Dynamic Equilibrium: Reactivity 2.3

Define dynamic equilibrium

Define dynamic equilibrium

A state in reversible reactions where:

• the continuous forward and reverse reaction rates are equal. (Rate_f=Rate_r)

• the concentration of reactants and products remains constant. ([R]=[R] & [P]=[P])

in a closed system.

Define equilibrium

A state in which reactant and product concentrations remain constant.

equation for rate

(Change in concentration)/ (change in time)

difference between equal and constant

• equal is used when comparing two things

• constant is used when comparing something to itself

Explain why the forward curve is above the reverse curve at the start.

because its at maximum rate due to the reactants having maximum concentration and therefore more frequent collisions happening.

Define irreversible reaction

reactants can form products, but products cannot form reactants

State three situations with irreversible reactions.

1. Reactions that produce gaseous products in an open system

2. Reactions that produce solid precipitates

3. Reactions between a strong acid and strong base

Explain why reactions that produce gaseous products in an open system are irreversible reactions.

Once released into the surrounding, gaseous particles are too far apart to collide with each other and react back into its reactant.

State an example of an irreversible reaction where the reaction produces a gaseous product in an open system.

2Na_(s)+2HCl_(aq)→2NaCl_(aq)+H_2(g)

State an example of an irreversible reaction where the reaction produces a solid precipitate

Pb(NO₃)_2(aq)+2Kl_(aq)→Pbl_2(s)+2KNO_3(aq)

State an example of an irreversible reaction where the reaction is between a strong acid and strong base.

HCl_(aq)+NaOH_(aq)→NaCl_(aq)H₂O_(l)

Define acids.

Substance that produces H⁺ when dissolved in water.

Define bases.

Substance that produces OH^- when dissolved in water.

Define strong acids and bases.

Acids and bases that undergo 100% dissociation.

Define weak acids and bases.

Acids and bases that do not undergo 100% dissociation.

Explain 100% dissociation.

Breaking up of 100% of a compound into simpler constituents

State an example of a strong acid.

HCl → H⁺+Cl^-

State an example of a strong base.

NaOH→Na⁺ + OH^-

Define reversible reactions.

Reactions that have both forward and reverse reactions simultaneously.

Define physical reactions.

Reactions that result in ONLY a change in the reactant’s state

Define chemical reactions.

Reaction in which valence electrons are transferred to break bonds of the reactant and form new bonds for the products.

State an example of a physical reaction/ system.

Br_2(l)⇌Br_2(g)

State an example of a chemical reaction/ system.

2NO_2(g)⇌2NO_(g)+O_2(g)

State the two types of reversible reactions.

• physical reaction

• chemical reaction

Explain saturated solutions using equilibrium.

dissolution rate = precipitation rate (at dynamic equilibrium) due to maximum amount of dissolved solute

Explain unsaturated solutions using equilibrium

Can dissolve more solute until saturation is reached.
Not in equilibrium state.

State the observations of a reaction at equilibrium state at a macroscopic level:

No observable changes in the system’s properties

State the observations of a reaction at equilibrium state at a microscopic level:

continuous interconversion of reactants and products

Define heterogenous equilibrium

Reaction at an equilibrium state with reactants of different phases.

Define homogenous equilibrium.

Reaction at an equilibrium state with reactants of same phases.

Define equilibrium position

Proportion of reactant and product in an equilibrium mixture (percentage)

Explain the phrase “lie to the right” in terms of equilibrium position.

Products>reactants

Explain the phrase “lie to the left” in terms of equilibrium position.

Reactants> products