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2ND SEM: CHEMISTRY > Thermochemistry > Flashcards

Thermochemistry Flashcards

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1
Q

It refers to the average kinetic energy of particles.

A

Temperature

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2
Q

The part of the universe being studied or to
which attention is focused.

A

System

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3
Q

A process in which a system absorbs heat
from its surroundings.

A

Endothermic process

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4
Q

Which is an example of an endothermic process?

Boiling of water

Melting of ice

A

Melting of ice

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5
Q

It is the capacity to do work or supply heat.

A

Energy

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6
Q

The rest of the universe
outside the system.

A

Surroundings

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7
Q

Types of Systems

Allows the exchange of
both energy (heat) and
matter with surroundings.

A

Open System

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8
Q

Types of Systems

Allows the exchange of
energy (heat) only with
surroundings.

A

Closed System

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9
Q

Types of Systems

Allows neither energy nor
matter to be exchanged
with surroundings.

A

Isolated System

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10
Q

Transfers from object with
higher temperature to object
with lower temperature.

A

HEAT

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11
Q

It is a type of reaction if the system absorbs
heat from its surroundings.

A

Endothermic Process

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12
Q

It is a type of reaction if the system gives
off heat to the surroundings.

A

Exothermic Process

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13
Q

Endothermic or Exothermic

Condensation

A

Exothermic

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14
Q

Endothermic or Exothermic

Evaporation

A

Endothermic

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15
Q

Endothermic or Exothermic

Burning of coal

A

Exothermic

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16
Q

Endothermic or Exothermic

Photosynthesis

A

Endothermic

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17
Q

What Law?

The total energy of a closed system is neither
created nor destroyed; but can be
transformed from one form to another.

A

First Law of
Thermodynamics

18
Q

is the capacity to do work.

A

Energy

19
Q

In chemical reaction, __________ energy may be released and converted to heat.

A

Potential

20
Q

What Law?

In interactions between system and
surroundings, the total energy remains
constant or energy is not created nor
destroyed.

the heat lost by the
surroundings is gained by the
system, and vice-versa.

A

Law of Conservation of Energy

21
Q

What Law?

deals with the interconversion of energy into two forms, work, and heat.

A

First Law of Thermodynamics

22
Q

First Law of Thermodynamics=
In any process, the change in energy of a
system is ______ to the heat absorbed by the system and the work done on it

A

equal

23
Q

Positive (+) Δesys = _____________ process.

A

Endothermic

24
Q

Negative (-) Δesys = _____________ process.

A

Exothermic

25
Q

amount of energy required
to raise the temperature of a sample by 1oC.

A

Heat capacity (C)

26
Q

amount of energy
required to raise one gram of a
substance by 1oC.

A

Specific Heat (c)

27
Q

The amount of heat absorbed or released by a chemical
reaction at a constant atmospheric pressure.

A

Enthalpy (H)

28
Q

Enthalpy is an ____________ property.

A

extensive

29
Q

The “sea level” reference point for all enthalpy expressions is called the _________________

A

standard enthalpy of formation (ΔHof)

30
Q

Substances are said to be in the standard state at __ atm, hence the term “standard enthalpy.”

A

1

31
Q

The standard enthalpy of formation of any element in its most stable form is ______.

A

zero

32
Q

Is the heat change that
results when 1 mole of
the compound is formed
from its elements at a
pressure of 1 atm.

A

standard enthalpy of formation (ΔHof)

33
Q

ΔH is positive = _____________ process.

A

endothermic

34
Q

ΔH is negative = _____________ process

A

exothermic

35
Q

is the enthalpy of a rxn
carried out at 1 atm

A

ΔH rxn

36
Q

stoichiometric coefficient for reactants

A

m

37
Q

stoichiometric coefficient for products

A

n

38
Q

What Law?

The value of enthalpy (ΔH) for a reaction is the same
whether it occurs in one step or in series of steps.

A

Hess’s Law

39
Q

What rule of Hess’ Law
Rule 1
Rule 2
Rule 3

Enthalpy is an extensive property; it depends on the amount of reactants and products

A

Rule 1

40
Q

What rule of Hess’ Law
Rule 1
Rule 2
Rule 3

ΔH for a forward rxn is equal in magnitude but opposite in sign to its reverse rxn

A

Rule 2

41
Q

What rule of Hess’ Law
Rule 1
Rule 2
Rule 3

ΔH for reaction is the same whether it occurs in one step or in a series of steps

A

Rule 3

2ND SEM: CHEMISTRY (8 decks)

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