Chemical EquilibriumHard
Question
A reaction at 300 K with ΔGo = −1743 J consists of 3 moles of A(g), 6 moles of B(g) and 3 moles of C(g). If A, B and C are in equilibrium in 1 L container, then the reaction may be (ln 2 = 0.7, R = 8.3 J/K-mol)
Options
A.A + B$\rightleftharpoons$C
B.A$\rightleftharpoons$B + 2C
C.2A$\rightleftharpoons$B + C
D.A + B$\rightleftharpoons$2C
Solution
$\Delta G^{o} = - RT.\ln K_{P}^{o}$
⇒ –1743 = – 8.3 × 300 × ln KP°
∴ KP° = 2
Create a free account to view solution
View Solution FreeMore Chemical Equilibrium Questions
The activation energies for the forward and reverse elementary reactions in the system A$\rightleftharpoons$B are 10.303...The equilibrium between gaseous isomers A, B and C can be represented as follows.A(g) $\rightleftharpoons$B(g); K1 =? B(...In a system A(s) $\rightleftharpoons$2B(g) + 3C(g), if the concentration of C at equilibrium is increased by a factor of...For the equilibrium SrCl2·6H2O(s) $\rightleftharpoons$SrCl2·2H2O(s) + 4H2O(g), KP = 8.1 × 10−7 atm4 at 27oC. If 1.642 L ...The reactions PCl5(g) ⇋ PCl3(g) + Cl2(g) and COCl2(g) ⇋ CO(g) + Cl2(g) are simultaneously in equilibrium at ...