What is the partial pressure of the NH3

AI Thread Summary
To find the partial pressure of NH3 in a mixture with a total pressure of 9.42 atm, first convert the given masses of CH4, NH3, and CO2 into moles. Use Dalton's Law of Partial Pressure, which states that the partial pressure of a gas is its mole fraction multiplied by the total pressure. Calculate the mole fraction of NH3 by dividing its moles by the total moles of all gases present. Finally, multiply this mole fraction by the total pressure to determine the partial pressure of NH3.
DallasMavs
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Homework Statement


The combined pressure of 32.0 g of CH4, 64.2 g NH3, and 100 g of CO2 is 9.42 atm. What is the partial pressure of the NH3



Homework Equations


Dalton's Law of Partial Pressure = P=Pa +Pb + Pc ...
The individual partial pressure follow the ideal gas law. For component A, (Pa)V=(nA)RT where nA is the number of oles in component A

The Attempt at a Solution


I have converted all the grams to moles by dividing the grams by the compounds molar mass. I have no idea what to do from there. Someone please help.
 
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Partial pressure of any gas is its molefraction * total pressure.
so, for your problem it is

\frac{n_{NH_3}}{n_{total}}.(9.42)
 
So, I would take the moles of NH3 and divide that by the total number of moles (moles of NH3, CH4, and CO2). Than multiply that by the total pressure. Is that correct?
 
DallasMavs said:
So, I would take the moles of NH3 and divide that by the total number of moles (moles of NH3, CH4, and CO2). Than multiply that by the total pressure. Is that correct?
yes that's it
 
Thanks for the assistance
 

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