- For the reaction N2(g)+3H2(g)⇌2NH3(g)N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)N2(g)+3H2(g)⇌2NH3(g), if the partial pressure of NH3NH_3NH3 is increased, the equilibrium will:
a) Shift to the right
b) Shift to the left
c) Remain unchanged
d) Increase the concentration of H2H_2H2
Answer: b - The equilibrium constant for the reaction 2SO2(g)+O2(g)⇌2SO3(g)2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)2SO2(g)+O2(g)⇌2SO3(g) will decrease if:
a) The temperature is increased
b) The pressure is increased
c) The concentration of SO2SO_2SO2 is increased
d) A catalyst is added
Answer: a - For a reaction with KpK_pKp = 0.5 at 300 K, if the temperature is increased to 400 K, the equilibrium constant becomes 0.3. This indicates:
a) The reaction is exothermic
b) The reaction is endothermic
c) The reaction has reached equilibrium
d) The reaction is at its highest rate
Answer: a - For the reaction H2(g)+I2(g)⇌2HI(g)H_2(g) + I_2(g) \rightleftharpoons 2HI(g)H2(g)+I2(g)⇌2HI(g), if the concentration of I2I_2I2 is doubled, the equilibrium will:
a) Shift to the right
b) Shift to the left
c) Remain unchanged
d) Increase the concentration of H2H_2H2
Answer: a - The van ‘t Hoff equation is used to:
a) Predict the shift in equilibrium due to changes in pressure
b) Calculate the effect of temperature on the equilibrium constant
c) Determine the reaction rate
d) Analyze the effect of concentration on equilibrium
Answer: b - For the reaction PCl5(g)⇌PCl3(g)+Cl2(g)PCl_5(g) \rightleftharpoons PCl_3(g) + Cl_2(g)PCl5(g)⇌PCl3(g)+Cl2(g), increasing the volume of the container will:
a) Shift the equilibrium to the right
b) Shift the equilibrium to the left
c) Have no effect on equilibrium
d) Decrease the pressure of Cl2Cl_2Cl2
Answer: a - In the equilibrium CO(g)+2H2(g)⇌CH3OH(g)CO(g) + 2H_2(g) \rightleftharpoons CH_3OH(g)CO(g)+2H2(g)⇌CH3OH(g), if the pressure is increased by adding an inert gas, the equilibrium will:
a) Shift to the right
b) Shift to the left
c) Remain unchanged
d) Increase the concentration of H2H_2H2
Answer: c - The equilibrium constant KcK_cKc for a reaction is 1×1051 \times 10^51×105 at 298 K and 2×1052 \times 10^52×105 at 350 K. This suggests:
a) The reaction is endothermic
b) The reaction is exothermic
c) The reaction does not reach equilibrium
d) The reaction rate decreases with temperature
Answer: a - For the reaction 2NO(g)+O2(g)⇌2NO2(g)2NO(g) + O_2(g) \rightleftharpoons 2NO_2(g)2NO(g)+O2(g)⇌2NO2(g), increasing the temperature will:
a) Shift the equilibrium to the right
b) Shift the equilibrium to the left
c) Have no effect on equilibrium
d) Increase the concentration of NO2NO_2NO2
Answer: b - In the equilibrium N2(g)+O2(g)⇌2NO(g)N_2(g) + O_2(g) \rightleftharpoons 2NO(g)N2(g)+O2(g)⇌2NO(g), if the temperature is decreased, the equilibrium constant KcK_cKc:
a) Increases
b) Decreases
c) Remains unchanged
d) Reaches zero
Answer: b
