# Answer to Question #26111 in Inorganic Chemistry for salma

Question #26111

A flask contains 2.00 moles of nitrogen and 2.00 moles of helium. How many grams of argon must be pumped into the flask in order to make the partial pressure of argon twice that of helium?

Expert's answer

You can use the following law for solving this question:

P

P

V

P

V

P

V

The same with P

P is proportional to amount

at the beginning P

Adding some extra argon will cause decreasing

of nitrogen and helium pressure.

If you have 2.00 moles of nitrogen and 2.00 moles of helium and P is proportional to amount, the amount of argon that must be pumped into the flask in order to make the partial pressure of argon twice that of helium is twice amount of nitrogen. It is 4.00 mol

n = m/M

m = n*M

P

_{f}V_{f}= P_{1}V_{1}+ P_{2}V_{2}+ P_{3}V_{3}… etcP

_{f}is final pressure of the mixtureV

_{f}is Final volume of the mixtureP

_{1}= Initial pressure of gas No. 1 before mixingV

_{1}= Initial volume of gas No. 1 before mixingP

_{2}= Initial pressure of gas No. 2 before mixingV

_{2}= Initial volume of gas No. 2 before mixingThe same with P

_{3}and V_{3}P is proportional to amount

at the beginning P

_{1}V_{1}= P_{2}V_{2}(2.00 moles of nitrogen and 2.00 moles of helium)Adding some extra argon will cause decreasing

of nitrogen and helium pressure.

If you have 2.00 moles of nitrogen and 2.00 moles of helium and P is proportional to amount, the amount of argon that must be pumped into the flask in order to make the partial pressure of argon twice that of helium is twice amount of nitrogen. It is 4.00 mol

n = m/M

_{w};m = n*M

_{w}= 4.00*40 = 160 gNeed a fast expert's response?

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## Comments

Assignment Expert02.02.17, 21:53Dear visitor,

please use panel for submitting new questions

Cecilia31.01.17, 19:37Show that κ for the state equation P (Vm-b) = RT are given by

Κ =

1P

(

1

1 + bp / RT).

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