Chemical Equilibrium

The %yield of ammonia as a function of time in the reaction
$$\ce{N2(g) + 3H2(g) <=> 2NH3(g)},\quad\Delta H<0$$
at $(P,T_1)$ is given below.

If this reaction is conducted at $(P,T_2)$, with $T_2>T_1$, the %yield of ammonia as a function of time is represented by

The following reaction is performed at 298 K.
$$\ce{2NO(g) + O2(g) <=> 2NO2(g)}$$
The standard free energy of formation of NO(g) is 86.6 kJ/mol at 298 K. What is the standard free energy of formation of $\ce{NO2(g)}$ at 298 K? ($K_p=1.6\times10^{12}$)

The standard Gibbs energy change at 300 K for the reaction $\ce{2A <=> B + C}$ is 2494.2 J. At a given time, the composition of the reaction mixture is $[A]=\dfrac12$, $[B]=2$ and $[C]=\dfrac12$. The reaction proceeds in the : [R = 8.314 J/K/mol, e = 2.718]

Gaseous $\ce{N2O4}$ dissociates into gaseous $\ce{NO2}$ according to the reaction
$$\ce{N2O4(g) <=> 2NO2(g)}$$
At 300 K and 1 atm pressure, the degree of dissociation of $\ce{N2O4}$ is 0.2. If one mole of $\ce{N2O4}$ gas is contained in a vessel, then the density of the equilibrium mixture is :

The increase of pressure on ice ⇌ water system at constant temperature will lead to :

For the reaction $\ce{SO2(g) + 1/2 O2(g) <=> SO3(g)}$, if $K_P=K_C(RT)^x$ where the symbols have usual meaning then the value of $x$ is : (assuming ideality)

At a certain temperature, only 50% HI is dissociated into $\ce{H2}$ and $\ce{I2}$ at equilibrium. The equilibrium constant is :

Consider the following equilibrium
$$\ce{AgCl v + 2NH3 <=> [Ag(NH3)2]+ + Cl-}$$
White precipitate of AgCl appears on adding which of the following ?

What happens when an inert gas is added to an equilibrium keeping volume unchanged ?

For the decomposition of the compound, represented as
$$\ce{NH2COONH4(s) <=> 2NH3(g) + CO2(g)}$$
the $K_p=2.9\times10^{-5}$ atm$^3$.

If the reaction is started with 1 mol of the compound, the total pressure at equilibrium would be :

The thermal dissociation equilibrium of $\ce{CaCO3}(s)$ is studied under different conditions.
$$\ce{CaCO3(s) <=> CaO(s) + CO2(g)}$$
For this equilibrium, the correct statement(s) is(are)

The equilibrium
$$\ce{2Cu^{I} <=> Cu^{0} + Cu^{II}}$$
in aqueous medium at 25 °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.

The value of $\log_{10}K$ for a reaction $\ce{A <=> B}$ is

(Given: $\Delta_rH^\circ_{298K}=-54.07$ kJ mol⁻¹, $\Delta_rS^\circ_{298K}=10$ J K⁻¹ mol⁻¹ and $R=8.314$ J K⁻¹ mol⁻¹; $2.303\times8.314\times298=5705$)