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AP Chemistry Fundamental Equilibrium Concepts — practice questions

Explore 20 free Fundamental Equilibrium Concepts questions in AP Chemistry Chemistry. Open each question or exercise to read its content, reference answers and available explanation.

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Fundamental Equilibrium Concepts questions and exercises with answers

Showing questions 1–20 of 20.

The constant value of the reaction quotient shown by a system at equilibrium is called the:Read the answer and worked solution →An equilibrium in which every reactant and product is in the same phase is described as:Read the answer and worked solution →For a gas-phase equilibrium, the constant can be written using concentrations or:Read the answer and worked solution →A reaction with a very large equilibrium constant reaches equilibrium when:Read the answer and worked solution →A change in conditions that upsets the balance of forward and reverse rates is called a:Read the answer and worked solution →If the reaction quotient is greater than the equilibrium constant, the reaction will proceed:Read the answer and worked solution →Adding reactant to a system at equilibrium makes the quotient smaller than K, so the equilibrium:Read the answer and worked solution →Adding hydrogen or iodine to a hydrogen iodide equilibrium increases the rate of:Read the answer and worked solution →Removing hydrogen iodide from its equilibrium mixture leaves the concentrations of all three species:Read the answer and worked solution →Multiplying every stoichiometric coefficient in an equation by a factor changes K:Read the answer and worked solution →Changing the volume of a gas-phase equilibrium changes the concentrations of:Read the answer and worked solution →A reaction quotient equation using absolute concentrations rather than relative values is:Read the answer and worked solution →Reactions differ from many physical processes in that they may proceed:Read the answer and worked solution →Many real systems involve coupled equilibria, meaning two reactions that share:Read the answer and worked solution →The reaction quotient is useful during a reaction because its value:Read the answer and worked solution →Which way does it shift?Read the answer and worked solution →Match each equilibrium termRead the answer and worked solution →True or false: equilibriumRead the answer and worked solution →Complete the Q against K ruleRead the answer and worked solution →Sort each symbol by what it measuresRead the answer and worked solution →

Worked practice questions

The constant value of the reaction quotient shown by a system at equilibrium is called the:

  1. Equilibrium constant
  2. The rate constant
  3. The gas law constant
  4. Avogadro's constant
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Correct answer: A. Equilibrium constant

1. The numerical value of the reaction quotient varies as a reaction proceeds towards equilibrium. 2. Once equilibrium is reached it stops changing. 3. The constant value of the reaction quotient exhibited by a system at equilibrium is called the equilibrium constant, K. 4. A rate constant belongs to kinetics rather than to equilibrium. _Source: OpenStax Chemistry 2e (CC BY 4.0), Ch 13 'Fundamental Equilibrium Concepts', sections 13.1-13.4_

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An equilibrium in which every reactant and product is in the same phase is described as:

  1. Instantaneous
  2. Homogeneous
  3. Heterogeneous
  4. Discontinuous
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Correct answer: B. Homogeneous

1. Equilibria are sorted by whether the species share a phase. 2. A homogeneous equilibrium is one in which all reactants and products are present in the same phase. 3. Any catalysts present are counted in that requirement too. 4. A heterogeneous equilibrium spans more than one phase. _Source: OpenStax Chemistry 2e (CC BY 4.0), Ch 13 'Fundamental Equilibrium Concepts', sections 13.1-13.4_

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For a gas-phase equilibrium, the constant can be written using concentrations or:

  1. Reaction rates
  2. Bond energies
  3. Partial pressures
  4. Absolute masses
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Correct answer: C. Partial pressures

1. A gas can be described equally well by how concentrated it is or by the pressure it exerts. 2. For gas-phase solutions, the equilibrium constant may be expressed in terms of either the molar concentrations or the partial pressures of the reactants and products. 3. The concentration form is written Kc and the pressure form Kp. 4. Rates and bond energies belong to other parts of chemistry entirely. _Source: OpenStax Chemistry 2e (CC BY 4.0), Ch 13 'Fundamental Equilibrium Concepts', sections 13.1-13.4_

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More Chemistry topics

Composition of Substances and SolutionsEquilibria of Other Reaction ClassesSolutions and ColloidsStoichiometry of Chemical ReactionsThermodynamicsAcid-Base EquilibriaAtoms, Molecules, and IonsChemical Bonding and Molecular Geometry