Ch 14 Salles Test

Rate

A rate is the ratio between two related quantities expressed in different units.

Reaction Rate

The reaction rate is the rate at which the reactants of a chemical reaction form the products.

Collision Theory

According to collision theory, in order for a collision to be effective, reactant particles must possess a sufficient amount of kinetic energy to break the necessary bonds in the reactants. They must also collide with the right orientation to form the bonds that make the products.

Activation Energy

The minimum energy requirement for colliding particles to react is known as the activation energy.

Activated complex

The activated complex is a transition state that exists for a short period of time in a chemical reaction as the bonds in the reactants are breaking and the bonds in the products are forming.

Reaction Intermediate

A reaction intermediate is a product of one step in a multistep reaction and a reactant in a following step.

Rate-Determining Step

For multistep reactions, the slowest reaction is called the rate-determining step, and it affects the overall rate of a reaction.

Catalyst

A catalyst is a substance that increases reaction rates by providing a lower energy path for the reaction without being used up during the reaction.

Enzyme

Therefore, a biological catalyst called an enzyme is often needed. Enzymes are proteins or other molecules that fold into specific shapes to form indentations called active sites.

Reversible reactions

product molecules under ordinary conditions can react to form the originall reactant molecules.

Chemical equilibrium

a state of balance in which the rates of the forward and reverse reactions are equal. In other words, the forward and reverse reactions are both happening at the same time and at the same rate.

Equilibrium Position

The relative concentrations of the reactants and products at equilibrium mark the equilibrium position of the reaction.

Le chateliers principle

states that if a chemical system at equilibrium experiences a disturbance, it changes in a way that counteracts the change as it returns to equilibrium.

2S02(g) + O2(g) →→ 2SO3(g)

Sulfur Trioxide Synthesis

CO2(aq) + H2O(l) →→H2CO3(aq)

Blood buffering system

2H2(g) + S2(g)→ →2H2S(g)

Hydrogen Sulfide Synthesis

N2(g) + 3H2(g) →→ 2NHg(g) + heat

Haber process