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Chemistry
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11 Dec 2019

What would be the change in pressure in a sealed 10.0 L vessel due to the formation of N2 gas when the ammonium nitrite in 2.00 L of 1.20 M NH4NO2 decomposes at 25.0°C

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Related questions

My answer is wrong, can anyone explain why?



Ammonium carbamate (NH2CO2NH4) decomposes when heated and, in a sealed vessel, the following equilibrium is established,

NH4CO2NH2(s) ⇌ 2 NH3(g) + CO2(g)

with Kp = 2.9 x 10–3 at 25oC. (a) Calculate the total gas pressure at equilibrium.

(c) If 5.00 g NH4CO2NH2 was introduced into an evacuated 5.00-L reaction vessel and the above equilibrium is established at 25oC, how many grams of solid NH4CO2NH2 still remains at equilibrium?
(R = 0.0821 L.atm/mol.K)

I only need help with part (c).

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