[kryssxxo]

Hi,
I'm new with Chemistry and I'm trying to teach it to myself before I have a big exam on it next week. I'm writing the Health Occupants Aptitude Exam in order to enter the Veterinary Technician program, and to do so I need a high score in Chemistry.
There is a few questions stumping me, but the biggest one is
"A mixture consisting of 8.0g of Oxygen and 14g of Nitrogen is prepared in a container such that the total pressure is 750 mm Hg. The partial pressure of Oxygen in the mixture is...?"
Please break this down for me as simply as possible. I'm not even good with Moles lol.. thanks.

[billnotgatez]

We like to help here but we operate by rules
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I assume you have a book to assist you, so maybe you can let us know what you know from the book  about gas laws so we can fill in the gaps.
By the way, understanding the Mole concepts is important to more than this question.

[kryssxxo]

We like to help here but we operate by rules
You have to show your attempts or thoughts at solving the question to receive help.
This is a forum policy.
Click on the link near the top center of the forum page.
Forum Rules: Read This Before Posting.

I assume you have a book to assist you, so maybe you can let us know what you know from the book  about gas laws so we can fill in the gaps.
By the way, understanding the Mole concepts is important to more than this question.

That's the thing.. I don't know where to start.. My prep book just tells me the definition of Partial Pressure and the formula Pt= P1 + P2 + P3 but this formula didn't work for me and the number of quantities I'm given.
I tried P1 + P2 which I thought was 60 + 105 but I was wrong.
I know the answer is 250 mm Hg, I just don't know how to go about getting there.

[billnotgatez]

Does your prep book have any discussion around the concept of
Partial pressure of each gas is proportional to its mole fraction in the mixture.