Chemical Equilibrium

What is Le Chatelier's principle and how does it relate to chemical equilibrium?

• Le Chatelier's principle is used to calculate the pH of a solution

• Le Chatelier's principle explains how a system at equilibrium responds to changes in conditions such as temperature, pressure, or concentration.

• Le Chatelier's principle only applies to solid-state reactions

• Le Chatelier's principle has no relation to chemical equilibrium

Tags

NGSS.HS-PS1-6

Discuss the factors that can affect the equilibrium of a chemical reaction.

• Color of the reactants

• Size of the reaction vessel

• Time of day

• Concentration, temperature, pressure, and catalysts

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

Write the equilibrium expression for the reaction: 2A + 3B ⇌ 4C + 5D

• Kc = [A]^2[B]^3 / [C][D]^5

• Kc = [C]^4[D]^5 / [A]^2[B]^3

• Kc = [C]^4[D]^5 / [A][B]

• Kc = [A]^2[B]^3 / [C]^4[D]^5

What is the effect of increasing the concentration of a reactant on the equilibrium position?

• No effect on the equilibrium position

• Causes the reaction to stop

• Shift to the right

• Shift to the left

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

Calculate the equilibrium constant (Kc) for the reaction: 2A + B ⇌ 3C, given the concentrations of A, B, and C at equilibrium.

• Kc = [A] * [B] / [C]

• Kc = [C] / ([A] * [B])

• Kc = [C]^3 / ([A]^2 * [B])

• Kc = [A]^2 * [B] / [C]^3

Tags

NGSS.HS-PS1-7

Explain the concept of dynamic equilibrium in chemical reactions.

• Equal rates of forward and reverse reactions

• The reaction only proceeds in one direction

• The reaction stops completely

• The reaction rate increases over time

Tags

NGSS.HS-PS1-6

Calculate the equilibrium constant (Kc) for the reaction: A + 2B ⇌ 3C, given the concentrations of A, B, and C at equilibrium.

• Kc = [A] / ([B]^2 * [C])

• Kc = [A]^2 / ([B] * [C]^3)

• Kc = [A]^3 / ([B]^2 * [C])

• Kc = [C]^3 / ([A] * [B]^2)

Tags

NGSS.HS-PS1-6

How is pH calculated?

• pH is calculated using the formula: pH = -log[H+]

• pH is calculated using the formula: pH = log[H+]

• pH is calculated by adding the concentration of H+ ions and OH- ions

• pH is calculated by multiplyingthe concentration of H+ ions and OH- ions

What is the relationship between pH and pOH?

• pH / pOH = 1

• pH *pOH = 14

• pH + pOH = 14

• pH - pOH = 14

Calculate the pH of a solution with a hydrogen ion concentration of 1.5 x 10^-3 M.

• pH = 5.67

• pH = 2.82

• pH = 1.23

• pH = 1.43