Kinetic Molecular Theory & Equillibruim

Equillibrium- The balanced state where the forward and reverse reactions are equal

Static equilibrium- A balanced state where theirs no movement

Dynamic Equilibrium- When the concentration of forward and reverse reactions are equal and the concentration of reactants and products remain the same

Forward reaction- when reactants form products

Reverse reaction- when products form reactants

Le Chateliers principle- when a stress is placed on a system at equilibrium, the system will go in the direction to minimize the stress placed on it

Stress- A change or disruption placed on a system at equilibrium

Shift- The direction the system moves in order to alleviate the stress ( study)

Temperature- The average kinetic energy

Concentration- The amount of molecules in a given area

Pressure- The amount of force of a substance in a given area

Increasing the temperature of an exothermic reaction results in

  • more reactants and fewer products ( it’s the shift)

Increasing the temperature of an endothermic reaction results in

  • more products and fewer reactants

————> positive enthalpy arrow goes to the right

<———— negative enthalpy arrow goes to the left

Why do Chemists want to prevent reactions from reaching equilibrium?

  • Chemists want to maximize the amount of chemicals they want to produce by keeping reactions from achieving equilibrium.

When are reactions reversible?

  • when they can go forward or backward without any extra energy being used

Haber process

  • N2+ 3H2——→ 2NH3

    • industrialized process for producing Ammonia

Disturbances to the equilibrium?

  • concentration

  • temperature

  • pressure

Kinetics- The study of chemical reaction rates

During collisions, the concentration of reactants and products will- both increase

Activation energy- The energy threshold thats needed to be overcome, in order to produce a chemical reaction

Kinetic energy- The actual speed of particles

reaction rates- The speed at which the chemical reaction takes place

Catalyst- increases the rate of reaction

What’s needed for a successful reaction to occur between reactant particles?

  • need to collide

  • need sufficient energy

  • need proper orientation