CH10 reaction rates and equilibrium

What is rate of reaction?

The rate of a chemical reaction measures how fast a reactant is being used up or how fast a product is being formed.

What makes an effective collision?

-particles collide with the correct orientation

-particles have sufficient energy to overcome the activation energy barrier of the reaction.

Methods for following the progress of a reaction

• removal of a reactant

• The formation of a product

What is a homogenous catalyst?

Has the same physical state as the reactants

What is a heterogeneous catalyst?

Has a different physical state from the reactants.

What is le chateliers principle?

When a system in equilibrium is subjected to an external change the system readjusts itself to minimise the effect of that change.

What is the effect on equilibrium is concentration changes?

• increased conc. of products means equilibrium shifts to the right

• Increased conc. of reactants means equilibrium shifts to the left.

Effect of temperature on position of equilibrium

Increase in temp shifts equilibrium to the endothermic side

Decrease in temp shifts equilibrium to the exothermic side

Effect of pressure on equilibrium

Increase= equilibrium shifts to side with fewer moles

Decrease= equilibrium shifts to side with more moles.

Equation for calculating the Kc constant (E.g equation= A + 2B = C + D

[C(g)][D(g)] / [A(g)][B(g)]2

What are the features of dynamic equilibrium

• rate of forwards reaction is equal to reverse reaction

• Concentrations of reactions are equal

• Closed system