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Reversible Reaction

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  • 29. In the equilibrium reaction 2NO₂(g) ⇌ N₂O₄(g), which change will shift the equilibrium to the right, producing more N₂O₄?
    Increasing the temperature
    Decreasing the temperature
    Decreasing the pressure
  • In a closed system at equilibrium, what happens to the concentration of reactants and products?
    It remains constant
    It decreases to zero
    It keeps changing
  • What is the effect of adding more reactants to an equilibrium mixture?
    The backward reaction speeds up
    The reaction stops
    The forward reaction speeds up
  • What happens when the temperature of an exothermic reversible reaction at equilibrium is increased?
    The equilibrium shifts to the left
    The reaction stops
    The equilibrium shifts to the right
  • If the equilibrium reaction CO(g) + Cl₂(g) ⇌ COCl₂(g) is subjected to an increase in pressure, the equilibrium will:
    Not change
    Shift to the right
    Shift to the left
  • Which of the following will NOT change the position of equilibrium?
    Changing pressure
    Adding a catalyst
    Changing temperature
  • A catalyst increases the rate of:
    The forward reaction only
    The backward reaction only
    Both the forward and backward reactions equally
  • The reaction H₂ + I₂ ⇌ 2HI reaches equilibrium. If more H₂ is added, what happens?
    The equilibrium shifts to the left
    The reaction stops
    The equilibrium shifts to the right
  • The reaction N₂ + 3H₂ ⇌ 2NH₃ is exothermic in the forward direction. What happens if the temperature is increased?
    Less ammonia is produced
    More ammonia is produced
    The reaction stops
  • Which symbol represents a reversible reaction?
    ⇌
    =
    →
  • When pressure is decreased in the equilibrium reaction 2SO₂ + O₂ ⇌ 2SO₃, what happens?
    The equilibrium shifts to the left
    No change occurs
    The equilibrium shifts to the right
  • In the equilibrium reaction N₂O₄ ⇌ 2NO₂, what happens when the pressure is decreased?
    The equilibrium shifts to produce more NO₂
    The reaction stops
    The equilibrium shifts to produce more N₂O₄
  • In the Haber process N₂ + 3H₂ ⇌ 2NH₃, why is a high pressure used?
    To increase the activation energy
    To make the reaction slower
    To shift equilibrium to produce more ammonia
  • What is meant by a reversible reaction?
    A reaction that can go in both forward and backward directio
    A reaction that only goes forward
    A reaction that stops after forming the product
  • When a reversible reaction reaches equilibrium, what happens to the rate of forward and backward reactions?
    The forward reaction stops
    The rates of both reactions are equal
    The backward reaction is faster than the forward reaction
  • If the equilibrium mixture H₂ + Cl₂ ⇌ 2HCl is subjected to an increase in pressure, what happens?
    The equilibrium shifts to produce more HCl
    The equilibrium shifts to produce more H₂
    No change occurs
  • In the reaction CaCO₃ ⇌ CaO + CO₂, what happens when CO₂ is removed from the system?
    The equilibrium shifts to produce more CaCO₃
    No change occurs
    The equilibrium shifts to produce more CO₂
  • The reaction CO(g) + Cl₂(g) ⇌ COCl₂(g) is exothermic in the forward direction. What happens if the temperature is decreased?
    Less COCl₂ is produced
    The reaction stops
    More COCl₂ is produced
  • In the reaction N₂O₄ ⇌ 2NO₂, increasing the temperature will:
    Increase the amount of NO₂
    Not affect the equilibrium
    Increase the amount of N₂O₄
  • Which of the following statements about dynamic equilibrium is true?
    The forward reaction happens faster than the backward reacti
    Both the forward and backward reactions stop
    The concentrations of reactants and products remain constant
  • Which factor affects only the speed at which equilibrium is reached but not the position of equilibrium?
    Pressure
    Temperature
    Catalyst
  • The reaction H₂ + CO₂ ⇌ CO + H₂O is at equilibrium. What happens if H₂O is removed?
    The equilibrium shifts to the right
    The equilibrium shifts to the left
    No change occurs
  • Which of the following changes the equilibrium constant of a reaction?
    Pressure
    Catalyst
    Temperature
  • Which of the following is an example of a reversible reaction?
    Electrolysis of water
    Combustion of methane
    Thermal decomposition of ammonium chloride
  • Which of the following reactions will be affected by a change in pressure?
    C(s) + O₂ ⇌ CO₂
    N₂ + 3H₂ ⇌ 2NH₃
    H₂ + Cl₂ ⇌ 2HCl
  • What happens to an equilibrium mixture if the pressure is increased in a reaction with equal numbers of moles of gas on both sides?
    There is no effect
    The equilibrium shifts to the right
    The equilibrium shifts to the left
  • When a reversible reaction reaches dynamic equilibrium, what can be said about the amounts of reactants and products?
    They remain constant
    The reactants disappear completely
    They are always equal
  • In the equilibrium reaction 2NO₂ ⇌ N₂O₄, the forward reaction is exothermic. What color change is observed when the reaction vessel is cooled?
    Dark brown to pale yellow
    Pale yellow to dark brown
    No change
  • What happens if the pressure is increased in a reaction where there are fewer gas molecules on the right side of the equation?
    The reaction rate decreases
    The equilibrium shifts to the right
    The equilibrium shifts to the left
  • Which of the following conditions would increase the yield of methanol in the reaction CO(g) + 2H₂(g) ⇌ CH₃OH(g) (ΔH = -91 kJ/mol)?
    Low pressure and high temperature
    High pressure and low temperature
    High pressure and high temperature
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