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 process 2A(g) $\rightleftharpoons$A2(g) has KP = 8 × 108 atm−1. If ‘A’ atoms are taken at 1 atm pressure, then what ...The equilibrium constant for the reaction N2(g) + O2(g) ⇋ 2NO(g) at temperature T is 4 × 10-4. The value of K...What is the approximate value of log KP for the following reaction?N2(g) + 3H2(g) $\rightleftharpoons$ 2NH3(g) at 25°C. ...The equilibrium NH4HS(s) $\rightleftharpoons$NH3(g) + H2S(g) is achieved at the equilibrium pressure of ‘X’ bar at T K. ...Which of the following hypothetical reactions is favoured by the increase of temperature as well as pressure?...