For the reaction NH 2 COONH 4( s ) leftharpoons 2 NH 3( g )+ CO 2( g ) the equilibrium constant KP=2.92 × 10-5 atm 3 . The total pressure of the gaseous products when 1 mol of reactant is heated will be:

Question

For the reaction NH 2 COONH 4( s ) leftharpoons 2 NH 3( g )+ CO 2( g ) the equilibrium constant KP=2.92 × 10-5 atm 3 . The total pressure of the gaseous products when 1 mol of reactant is heated will be: (A) 0.0194 atm (B) 0.0388 atm (C) 0.0582 atm (D) 0.0667 atm

Tardigrade Admin · Accepted Answer

underset(1-x)NH 2 COONH 4(s) leftharpoons underset2x2 NH 3(g)+ undersetxCO 2(g) Only gaseous substance are NH 3 and CO 2 ∴ Total mol of gaseous substances =3 x ∴ p NH 3 =peq ⋅ (2 x/3 x)=(2/3) p eq p CO 2=(1/3) p eq , Kp=(p NH 3)2(p CO 2) =((2/3) p eq )2((1/3) p eq )=2.92 × 10-5 ∴ p eq = 0.0582 atm

Q. For the reaction NH2​COONH4​(s)⇌2NH3​(g)+CO2​(g) the equilibrium constant KP​=2.92×10−5atm3. The total pressure of the gaseous products when 1mol of reactant is heated will be:

0.0194 atm

0.0388 atm

0.0582 atm

0.0667 atm

Q. For the reaction
$N H_{2} COON H_{4} (s) ⇌ 2 N H_{3} (g) + C O_{2} (g)$
the equilibrium constant $K_{P} = 2.92 \times 1 0^{- 5} a t m^{3} .$ The total pressure of the gaseous products when $1 m o l$ of reactant is heated will be: