Unit D - Energy & Rates

How does how effectively transformation energy affect human civilization.

Our ability to harness energy has greatly, contributed to the development of human civilization, but how efficiently we transform energy determines the sustainability and effectiveness of those advancements.

What is energy efficiency? (6)

Energy efficiency is the percentage of useful energy produced compared to the total energy used.

• Higher efficiency = less wasted energy

• Hydroelectricity ≈ 85% efficient

• Solar energy ≈ 15% efficient

• Using energy-efficient devices helps conserve energy and reduce costs.

an alternative energy source

Hydrogen gas is an alternative energy source that can be used as a fuel. When hydrogen burns, it releases a large amount of energy, and the only product formed is water vapour, which makes it cleaner for the environment than fossil fuels. However, hydrogen gas also has some disadvantages. It is expensive to produce because it is usually made through electrolysis (the process of using electricity to split water into hydrogen gas and oxygen gas). It is also difficult to store and transport safely because hydrogen is highly flammable.

Why doesn’t a perpetual motion machine work?

t would violate the laws of thermodynamics.

• First Law of Thermodynamics: Energy cannot be created or destroyed. A machine cannot make more energy than it receives.

• Second Law of Thermodynamics: Every energy transfer loses some energy as heat due to friction and inefficiency.

Therefore, a machine cannot run forever while producing unlimited energy.

Thermochemistry

The study of energy changes during physical or chemical changes in matter

Energy

the ability to do work (Joules or J)

Work

the amount of energy transferred by a force over a distance (J)

All forms of energy can be classified as either…

kinetic energy: the energy of an object due to its motion

potential energy: the energy of a body or system due to its position or composition:

thermal energy Vs Heat Vs Temp

The total quantity of potential energy of a substance

Heat The transfer of thermal energy from a warm object to a cooler object. ( - When you heat water in a kettle, you transfer thermal energy from the burner to the kettle on the water. - When you cool an object such as letting the kettle rest, the energy is transferred to its surroundings.)

Temperature a measure of the average kinetic energy of entities in a substance

Temperatures relation to kinetic energy

The higher the temperature the higher the kinetic energy

Law of Conservation of Energy, What does is tell us about Chemical Systems?

Energy cannot be created or destroyed, It just changes from. 

From the law of conservation fo energy, you know that the total energy in a chemical system and its surrounds must be the same before and after the reaction

Chemical System Vs surrounding

a group of reactants and products being studied vs All the matter that is not part of the system

Types of Reactions explain

Exothermic: releasing energy to the surroundings Eng on product side

Endothermic: Absorbing energy from the surroundings Energy on reactant side

Endothermic or Exothermic?

Exothermic

Endothermic or Exothermic?

Endothermic

Nuclear Energy (3) + 2 forms (3 each)

all nuclear reactions are exothermic.

Per unit of mass, nuclear reactions release much more energy than standard exothermic chemical reactions.

There a two types of nuclear reactions: Fusion & Fission

Fusion: the process of combining two or more nuclei of low atomic mass to form a heavier, more stable nucleus Currently the sun is undergoing this kind of fusion reaction making helium. As planets get older they will start fusing heavier elements. Hydrogen > Helium > Lithium etc Fusion reactions are extremely energy efficient

Fission: the process of using a neutron to split a nucleus of high atomic mass into two nuclei with smaller masses Fusion reactions are 3-4x more efficient than fission reactions Fusion is 4 million times more efficient than gas

potential or kinetic?

A stick of dynamite prior to explode

a space shuttle before launch

the soot rising above a campfire

the chemicals inside a battery

potential

potential

kinetic

potential

endo or exo? 

water evaporating into steam.

a candle burning

the combustion of gasoline

the melting of ice

the splitting of a nitrogen molecule, n2, into two individual atoms

endo

exo

exo

endo

exo

mass

n x M

Specific heat capacity (fancy. simple, symbol)

(c) The quantity of thermal energy required to raise the temperature of 1g of substance by 1C; J/(g.C)

- In simple terms it tells you how resistant a material is to changing temperature. How “stubborn” the substance is.

Lower specific heat → ______ resistant to change

Higher specific heat→ ______ resistant to change

Less

more

Specific heat capacity (Water)

4.18 J/g.c

Calorimetry? What do scientists use calorimetry for? Calorimeter

the process of measuring energy changes during physical/chemical changes

study the thermal energy transfer

a device that is used to measure thermal energy change in physical/chemical changes

specific heat capacity formula or the heat energy formula.

Q=MCT

q: the total amount of thermal energy absorbed or released by a chemical system (J)

m: mass in grams

c: specific heat capacity (J/g x C)

ΔT: change in temperature (C)

ΔT = Tfinal - Tinitial

Enthalpy (H)

The total amount of thermal energy in a substance/system

Enthalpy Change (ΔH) (3)

Enthalpy change represents the heat energy transferred into or out of a chemical system during a reaction/chemical or physical change

H is neg (exothermic)

H is pos (endothermic)

Endothermic or Exothermic?

Exothermic

Endothermic or Exothermic?

Endothermic

Change in Hr

ΔHr: The enthalpy change associated with a physical, chemical, or nuclear change involving 1 mol of a substance, J/mol

We use this to determine how much energy might be produced or absorbed in a given chemical reaction

Change in Hr for solution, combustion, vaporization, formation, neutralization

Hsol

Hc

Hvap

Hf

Hneut

Always set to one mol

total enthalpy change formula

ΔH=nΔHr​

• ΔH = total enthalpy change of the reaction (kJ)

• n = number of moles (mol)

• ΔHr = molar enthalpy change (enthalpy change per mole of reaction) (kJ/mol)

ΔHsystem​ = −q surroundings​, what does it show?

It shows that heat energy is conserved. The heat lost by the system is gained by the surroundings (and vice versa). If the system releases heat, the surroundings absorb the same amount of heat, and if the system absorbs heat, the surroundings lose it.

Exothermic or Endothermic?

Exothermic

Exothermic or Endothermic?

Endothermic

A covalent bond between 2 atoms will break if…

enough energy is supplied

bond dissociation energy (4)

The quantity of energy required to break a chemical bond

They all have positive values

- All for 1 mol

(kJ/mol)

Bond dissociation energy for C = O

799 kJ/mol

Bond Energies

Bond energies can be used to calculate approximate enthalpy changes

ΔH=∑Ebonds broken​−∑Ebonds formed​

• Bonds broken → energy is absorbed (positive)

• Bonds formed → energy is released (negative)

D is the bond energy taken from the tables

Hess’s Law

The enthalpy change for the conversion of reactants to products is the same whether the conversion occurs in one step or several steps

Standard Enthalpy of Formation + formula (2)

The Standard Enthalpy of Formation (ΔHf) of a compound is the change in enthalpy that occurs when 1 mol of compound is formed from its elements, with all substances in their standard states. (kJ/mol)

ΔH reaction = {n products ΔH products - {n reactants ΔH reactants

Standard State + At standard state (4)

The most stable form of a substance under standard conditions 25oC and 100kPa

HOFNCl and Nobles gases are gases

Mercury and Bromine are liquids

All others are solids

Chemical Kinetics

the branch of chemistry that deals with rates of reactions

what is the reaction rate of a chemical reaction (2)

The reaction rate of a chemical reaction is the change in concentration of a reactant or product per unit of time

The stems from the concept that different reactions have different speeds.

How do chemists measure reaction rates if there is no “speedometer” for reactions?

how fast reactants are used up

products are formed over time

eactions don’t have “end point,”

scientists measure changes over time to determine arr

Average Reaction Rate + formula +Determining Average Reaction Rate using Graphical Data

the change of reactant or product concentration over a unit of time

rate A = Conentration of A at time t2 - concentration of A at time 1 / t2- - t1 

you would always want a positive reaction rate

rate a = change in (A)/change in T 

change in y (concentration) /change in x (time)

(rise over run)

Factors Affecting Reaction Rates

Chemical Properties

Concentration of reactants

Surface Area

Temperature

Presence of a catalyst

Catalyst

a substance that alters the rate of a chemical reaction without itself being permanently changed

Why are reaction rates important in industry, and what role do catalysts play?

Reaction rates are important in industry because they make manufacturing processes faster, cheaper, and more efficient. Catalysts are substances that speed up reactions without being used up. They are used in real-life applications like catalytic converters and in food production (e.g., blue cheese).

Collision Theory, what is it? how do the 5 factors inc it?

Collision Theory states that chemical reactions can occur only if reactants collide with proper orientation and with enough kinetic energy. (activation energy)

Enough to break the bonds and form products By adjusting our 5 factors of reaction rate, we are increasing the amount of collisions that can occur making the reaction happen

“Enough kinetic energy” → Activation Energy

The minimum energy that reactant molecules must possess for a reaction to be successful.(Ea)

Think of the activation energy as a hill or barrier that the reactants must undergo to perform the reaction (hump on graph)

Temperature in correlation to rates of reactions

When temperature is increased, there is higher kinetic energy in the system, thus a higher likelihood of collisions

Faster reaction rate

Concentration affect on the rate of reaction:

As concentration increases → more reactant products in the same volume → higher likelihood of collisions → faster reaction

Where would the reaction be slower, wb faster? Why?

slow, fast - concentration because there are more particles in the same volume.

Surface Area affect on the rate of reaction: why?

As Surface Area increases → more opportunities for collisions → faster reaction

How do catalysts work + Two types of Catalyst: explain + biological catalysts

For any reaction to occur, the kinetic energy of colliding reactant entities must be equal to or greater than the activation energy. However, Catalysts don’t affect either of these things

Catalysts provides an alternative pathway for the reaction, which has a lower activation energy

Heterogeneous Catalyst: a catalyst in a reaction in which the reactants and the catalyst are in different physical states

Homogeneous Catalyst: a catalyst in a reaction in which the reactants and the catalysts are in the same physical state

A catalyst made by a living system, usually an enzyme eg) lactase to break down the sugars in milk products for someone who is lactose intolerant To speed up fermentation of alcohols, cheeses, yogurts etc