NEET Chemistry Chemical Equilibrium MCQs

A system at equilibrium consisting of $N_2(g)$, $O_2(g)$ and $NO(g)$ in a sealed vessel at constant temperature is subjected to a sudden increase in pressure. According to Le Chatelier's principle, which of the following is most likely to occur?

The solubility product ($K_{sp}$) of $AgCl$ in water at 25°C is $1.8 imes 10^{-10}$. A solution of $AgCl$ in water is in equilibrium with solid $AgCl$. If a small amount of $NaCl$ is added to this saturated solution, what will happen to the solubility ($s$) and $K_{sp}$ of $AgCl$?

Consider the endothermic reaction: $N_2O_4(g) \rightleftharpoons 2NO_2(g)$. A sealed container filled with an equilibrium mixture of $N_2O_4$ and $NO_2$ is suddenly immersed in an ice bath. Which of the following changes will occur initially?

In the Haber-Bosch process for ammonia synthesis, $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$, the reaction is exothermic. To maximize ammonia yield at high pressure, which catalyst would theoretically be most effective, assuming all are equally active at standard conditions?

A reaction $A(g) + B(g) \rightleftharpoons C(g)$ has a $K_c$ of 0.1 at 298 K. If initially 1 mole each of A and B are introduced into a 1L vessel, and the system is allowed to reach equilibrium, what approximate pressure change ($\Delta P$) must be applied to double the equilibrium concentration of C?

A reaction mixture for the reversible reaction $A(g) + 2B(g) \rightleftharpoons C(g)$ is at equilibrium at a given temperature. If the equilibrium partial pressures are $P_A$ = 0.2 atm, $P_B$ = 0.4 atm, and $P_C$ = 0.6 atm, what would be the effect of increasing the pressure of A to 0.3 atm while keeping the volume and temperature constant?

For the reaction $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$, $\Delta H$ = -198 kJ/mol. Which of the following changes will NOT increase the yield of $SO_3$ at equilibrium?

For the reversible reaction $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$ at a certain temperature, the partial pressures at equilibrium are $P_{SO_2} = 0.2$ atm, $P_{O_2} = 0.1$ atm, and $P_{SO_3} = 0.8$ atm. If the total pressure is suddenly doubled by adding an inert gas at constant volume, the new partial pressure of $SO_3$ at the newly established equilibrium will be closest to:

Which factor does NOT affect the equilibrium position of a reversible reaction?

For the reaction $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$ at equilibrium, increasing the pressure by decreasing the volume of the container will: