ACS Domain 7: Equilibrium

In a closed system at equilibrium, if the concentration of the reactant is doubled, what happens to the equilibrium constant \( K_c \) for the reaction?

A reaction mixture initially contains 1.00 M A and 2.00 M B. At equilibrium, the concentration of C is 0.50 M. If the reaction is \( A + 2B \rightarrow 3C \), what is the equilibrium constant \( K_c \)?

For the reaction \( 2NO_2(g) \leftrightarrow N_2O_4(g) \), which change would increase the quantity of \( N_2O_4 \) at equilibrium?

If the equilibrium constant for a reaction at 300 K is 10 and at 350 K is 25, what can be inferred about the reaction?

In which case will the addition of an inert gas at constant volume to the following reaction \( H_2(g) + I_2(g) \leftrightarrow 2HI(g) \) have no effect on the position of equilibrium?

What is the effect on the equilibrium position when the temperature is decreased for the exothermic reaction \( 2SO_2(g) + O_2(g) \leftrightarrow 2SO_3(g) \)?

The equilibrium constant for the reaction \( A(g) + B(g) \leftrightarrow C(g) + D(g) \) is 4.0 at a certain temperature. If the initial concentrations of A and B are each 2.0 M, what is the concentration of D at equilibrium?

The reaction \( PC_5(g) \leftrightarrow PCl_3(g) + Cl_2(g) \) has \( K_p = 0.25 \) at 500 K. If the initial pressure of \( PCl_5 \) is 0.4 atm, what is the total pressure at equilibrium?

If the equilibrium constant for a decomposition reaction is less than 1, what can be inferred about the reaction?

For a reaction where \( \Delta H = -30 \, kJ/mol \) and \( \Delta S = -80 \, J/mol \cdot K \), what is the effect of increasing temperature on the equilibrium constant?