# Chemical Forums

• February 21, 2019, 07:32:59 AM
• Welcome, Guest

•

Pages: [1]   Go Down

### AuthorTopic: Partial pressure problem..  (Read 3945 times) !function(d,s,id){var js,fjs=d.getElementsByTagName(s)[0];if(!d.getElementById(id)){js=d.createElement(s);js.id=id;js.src="https://platform.twitter.com/widgets.js";fjs.parentNode.insertBefore(js,fjs);}}(document,"script","twitter-wjs"); (function() {var po = document.createElement("script"); po.type = "text/javascript"; po.async = true;po.src = "https://apis.google.com/js/plusone.js";var s = document.getElementsByTagName("script")[0]; s.parentNode.insertBefore(po, s);})();

0 Members and 1 Guest are viewing this topic.

#### petstar21

• Regular Member
• Mole Snacks: +0/-0
• Offline
• Gender:
• Posts: 26
• Dogs rule
##### Partial pressure problem..
« on: October 24, 2009, 01:37:23 PM »

NO reacts with molecular oxygen:
2 NO(g) + O2(g)  2 NO2(g)

Initially NO and O2 are separated as shown below. When the valve is opened, the reaction quickly goes to completion. Determine what gases remain at the end and calculate their partial pressures. Assume that the temperature remains constant at 25°C.

*NO is at 4L at .5atm
*O2 is at 2L and 1 atm

How do I get the partial press. of NO?
thanks

PNO
??
PO2
.1663 atm
PNO2
.3331

Logged

#### Dan

• Retired Staff
• Sr. Member
• Mole Snacks: +467/-72
• Offline
• Gender:
• Posts: 4716
• Organic Chemist
##### Re: Partial pressure problem..
« Reply #1 on: October 26, 2009, 01:32:33 AM »

I think you need to calculate the total pressure of the system (after the valve is opened), then use Dalton's law to calculate the unknown partial pressure.
Logged
My research: Google Scholar and Researchgate

Pages: [1]   Go Up

Mitch Andre Garcia's Chemical Forums 2003-Present.

Page created in 0.07 seconds with 23 queries.