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Chemistry Forums for Students => Physical Chemistry Forum => Topic started by: valenceshell on September 27, 2016, 09:48:09 PM

Title: Ideal Gas Law
Post by: valenceshell on September 27, 2016, 09:48:09 PM

I'm having some trouble with this question: 15.00g of N2(g) are mixed with 5.00g of O2(g) at 30.0C and 100kPa. Assuming ideal behavior, what are the partial pressures of N2(g) and O2(g)? What is the volume of the mixture?

I know I can use the ideal gas law with P(N2)=nRT/V but I'm not given a volume to substitute. Do I just assume a volume of 1L?

For calculating the volume of the mixture, I used Vm=V/n and got 13.51L for N2 and 3.93L for O2. Would a final volume of 17.44L be correct?

Secondly, I have no idea how to go about answering this question: 1.00g CO(g) react with 1.00g O2(g) to form CO2(g) in a closed container. What is the mole fraction of CO2(g) when the reaction has gone to completion?

Title: Re: Ideal Gas Law
Post by: Borek on September 28, 2016, 02:47:47 AM

Do you know Dalton's law of partial pressures? Avogadro's hypothesis?