Question

Ammonium carbamate decomposes as
NH,COONH,(s)
2NH3(g) + CO2(9)
For this reaction, Kp = 108 x 10-6 atm3. 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​

Answer 1

Given info : Ammonium carbamate decomposes as NH2COONH4(s) ⇒2NH3(g) + CO2(g) , For this reaction, Kp = 108 x 10-6 atm³

To find : if we start with 1 mole of the compound, the total pressure at equilibrium would be...

solution : chemical reaction is ..

NH2COONH4(s) ⇒2NH3(g) + CO2(g)

at eql 2x x

so p(NH3) = 2x

p(CO2) = x

now equilibrium constant, Ksp = [2p(NH3)]² [p(CO2)]

⇒108 × 10¯⁶ atm³ = (2x)² × x = 4x³

⇒27 × 10¯⁶ atm³ = x³

⇒(3 × 10¯² atm)³ = x³

⇒x = 3 × 10¯² atm = 0.03 atm

Therefore the total pressure would be = (2x + x) = 3x = 0.09 atm.

Answer 2

Answer:

0.09atm

Explanation:

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