Chemical Equilibrium digital book with solutions

Q. 1/6· Easy

Identify from following, the relation between standard free energy change in a reaction and equilibrium constant $K_{c}$ .

Q. 2/6· Medium

The equilibrium constants of the following are

\begin{array}{rl} & N_{2}+3H_{2}\longrightarrow 2NH_{3};K_{1} \\ & N_{2}+O_{2}\longrightarrow 2NO;K_{2}\end{array} \\ H_{2}+\dfrac{1}{2}O_{2}\longrightarrow H_{2}O;K_{3}

The equilibrium constant $(K)$ of the reaction : $2NH_{3}+\dfrac{5}{2}O_{2}\xrightarrow{K}2NO+3H_{2}O$ will be

Q. 3/6· Medium

The equilibrium constant for a reaction is 100 . What will be the value of standard Gibbs energy change at 298 K ? ( $R=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$ )

Q. 4/6· Medium

For the reaction $\mathrm{CH}_{4(\mathrm{~g})}+\mathrm{H}_{2(\mathrm{~g})} \longrightarrow C_{2} \mathrm{H}_{6(\mathrm{~g})} \mathrm{K}_{\mathrm{p}}=3.356 \times 10^{17}$ , calculate $\Delta \mathrm{G}^{\circ}$ for the reaction at 298 K .

Q. 5/6· Medium

Calculate standard Gibbs energy for any gaseous reaction if values of $K_{p}$ and $R$ respectively are $3.5 \times 10^{17}$ ; $8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}$

Q. 6/6· Hard

Calculate $\triangle G^{\circ}$ for reaction,

\mathrm{CH}_{4(g)}+\mathrm{H}_{2(g)} \rightarrow C_{2} \mathrm{H}_{6(g)}\left(K_{p}=2 \times 10^{17}, R=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)