Pure solid ammonium carbamate, NH4CO2NH2, is allowed to dissociate into a vacuum according to the equation:(adsbygoogle = window.adsbygoogle || []).push({});

NH4CO2NH2(s) ---> 2 NH3(g) + CO2(g)

At 25oC, the total pressure of the gases in equilibrium with the solid is 0.116 atm. If carbon dioxide, CO2, was then added, sufficient to have increased the carbon dioxide pressure by 0.100 atm under these conditions, when equilibrium is re-established, the new partial pressure of gaseous ammonia, NH3, will be

a. 1.16 atm

b. 1.08 atm

c. 4.36 x 10¨C2 atm

d. 2.31 x 10¨C3 atm

e. 6.93 x 10¨C4 atm

Ok, I can't seem to solve this problem. I know that total pressure = pressure of individual components in the mixture.

As well, since NH3 and CO2 is a 2:1 ratio:

2x + x = 0.116 atm

x = 0.03866 atm

I tried using the Kp to solve this problem, but the equation becomes way to difficult to find the root. The equation ends up being to the third power.

Is there a way to solve this? Thanks.

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# Homework Help: Partial Pressure Equilibrium lab

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