pretty sure its a simple problem, but for some reason im lost on it...
i dont understand Qvault's explanation, so if anyone can help with their own explanation itd be great

6 moles of nitrogen and an unknown amount of hydrogen are held at 40atm. The partial pressure exerted by the nitrogen is 24atm. How many moles of hydrogen are present?

also, has anyone heard of this - · For a gas, the equilibrium expression is written in terms of pressure, not concentration.
.N.2(.g..).+.3..H2(.g..)...↽.−.−.⇀.2..NH3(.g..).. --- Keq =.(..P..NH3.)2 ./ ..(.(.P.H2)3(.P.N2).).
I had selected [Nh3]^2 / [H2]^3[N2] like ive always seen and i think theres an exact same problem with the Haber Process in the Destroyer too, but i never saw the "P" in the Keq before

whats Pn2?....pressure of N2?
so then 24 = (6/6+x)(40) which leads to x = 4 right? nice bc thats the answer...so that was just the partial pressure formula right? partial pressure = mole fraction/mole total)(total pressure)?

idk whats with these mole fraction/partial pressure problems thats giving me trouble when they used to be so easy...heres another one if you or anyone can please help:

The solubility of dissolved oxygen in water is 1.25 x 10-4 M at 25°C, where the mole fraction of oxygen is 0.21 and atmospheric pressure is 1.0 atm. In a pure oxygen atmosphere at the same pressure, what would the solubility be?

pretty sure its a simple problem, but for some reason im lost on it...
i dont understand Qvault's explanation, so if anyone can help with their own explanation itd be great

6 moles of nitrogen and an unknown amount of hydrogen are held at 40atm. The partial pressure exerted by the nitrogen is 24atm. How many moles of hydrogen are present?

also, has anyone heard of this - · For a gas, the equilibrium expression is written in terms of pressure, not concentration.
.N.2(.g..).+.3..H2(.g..)...↽.−.−.⇀.2..NH3(.g..).. --- Keq =.(..P..NH3.)2 ./ ..(.(.P.H2)3(.P.N2).).
I had selected [Nh3]^2 / [H2]^3[N2] like ive always seen and i think theres an exact same problem with the Haber Process in the Destroyer too, but i never saw the "P" in the Keq before

Yes equilibrium constant for a gas can also be written in terms of their partial pressure. If you watch chad's videos you will see this.
PN2= partial pressure of N2 and so on.

The solubility of dissolved oxygen in water is 1.25 x 10-4 M at 25°C, where the mole fraction of oxygen is 0.21 and atmospheric pressure is 1.0 atm. In a pure oxygen atmosphere at the same pressure, what would the solubility be?

Yes equilibrium constant for a gas can also be written in terms of their partial pressure. If you watch chad's videos you will see this.
PN2= partial pressure of N2 and so on.

The solubility of dissolved oxygen in water is 1.25 x 10-4 M at 25°C, where the mole fraction of oxygen is 0.21 and atmospheric pressure is 1.0 atm. In a pure oxygen atmosphere at the same pressure, what would the solubility be?

i gotta look into the previous problem still, but thanks for the responses... any help with this one..idk why im having trouble with these when partial pressure used to be the easiest calculation lol:
When it is bottled, the partial pressure of [FONT=MathJax_Main]CO.[FONT=MathJax_Main]2. over a 1 L bottle of soda is 4.0 atm. The concentration of dissolved [FONT=MathJax_Main]CO.[FONT=MathJax_Main]2. is 0.12M. The soda is opened at left at 1.0 atm. What will be the new concentration of dissolved [FONT=MathJax_Main]CO.[FONT=MathJax_Main]2. ?

i gotta look into the previous problem still, but thanks for the responses... any help with this one..idk why im having trouble with these when partial pressure used to be the easiest calculation lol:
When it is bottled, the partial pressure of [FONT=MathJax_Main]CO.[FONT=MathJax_Main]2. over a 1 L bottle of soda is 4.0 atm. The concentration of dissolved [FONT=MathJax_Main]CO.[FONT=MathJax_Main]2. is 0.12M. The soda is opened at left at 1.0 atm. What will be the new concentration of dissolved [FONT=MathJax_Main]CO.[FONT=MathJax_Main]2. ?

That's all they give you? Is the final 1.0 atm the pressure of the the vapor pressure of CO2, or is it the total vapor pressure of the solution? Do they give you a molecular formula for what "soda" is?

If they gave the molecular formula for soda in this problem, it would be easy since you can figure out the mole fraction and go from there. Since they don't give it to you, I don't know how to convert 1L = 1000g = ? moles. Otherwise, I'm also unsure of how to do this problem with the information you gave. All I know is, solubility of CO2 in soda decreases because the pressure above the solution drops.

BUMPPPPPPPPPPPPPPPPPPPPPPPPPPPP

Also, can you please give us an answer to the first problem so we know what's going on?

That's all they give you? Is the final 1.0 atm the pressure of the the vapor pressure of CO2, or is it the total vapor pressure of the solution? Do they give you a molecular formula for what "soda" is?

If they gave the molecular formula for soda in this problem, it would be easy since you can figure out the mole fraction and go from there. Since they don't give it to you, I don't know how to convert 1L = 1000g = ? moles. Otherwise, I'm also unsure of how to do this problem with the information you gave. All I know is, solubility of CO2 in soda decreases because the pressure above the solution drops.

BUMPPPPPPPPPPPPPPPPPPPPPPPPPPPP

Also, can you please give us an answer to the first problem so we know what's going on?

sorry...the very first problem? yeah the answer was 4...i havent got a chance to look at the others yet...im going to look back at them when i review them

When it is bottled, the partial pressure of CO2 over a 1 L bottle of soda is 4.0 atm. The concentration of dissolved CO2 is 0.12M. The soda is opened at left at 1.0 atm. What will be the new concentration of dissolved CO2 ?

I'm taking my DAT soon and I would like to know what the answer is and how to do it, lol.

When it is bottled, the partial pressure of CO2 over a 1 L bottle of soda is 4.0 atm. The concentration of dissolved CO2 is 0.12M. The soda is opened at left at 1.0 atm. What will be the new concentration of dissolved CO2 ?

I'm taking my DAT soon and I would like to know what the answer is and how to do it, lol.

i just logged into qvault to check back at these problems but apparently their server has been down since yesterday!! wtf! i have a schedule to keep to...ill let u know once i can get in

wow i think youre rite... (4atm)(.12M)=(1atm)(M2) ? but then wouldnt M2 be 0.48M which doesnt seem to make sense that theres more CO2 in it if cap is left open (even though P down = M up)..? or am i setting it up incorrectly? lol

are maybe the numbers used just poor choices bc they dont make sense in that gas solubility would go UP with INCREASED pressure and vice versa??

wow i think youre rite... (4atm)(.12M)=(1atm)(M2) ? but then wouldnt M2 be 0.48M which doesnt seem to make sense that theres more CO2 in it if cap is left open (even though P down = M up)..? or am i setting it up incorrectly? lol

are maybe the numbers used just poor choices bc they dont make sense in that gas solubility would go UP with INCREASED pressure and vice versa??

It would be (4atm / 1 atm) = (0.12M / M2).
You are comparing the RATIO of partial pressure with the RATIO of concentration.
The ratio between the two should be equal.

It would be (4atm / 1 atm) = (0.12M / M2).
You are comparing the RATIO of partial pressure with the RATIO of concentration.
The ratio between the two should be equal.

o yup youre right...and just verified by finding out on qvault..im not sure if i ever saw a Molarity to Pressure setup before...where have you seen these problems?

The partial pressure over a dissolved gas is proportional to the concentration of that gas in solution. This is Henry's Law.

[FONT=MathJax_Main]Concentration.[FONT=MathJax_Main]=.[FONT=MathJax_Main](.[FONT=MathJax_Main]0.12.[FONT=MathJax_Main] M.[FONT=MathJax_Main]).[FONT=MathJax_Main](.[FONT=MathJax_Main]1.0.[FONT=MathJax_Main] atm.[FONT=MathJax_Main]).[FONT=MathJax_Main]4.0.[FONT=MathJax_Main] atm.[FONT=MathJax_Main]=.[FONT=MathJax_Main]0.03.[FONT=MathJax_Main] M

.

[FONT=MathJax_Main] anything for this one?. The solubility of dissolved oxygen in water is 1.25 x 10-4 M at 25°C, where the mole fraction of oxygen is 0.21 and atmospheric pressure is 1.0 atm. In a pure oxygen atmosphere at the same pressure, what would the solubility be?

I just figured 100/21 = 4.76 and multiplied that by (1.25 x 10^-4) = 6 x 10^-4 but i dont know if i had the correct thinking on this? They have the answer in setup form as (1.25 x 10^-4) / 0.21 ...and both equal approximately 6x10^-4

I guess its similar to the above problem? ratio would be Mole fraction 1 / Mole fraction 2 = Concentration 1 / Concentration 2? so 0.21/1 = (1.25x10^-4)/C2

o yup youre right...and just verified by finding out on qvault..im not sure if i ever saw a Molarity to Pressure setup before...where have you seen these problems?

The partial pressure over a dissolved gas is proportional to the concentration of that gas in solution. This is Henry's Law.

[FONT=MathJax_Main]Concentration.[FONT=MathJax_Main]=.[FONT=MathJax_Main](.[FONT=MathJax_Main]0.12.[FONT=MathJax_Main] M.[FONT=MathJax_Main]).[FONT=MathJax_Main](.[FONT=MathJax_Main]1.0.[FONT=MathJax_Main] atm.[FONT=MathJax_Main]).[FONT=MathJax_Main]4.0.[FONT=MathJax_Main] atm.[FONT=MathJax_Main]=.[FONT=MathJax_Main]0.03.[FONT=MathJax_Main] M

.

[FONT=MathJax_Main] anything for this one?. The solubility of dissolved oxygen in water is 1.25 x 10-4 M at 25°C, where the mole fraction of oxygen is 0.21 and atmospheric pressure is 1.0 atm. In a pure oxygen atmosphere at the same pressure, what would the solubility be?

I just figured 100/21 = 4.76 and multiplied that by (1.25 x 10^-4) = 6 x 10^-4 but i dont know if i had the correct thinking on this? They have the answer in setup form as (1.25 x 10^-4) / 0.21 ...and both equal approximately 6x10^-4

I guess its similar to the above problem? ratio would be Mole fraction 1 / Mole fraction 2 = Concentration 1 / Concentration 2? so 0.21/1 = (1.25x10^-4)/C2

o yup youre right...and just verified by finding out on qvault..im not sure if i ever saw a Molarity to Pressure setup before...where have you seen these problems?

The partial pressure over a dissolved gas is proportional to the concentration of that gas in solution. This is Henry's Law.

[FONT=MathJax_Main]Concentration.[FONT=MathJax_Main]=.[FONT=MathJax_Main](.[FONT=MathJax_Main]0.12.[FONT=MathJax_Main] M.[FONT=MathJax_Main]).[FONT=MathJax_Main](.[FONT=MathJax_Main]1.0.[FONT=MathJax_Main] atm.[FONT=MathJax_Main]).[FONT=MathJax_Main]4.0.[FONT=MathJax_Main] atm.[FONT=MathJax_Main]=.[FONT=MathJax_Main]0.03.[FONT=MathJax_Main] M

.

[FONT=MathJax_Main] anything for this one?. The solubility of dissolved oxygen in water is 1.25 x 10-4 M at 25°C, where the mole fraction of oxygen is 0.21 and atmospheric pressure is 1.0 atm. In a pure oxygen atmosphere at the same pressure, what would the solubility be?

I just figured 100/21 = 4.76 and multiplied that by (1.25 x 10^-4) = 6 x 10^-4 but i dont know if i had the correct thinking on this? They have the answer in setup form as (1.25 x 10^-4) / 0.21 ...and both equal approximately 6x10^-4

I guess its similar to the above problem? ratio would be Mole fraction 1 / Mole fraction 2 = Concentration 1 / Concentration 2? so 0.21/1 = (1.25x10^-4)/C2

wow i think youre rite... (4atm)(.12M)=(1atm)(M2) ? but then wouldnt M2 be 0.48M which doesnt seem to make sense that theres more CO2 in it if cap is left open (even though P down = M up)..? or am i setting it up incorrectly? lol

are maybe the numbers used just poor choices bc they dont make sense in that gas solubility would go UP with INCREASED pressure and vice versa??

When I first read the question I also thought of the problem as a simple proportion problem and set up my proportion exactly like you did but I realize that

Pv=nRT

and since p and v is on the same side then you must keep both volume and pressure on the same side.

in contrast to M1V1=M2V2

molarity(moles/L) is on the opposite side of volume in Pv=nrt so that is why it is written like that