Ammonium carbamate decomposes as NH,COONH, (s) 2NH,(g) +CO,(g) For this reaction, Kp = 108 x 10- atm2. If we start with 1 mole of the compound, the total pressure at equilibrium would be [NCERT Pg. 203, 204] (1) 0.058 atm (2) 0.048 atm (3) 0.09 atm (4) 0.03 atm
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Explanation:
The correct option is B 0.0582 atm
Correct option is b).
NH2COONH4 (s) 2NH3(g) + CO₂ (g)
At equilibrium, if partial pressure of CO₂ = p, and that of NH3 = 2p. Solving for p, p = 1.935x 10-²
Kp = (PNH3)2 x (Pco2) = (2p)² x p = 4p³ = 2.9×10³
Hence, total pressure = 3p = 0.0581 atm
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