gases

Answer 15

30 degrees C, 500cm^3 of H_2 at 0.52 atm -> use ideal gas law to find moles
30 degrees C, 1 dm^3 of N_2 at 0.78 atm -> use ideal gas law to find moles

Answer 16

so the 500 and 1 are useless ? ...the main volume is 1500 right ?

Answer 17

no they aren't useless you need that information to find the moles of the individual gases

Answer 18

okay first i have to find moles then ?

Answer 19

Yes of both gases

Then once you have the moles you can use the equations, posted here,

http://www.chm.davidson.edu/vce/gaslaws/daltonslaw.html

Then just add both pressures if I'm not mistaken

Answer 20

why are we finding moles for ?

Answer 21

because you need to find them to figure out the pressure of each gas in the final volume

Answer 22

oh!!

Answer 23

i am doing it !! wait

Answer 24

how to find moles ?

Answer 25

Just use PV = nRT

Answer 26

assuming it acts like an ideal gas

Answer 27

oh !! i did'nt thought of that !!!

Answer 28

thanks

Answer 29

H_2 = 0.0104 moles

Answer 30

just use that website I posted, and add the pressures, I could be wrong though I'm not great a physical chemistry

Answer 31

at*

Answer 32

These two gases aren't ideal, so you might want to look up how to calculate the moles of a non ideal gas

Answer 33

http://www.chm.davidson.edu/vce/gaslaws/daltonslaw.html

This resource will help I think

Answer 34

If this is just an intro chem course though you can just use PV = nRT to solve this, by making the assumption that these gases act like ideal gasses (monoatomic gasses)