Equilibrium Constants

What states or phases are  not included in the calculation of the equilbrium constant Keq?

• pure solids

• pure liquids

• gases

• aqueous ions

• pure solids & liquids

If in the chemical change: A(aq) + B(aq) -> C (aq) ,

and more A is added, then what happens?

• The Kc or Keq for this aqueous reaction stays the same.

• The Kc or Keq for this aqueous reaction changes.

• This aqueous reaction shifts "to the right" toward products.

• This aqueous reaction shifts "to the left" toward reactants.

Tags

NGSS.HS-PS1-5

What happens to the amount of chemical reactants (measured in Molarity or pressure) as a chemical change progresses "to the right" towards products, aka: "in the forward direction?"

• it stays constant before it reaches equilibrium

• it goes up before it reaches equilibrium

• it decreases before it reaches equilibrium

Tags

NGSS.HS-PS1-5

The equilibrium constant that is significantly greater than one favors:

• reactants

• products

• neither reactants nor products

Consider what "Ksp" means.

Equilibrium can only be mathematically applied to chemical changes, but not physical changes.

• true

• false

What type of system are most chemical systems in our world? This makes it more difficult to calculate equilibrium constants?

• constant Temperature

• Constante Pressure

• Constant Concentrations & Pressure of reactants & products

• open system

• closed system

Tags

NGSS.HS-PS1-6

How is the equilibrium constant defined?

• It is defined as the sum of the concentrations of reactants and products at equilibrium

• It is defined as the ratio of the initial concentrations of reactants and products

• It is defined as the ratio of the equilibrium concentrations of products to reactants

• It is defined as the difference between the initial and equilibrium concentrations of reactants and products

Can the value of the equilibrium constant (K) change with temperature?

• Yes, the value of K is temperature-dependent

• No, the value of K remains constant regardless of temperature

• Only for exothermic reactions

• Only for endothermic reactions

Tags

NGSS.HS-PS1-5

How can the equilibrium constant (K) be used to predict the direction of a reaction?

• If K is greater than 1, the reaction will proceed to the right (towards products)

• If K is greater than 1, the reaction will proceed to the left (towards reactants)

• If K is less than 1, the reaction will proceed to the right (towards products)

• If K is less than 1, the reaction will proceed to the left (towards reactants)

What role did Cato Guldberg and Peter Waage play in understanding chemical equilibrium?

• They discovered the law of mass action

• They formulated the concept of the equilibrium constant

• They developed the method for measuring equilibrium concentrations

• They studied the reaction between NO2 and N2O4