For the reaction taking place at certain temperature NH2 COONH4 (s) 2NH3 (g) + CO2 (g) , if equilibrium pressure is 3X bar then ΔG would be

Question

For the reaction taking place at certain temperature NH2 COONH4 (s) <=> 2NH3 (g) + CO2 (g) , if equilibrium pressure is 3X bar then ΔG would be (A) - RT ln 9 - 3RT ln X (B) RT ln 4 - 3RT ln X (C) - 3RT ln X (D) None of these

Tardigrade Admin · Accepted Answer

N H 2 C O O N H 4 arrow 2 N H 3+ C O 2 2 X+X=3 X K=2 X2 × X=4 X3 Standard gibb's free energy =-R T × ln K Δ G°=-R T × ln 4 X3 Δ G°=-3 R T ln 4 X

Q. For the reaction taking place at certain temperature
$NH X_{2} COONH X_{4} (s) 2 NH X_{3} (g) + CO X_{2} (g)$ , if equilibrium pressure is 3X bar then $Δ_{G}$ would be

- RT ln 9 - 3RT ln X

RT ln 4 - 3RT ln X

- 3RT ln X

None of these

$N H_{2} COON H_{4} \to 2 N H_{3} + C O_{2}$
$2 X + X = 3 X$
$K = 2 X^{2} \times X = 4 X^{3}$
Standard gibb's free energy $= - RT \times ln K$
$Δ G^{\circ} = - RT \times ln 4 X^{3}$
$Δ G^{\circ} = - 3 RT ln 4 X$

Q. For the reaction taking place at certain temperature NHX2​ COONHX4​(s)​2NHX3​(g)+COX2​(g), if equilibrium pressure is 3X bar then ΔG​ would be