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Thermal decomposition of gaseous X₂ to gaseous X at 298 K takes place according to the following equations:
X₂ (g) $\leftrightharpoons$ 2X (g)
The standard reaction Gibbs energy, $\Delta _rG^o$, of this reaction is positive. At the start of the reaction, there is one mole of X₂ and no X. As the reaction proceeds, the number of moles of X formed is given by $\beta$. Thus, $\beta _{equilibrium}$ is the number of moles of X formed at equilibrium. The reaction is carried out at a constant total pressure of 2 bar. Consider the gases to behave ideally. (Given R = 0.083 L bar K^-1 mol^-1)
Question
The equilibrium constant K_p for this reaction at 298 K, in terms of $\beta _{equilibrium}$, is

The thermal dissociation equilibrium of CaCO₃(s) is studied under different conditions

CaCO₃(s) $\leftrightharpoons$ CaO(s) + CO₂(g).

For this equilibrium, the correct statement(s) is (are)

The equilibrium

$2C{u^+} \to Cu^\circ + C{u^{2+}}$

In aqueous medium at 25$^\circ$C shifts towards the left in the presence of

Statement 1 : For every chemical reaction at equilibrium, standard Gibbs energy of reaction is zero.

and

Statement 2 : At constant temperature and pressure, chemical reactions are spontaneous in the direction of decreasing Gibbs energy.

$ \begin{aligned} & \mathrm{Ag}^{+}+\mathrm{NH}_3 \quad\left[\mathrm{Ag}\left(\mathrm{NH}_3\right)\right]^{+} \\ & k_1=3.5 \times 10^{-3} \\ & {\left[\mathrm{Ag}\left(\mathrm{NH}_3\right]^{+}+\mathrm{NH}_3 \quad\left[\mathrm{Ag}\left(\mathrm{NH}_3\right)_2\right]^{+}\right.} \end{aligned} $

$k_2=1.7 \times 10^{-3}$, then the formation constant of $\left[\mathrm{Ag}\left(\mathrm{NH}_3\right)_2\right]^{+}$ is :

$ \mathrm{N}_2+3 \mathrm{H}_2 \to 2 \mathrm{NH}_3 $

Which is the correct statement if $\mathrm{N}_2$ is added at equilibrium condition?