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CHM012 > TOPIC 11- THERMOCHEMISTRY > Flashcards

TOPIC 11- THERMOCHEMISTRY Flashcards

1
Q

is the capacity to do work or produce heat.

A

Energy

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2
Q

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

A

Law of Conservation of Energy

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3
Q

The total energy content of the universe is

A

Constant

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4
Q

What are the classifications of energy?

A
  1. Potential Energy
  2. Kinetic Energy
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5
Q

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

A

Potential Energy

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6
Q

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

A

Kinetic Energy

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6
Q

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

A

system

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7
Q

include everything else in the universe.

A

Surroundings

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8
Q

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

negative

A

Exothermic Reactions

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9
Q

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

A

Endothermic Reactions

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10
Q

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

A

exothermic

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11
Q

endothermic reaction ____ the solution.

A

cools

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12
Q

What are the types of systems?

A
  1. Open System
  2. Closed System
  3. Isolated System
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13
Q

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

A

Open System

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14
Q

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

A

Closed System

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15
Q

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

A

Isolated System

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16
Q

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.

A

Internal Energy (E)

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17
Q

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

A

Law of Conservation of Energy

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18
Q

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

A
  1. Losing some energy to the sorroundings
  2. Gaining some energy to the surroundings
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19
Q

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

A

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

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20
Q

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

A

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

21
Q

What are the possibilities when energy transfers as heat only?

A
  • heat flows out of the system
  • heat flows into the system
22
Q

What are the possibilities when energy transfer as work only?

A
  • work done by the system (exothermic)
  • work done by the surrounding (endothermic)
23
Q

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

A

First Law of Thermodynamics

24
Q

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

A

enthalpy

25
Q

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

A

State function

26
Q

Enthalpy change is affected by the?

A

states of product and reactants

27
Q

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

A

heat

28
Q

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

A

change in enthalpy

29
Q

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

A

positive

30
Q

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

A

negative

31
Q

does not depend on the
pathway between two states.

A

change in enthalpy

32
Q

It is the science of measuring heat.

A

calorimetry

33
Q

measures the heat associated with chemical reactions.

A

calorimeter

34
Q

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

A

Specific Heat Capacity

34
Q

is like specific heat capacity but without the gram units.

A

Heat Capacity

35
Q

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

A

Molar Heat Capacity

36
Q

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

A

smaller

37
Q

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

A

lesser energy

38
Q

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

A

coffee-cup calorimeter

39
Q

Determines changes in enthalpy for reactions that occur in solution.

A

Constant-Pressure Calorimetry

40
Q

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

A

Constant-Volume Calorimetry

41
Q

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

A

Hess’s Law

42
Q

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

A

opposite

43
Q

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

A

standard ethalpy of formation

44
Q

Positive Δ𝐻 exhibits an?

A

Endthermic Reaction

45
Q

Negative Δ𝐻 exhibits an

A

Exothermic Reaction

46
Q

is a precisely defined reference state.

A

standard state

47
Q

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

A

compounds

48
Q

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

A

elements

49
Q

_____ in their standard states are not included in the calculations

A

Elements

CHM012 (13 decks)

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