Plant Systems Quiz #2

Question 1

The _____ represents the chaotic movements of particles, ΔU = ΔT.

Answer 1

Kinetic (Uk)

Question 2

The First Law of Thermodynamics in a closed system is represented by the formula _____ or _____.

Answer 2

ΔU = Q + W, ΔU = Q - W

Question 3

If there is rise in temperature, the reaction is _____ and involves a _____ change.

Answer 3

exothermic, negative

Question 4

The activation energy (Ea) for the forward reaction is Ea (forward) = (_____) - H (reactant)

Answer 4

H (activated complex)

Question 5

In Thermodynamics, _____ is a measure of the heat content of a chemical or physical system.

Answer 5

enthalpy

Question 6

_____ is the proportion of a form of energy that is not converted into useful work.

Answer 6

Anergy

Question 7

There are two types of _____ namely solar thermal and _____.

Answer 7

solar energy, solar photovoltaic

Question 8

Inside the sun, hydrogen atoms are heated so much they turn into a _____ state where electrons no longer orbit the protons in the atom’s nuclei.

Answer 8

plasma

Question 9

The ΔH change for the forward reaction is:

ΔH = (_____) - H (reactants)

Answer 9

H (products)

Question 10

_____ is energy that can be completely transformed into work without any loss or with minimal loss i.e. fully utilized.

Answer 10

High Grade Energy

Question 11

The 2nd Law of Thermodynamics is also known as _____

Answer 11

Law of Transmutability

Question 12

_____ is the transfer of thermal energy by electromagnetic waves.

Answer 12

Radiation

Question 13

When a process begins at constant pressure, the evolving heat either absorbed _____ or released _____ equals to the change in _____.

Answer 13

endothermic, exothermic, enthalpy

Question 14

The atmosphere also prevents heat from escaping back into space too quickly. It is called as _____.

Answer 14

Greenhouse effect

Question 15

_____ is the energy that is available to be used.

Answer 15

Exergy

Question 16

What are the state functions: _____, _____, _____, _____, and _____ inside the _____ of _____ functions.

Answer 16

entropy, enthalpy, Helmholtz, Gibbs, internal energy, space, thermodynamic

Question 17

Anyone who speaks about ‘energy _____’, or ‘energy _____’ is probably _____ about the _____ Law of Thermodynamics.

Answer 17

production, consumption, ignorant, First

Question 18

The _____ Law tells us about the _____ of the _____ and all process, namely towards a decreasing _____ content of the _____.

Answer 18

Second, direction, universe, exergy, universe

Question 19

_____ means absorbing _____ in the form of _____, while _____ means releasing _____ in the _____ of work.

Answer 19

Endergonic, energy, work, exergonic, energy, form

Question 20

When _____ say “free energy”, they usually mean _____ free energy (Arbeit in German), on the other hand, when _____ say “free energy” they refer to _____ free energy.

Answer 20

physicists, Helmholtz, chemists, Gibbs

Question 21

At constant volume, the heat of reaction is equal to the change in the internal energy of the system.

Answer 21

TRUE

Question 22

Inside the sun, helium atoms are heated and break as hydrogen and energy is released to the space as radiant energy.

Answer 22

FALSE

Question 23

At constant pressure, the heat of reaction is equal to the enthalpy change of the system.

Answer 23

TRUE

Question 24

All energy is composed of Free Energy, Bond Energy, Kinetic Energy, and Potential Energy in its initial kind.

Answer 24

FALSE

Question 25

Most chemical reactions occur at constant pressure, so enthalpy is more often used to measure the heat of reaction rather than internal energy.

Answer 25

TRUE

Question 26

If q < 0 and ΔH > 0 then it is exothermic

Answer 26

TRUE

Question 27

Your hand gets cold when you touch ice is an endothermic reaction.

Answer 27

FALSE

Question 28

The ice gets warmer when you touch it is an exothermic reaction.

Answer 28

FALSE

Question 29

Water boiling in a kettle being heated on a stove is an endothermic reaction.

Answer 29

TRUE

Question 30

Water vapor condenses on a cold pipe is an exothermic reaction.

Answer 30

TRUE

Question 31

Ice cream melts is an exothermic reaction.

Answer 31

FALSE

Question 32

The enthalpy change for an endothermic reaction is always negative.

Answer 32

FALSE

Question 33

Potential (Up) represents the strength of bonds ΔU = change in strength in bonds (state of matter).

Answer 33

TRUE

Question 34

To change internal energy is both to do work and to change heat (Q).

Answer 34

TRUE

Question 35

Low Grade Energy examples are wind turbine and hydro power because of limited wind and water availability especially during summer.

Answer 35

FALSE

Question 36

Breaking a bond is always endergonic.

Answer 36

TRUE

Question 37

Helmholtz is the capacity to do mechanical plus non-mechanical work.

Answer 37

TRUE

Question 38

Gibbs are often used since it is considered a constant volume condition.

Answer 38

FALSE

Question 39

ΔH > 0, ΔS > 0, T (high) is an endothermic and exergonic.

Answer 39

TRUE

Question 40

spontaneous = (of a process or event) occurring without apparent internal cause.

Answer 40

FALSE