Question:
For the reaction taking place at certain temperature
${NH_2 COONH_4 (s) <=> 2NH_3 (g) + CO_2 (g) }$, if equilibrium pressure is 3X bar then $ \Delta_G$ would
be
For the reaction taking place at certain temperature
${NH_2 COONH_4 (s) <=> 2NH_3 (g) + CO_2 (g) }$, if equilibrium pressure is 3X bar then $ \Delta_G$ would
be
Updated On: Jan 30, 2025
- - RT ln 9 - 3RT ln X
- RT ln 4 - 3RT ln X
- - 3RT ln X
- None of these
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The Correct Option is D
Solution and Explanation
$N H _{2} C O O N H _{ 4 } \rightarrow 2 N H _{3}+ C O _{2}$
$2 X+X=3 X $
$K=2 X^{2} \times X=4 X^{3}$
Standard gibb's free energy $=-R T \times \ln K$
$\Delta G^{\circ}=-R T \times \ln 4 X^{3} $
$\Delta G^{\circ}=-3 R T \ln 4 X$
$2 X+X=3 X $
$K=2 X^{2} \times X=4 X^{3}$
Standard gibb's free energy $=-R T \times \ln K$
$\Delta G^{\circ}=-R T \times \ln 4 X^{3} $
$\Delta G^{\circ}=-3 R T \ln 4 X$
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Concepts Used:
Gibbs Free Energy
The energy associated with a chemical reaction that can be used to do work.It is the sum of its enthalpy plus the product of the temperature and the entropy (S) of the system.
The Gibbs free energy is the maximum amount of non-expansion work that can be extracted from a thermodynamically closed system. In completely reversible process maximum enthalpy can be obtained.
ΔG=ΔH−TΔS
The Conditions of Equilibrium
If both it’s intensive properties and extensive properties are constant then thermodynamic system is in equilibrium. Extensive properties imply the U, G, A.
