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

P_{f} is final pressure of the mixture

V_{f} is Final volume of the mixture

P_{1} = Initial pressure of gas No. 1 before mixing

V_{1} = Initial volume of gas No. 1 before mixing

P_{2} = Initial pressure of gas No. 2 before mixing

V_{2} = Initial volume of gas No. 2 before mixing

The 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 g

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

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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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