Question

A reaction at 300 K with $\Delta G^o$ = -1743 J/mol consists of 3 mole of $A\left(g\right)$, 6 mole of $B\left(g\right)$ and 3 mole of $C\left(g\right)$. If given $A,B$ and $C$ are in equilibrium in 1 litre container then the reaction may be:
[Given : 2 = $e^{0.7}$, R = 8.3 J/K - mol]

• A. $A+B\rightleftharpoons C$
• B. $A\rightleftharpoons B+2C$
• C. $2A\rightleftharpoons B+C$
• D. $2C\rightleftharpoons A+B$

Answer 1

The correct option is B $A\rightleftharpoons B+2C$

$\Delta G=-RTlnK$

$-1743=-8.3\times 300lnK$

$\frac{-1743}{-8.3\times 300}=lnk$

$0.7=lnk$

$k=e^{0.7}=2$

Let reaction x $A+yB\to C$

$k=\frac{[C{]}^2}{\left[A{]}^x\right[B{]}^4}$

$2=\frac{3^2}{3^x{6}^y}$

$2=3^{z-x-y}{2}^{-y}$

$y=-1$ $z-x=1$

$z=2x=1$

Reaction would be

since y becomes -1 so it be in product

$A\rightleftharpoons B+2C$