Well i have the total pressure of gases above water ( hydrogen and water vapor) which is 1.001 atm. I have the Partial pressure of water vapor which is 19.8 mm. How do i calculate the partial pressure of hydrogen? Thanks.
1 comment May 12th, 2009
The barometer shows the atmospheric pressure to be 760 mm Hg. What is the partial pressrure of nitrogen if nitrogen makes up 78% of the air?
In class we did practice problems with these equations:
Pgas=Ptotal-Pwatervapor
Ptotal=P1+P2+P3
I don’t understand what to do with the percent in the problem though because the equations only talk about pressure. Or are those equations even needed for this problem?
1 comment May 12th, 2009
Solid carbon reacts with carbon dioxide gas to produce carbon monoxide. At 1500 C the reaction is found to be at equilibrium with a Kp value of 0.50 and a total pressure of 3.5 atm.
1 comment May 12th, 2009
A 2.00 mole sample of gas is found to occupy 3.50L at 50 degrees Celsius and some pressure. What will be the new volume if the pressure is doubled, 3.00 moles of gas is added and the temperature is reduced to 15 degrees Celsius.
2 comments April 28th, 2009
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