TOPIC 11- THERMOCHEMISTRY

Question 1

is the capacity to do work or produce heat.

Answer 1

Energy

Question 2

states that energy can be
converted to another form but can be neither created nor destroyed.

Answer 2

Law of Conservation of Energy

Question 3

The total energy content of the universe is

Answer 3

Constant

Question 4

What are the classifications of energy?

Answer 4

1. Potential Energy
2. Kinetic Energy

Question 5

is due to position or composition and can also be a
result of attractive and repulsive forces.

Answer 5

Potential Energy

Question 6

is due to the motion of an object and depends on the
mass and velocity of the object.

Answer 6

Kinetic Energy

Question 6

is the part of the universe that is the current point of focus.

Answer 6

system

Question 7

include everything else in the universe.

Answer 7

Surroundings

Question 8

are reactions in which heat is expended and
flows out of the system.

negative

Answer 8

Exothermic Reactions

Question 9

are reactions in which heat is absorbed and
flows into the system.

Answer 9

Endothermic Reactions

Question 10

If two reactants at the same temperature are mixed and the resulting
solution gets warmer, this means the reaction taking place

Answer 10

exothermic

Question 11

endothermic reaction ____ the solution.

Answer 11

cools

Question 12

What are the types of systems?

Answer 12

1. Open System
2. Closed System
3. Isolated System

Question 13

allows both matter and energy (heat) to be exchanged
between the system and surrounding.

Answer 13

Open System

Question 14

only allows energy (heat) to be exchanged between
the system and surrounding.

Answer 14

Closed System

Question 15

does not allow both matter and energy (heat) to be
exchanged between the system and surrounding.**

Answer 15

Isolated System

Question 16

of a system is the sum of the kinetic and potential
energies of all “particles” in the system.

can be changed by a flow of work,
heat, or both.

Answer 16

Internal Energy (E)

Question 17

is often called the first law of
thermodynamics and proposes that the energy of the universe is
constant.

Answer 17

Law of Conservation of Energy

Question 18

What are the two ways which a system can change its internal energy?

Answer 18

1. Losing some energy to the sorroundings
2. Gaining some energy to the surroundings

Question 19

When losing some energy to the surroundings, what happens to the △E and energy?

Answer 19

△E is negative and energy leaves the system. Therefore, it is exothermic.

Question 20

When gaining some energy from the surroundings, what happens to the △E and energy?

Answer 20

△E is positive and energy enters the system. Therefore, it is endothermic.

Question 21

What are the possibilities when energy transfers as heat only?

Answer 21

• heat flows out of the system
• heat flows into the system

Question 22

What are the possibilities when energy transfer as work only?

Answer 22

• work done by the system (exothermic)
• work done by the surrounding (endothermic)

Question 23

When a system gains energy, the surrounding loses the same magnitude of
energy and vice versa.

Answer 23

First Law of Thermodynamics

Question 24

It is expressed using the letter H and is a state function.

Answer 24

enthalpy

Question 25

is a property of a system that depends on the state of a system only, such as internal energy, pressure, and volume.

Answer 25

State function

Question 26

Enthalpy change is affected by the?

Answer 26

states of product and reactants

Question 27

The change in enthalpy at **constant pressure** is equal to the _______________ at that same pressure (only pressure-volume work is allowed).

Answer 27

heat

Question 28

The _________________ is also equal to the difference of the enthalpy of products and reactants.

Answer 28

change in enthalpy

Question 29

Δ𝐻 is ------- when the enthalpy of products is **greater** than that of reactants.

Answer 29

positive

Question 30

Δ𝐻 is _____________ when the enthalpy of products is **lesser** than that of reactants.

Answer 30

negative

Question 31

does not depend on the pathway between two states.

Answer 31

change in enthalpy

Question 32

It is the science of measuring heat.

Answer 32

calorimetry

Question 33

measures the heat associated with chemical reactions.

Answer 33

calorimeter

Question 34

is the energy required to **raise the temperature of one gram** of substance by one degree Celsius.

Answer 34

Specific Heat Capacity

Question 34

is like specific heat capacity but **without the gram units**.

Answer 34

Heat Capacity

Question 35

is the energy required to **raise the temperature of one mole** of substance by one degree Celsius.

Answer 35

Molar Heat Capacity

Question 36

If a substance has a **higher Δ𝑇** than another, it means it has a __________ specific heat.

Answer 36

smaller

Question 37

Metals require comparatively ___________ to increase their temperature by one degree.

Answer 37

lesser energy

Question 38

is often used to measure the heat transferred in processes open to the atmosphere.

Answer 38

coffee-cup calorimeter

Question 39

Determines changes in enthalpy for **reactions that occur in solution**.

Answer 39

Constant-Pressure Calorimetry

Question 40

In a constant-volume process, the change in volume ΔV is equal to zero, meaning that work is also zero.

Answer 40

Constant-Volume Calorimetry

Question 41

The Δ𝐻 of an overall reaction is equal to the sum of the individual enthalpy change of each step.

Answer 41

Hess's Law

Question 42

If a reaction is reversed, the sign of Δ𝐻 becomes the _________.

Answer 42

opposite

Question 43

is the change in enthalpy accompanying the formation of **one mole** of a compound from its elements with all substances in their standard states.

Answer 43

standard ethalpy of formation

Question 44

Positive Δ𝐻 exhibits an?

Answer 44

Endthermic Reaction

Question 45

Negative Δ𝐻 exhibits an

Answer 45

Exothermic Reaction

Question 46

is a precisely defined reference state.

Answer 46

standard state

Question 47

In standard states, _________ are: * a pressure of exactly 1 atm in gases * pure liquid or solid for condensed pure substances * a concentration of exactly 1 M for substances in a solution

Answer 47

compounds

Question 48

In standard states, _________ is a form in which the elements exist under conditions of 1 atmosphere and 25°C

Answer 48

elements

Question 49

_____ in their **standard states** are not included in the calculations

Answer 49

Elements