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chem unit 2 > 10E- applications in society-Table 1 > Flashcards

10E- applications in society-Table 1 Flashcards

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1
Q

Define: Combustion

A

When a fuel reacts with oxygen (also called burning)

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2
Q

Define: Calcification

A

A chemical process that forms calcium carbonate

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3
Q

Define: Decalcification

A

A chemical process that breaks down calcium carbonate

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4
Q

Define: Carbonic acid

A

Formed by the reaction of carbon dioxide and water

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5
Q

Define: Exoskeleton

A

The outer shell of a marine creature that is made of calcium carbonate

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6
Q

Define: Marine invertebrates

A

Ocean and sea creatures that do not have a backbone

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7
Q

Define: Nitric acid

A

Can be formed from a series of reactions in the atmosphere between nitrogen gas, oxygen gas, and water

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8
Q

Define: Sulfuric acid

A

Can be formed from a series of reactions in the atmosphere between sulfur, oxygen gas, and water

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9
Q

Natural
rainfall(adj.) definition

A

-Natural rainfall(adj.)=Water falling from
the sky, through the water cycle

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10
Q

Dissolves(v.)
definition

A

-Dissolves(v.)=Becomes mixed and included in
the liquid

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11
Q

Atmosphere(n.)
definition

A

-Atmosphere(n.)=Mass of gas that surrounds
the earth

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12
Q

Emission(n.)
definition

A

-Emissions(n.)=something being released or
discharged

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13
Q

how is acid rain formed

A

CO2(g) + H2O(l) ⇌H2CO3(aq) ⇌ H+(aq) + HCO3−(aq)

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14
Q

how does human activity create more acid rain ()()()()()()()

A

combustion of fossil fuels increases the acidity of rainwater. there are several acids that make up what is known as acid rain

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15
Q

how is dilute sulfuric acid in the atmosphere created

A

S(s) + O2(g) → SO2(g) =combustion(Sulfur present in fossil fuels)
SO2(g) + H2O(l) ⇌H2SO3(aq) =react with water in atmosphere
2H2SO3(aq) + O2(g) ⇌ 2H2SO4(aq) =react with oxygen in atmosphere

Overall simplified reaction=
2SO2(g) + O2(g) + 2H2O(l) ⇌2H2SO4(aq)

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16
Q

where does dilute nitric acid originate from

A

combustion of fossil fuels like petrol and diesel from vehicles

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17
Q

how is dilute nitric acid in the atmosphere created

A

N2(g) + O2(g) → 2NO(g) =combustion(nitrogen present in the atmosphere)
2NO(g) + O2(g) → 2NO2(g) =combustion
H2O(l)+ 2NO2(g)⇌HNO2(aq) + HNO3(aq) =react with water in atmosphere
2HNO2(g) + O2(g) → 2HNO3(aq) =react with oxygen in atmosphere

Overall simplified reaction=
2N2(g) + 5O2(g) + 2H2O(l) ⇌4HNO3(aq)

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18
Q

how are aluminium ions released into the soil

A

Al(OH)3(s) + 3H+(aq) → ←Al3+(aq) + 3H2O(l)

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19
Q

what are some effects of acid rain

A

• Vegetation is widely affected as the acidic rainwater causes metal ions(Ca2+, K+, Mg2+) like aluminium that are normally bonded in a compound to become aqueous ions that are able to be absorbed by plants.
-E.g. Of acid rain(acid-base reaction) releasing aluminium ions into the soil=Al(OH)3(s) + 3H+(aq) ⇌ Al3+(aq) + 3H2O(l)

• damage to the waxy layer on the leaves of plants which may eventually lead
to the death of the plant
• acid rain runoff which can also cause the acidification of lakes, reducing the pH
to the extent that it can harm or kill aquatic life,
• and reactions with metals that are exposed to the weather.
•cave formation
•statue and building weathering

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20
Q

how does sulfuric and nitric acid react with limestone

A

CaCO3(s) + H2SO4(aq) → CaSO4(aq) + CO2(g) + H2O(l)
CaCO3(s) + 2HNO3(aq) → Ca(NO3)2(aq) + CO2(g) + H2O(l)

-cave formation
-statue and building weathering

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21
Q

what is the pH of sea water

A

around pH8

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22
Q

what happens when CO2 is absorbed by oceans

A

when CO2 is absorbed by oceans, reactions occur that reduce pH, carbonate ion concentration and the insolubility of calcium carbonate

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23
Q

how much man made carbon dioxide emissions have been dissolved by the oceans

A

30%

24
Q

how does decalcification occur

A

calcium carbonate is a base that reacts with weak acids. As the oceans become more acidic, creatures with exoskeletons are increasingly unable to grow and maintain the structure of their shells and exoskeletons due to their shells slowly dissolving

25
Q

Calcification reaction

A

Ca 2+(aq) + CO3 2-(aq) → CaCO 3-(s)

26
Q

decalcification reaction

A

CO2 (g) + H2O(l) ⇌ H2CO3(aq)
H2CO3(aq) ⇌ HCO3 -(aq) + H +(aq)
H +(aq) + CaCO3(s) → HCO3 -(aq) + Ca 2+(aq) =will dissolve away in water + dissolves skeletal structure and shells with more H+ in water.

27
Q

affect on CO2 in ocean reducing calcification

A

CO2 (g) + H2O(l) ⇌ H2CO3(aq)
H2CO3(aq) ⇌ HCO3 -(aq) + H +(aq)
H +(aq) + CO3(aq) → HCO3 -(aq)=not usable to create calcium carbonate shell

28
Q

Natural rainfall
is normally slightly acidic why?

A

-Natural rainfall
normally slightly acidic= water dissolves carbon dioxide from the air to
produce carbonic acid(H2CO3)

29
Q

Acidic rainfall is
acidic why?

A

-gases in atmosphere combine with water vapour, and then precipitate as dilute sulfuric acid or dilute nitric acid: This is acid rain.

30
Q

Difference between
natural rainfall and acidic rainfall

A

Natural rainfall
is acidic only from CO2 dissolving within water in the atmosphere and
reacting to produce H2CO3.

Acidic rainfall is
far more acidic than natural rain, and is caused buy sulfur dioxide and
nitrous oxide reacting with water in the atmosphere to produce sulfuric acid
or nitric acid.

31
Q

Natural sources of
emission include

A

-Emissions from
volcanoes and biological processes that occur on the land, in wetlands, and
in the oceans contribute acid-producing gases to the atmosphere.

32
Q

Human sources of
emission include

A

-Industrial
factories power-generating plants and vehicles

33
Q

Is carbonic acid
weak or strong

A

Carbonic acid= a
weak diprotic acid

34
Q

what does carbonic
acid produce when it reacts with water

A

:hydronium ions
:hydrogen
carbonate ions
:carbonate ions

35
Q

Chemical reaction
of CO2 in oceans

A

-in
oceans=CO2(g) + H2O(l) ⇌ H2CO3(aq) ⇌ H+(aq) + HCO3− (aq)

36
Q

Some random facts
if you want

A

-Historically,
there has been a balance between carbon dioxide being generated, and carbon
dioxide being dissolved.
-excess human made
CO2=result in ocean becoming more acidic.
-30% of human made
CO2 has been dissolved in the oceans.

37
Q

What is the
negative impacts of ocean acidification

A

-Marine
Invertebrates have shells(exoskeletons)= made of calcium carbonate.
-shells made from a process= calcification
-calcium
carbonate=base that reacts with weak acids
-ocean becoming
more acidic= creatures are increasingly unable to grow their shells and
exoskeletons, as well as their shells slowly dissolving=decalcification

38
Q

Why do marine organisms undergo calcification

A

-Marine organisms, such as invertebrates= use calcium ions and carbonate ions to protect themselves with layers of calcium carbonate(base), creating a shell or an exoskeleton for themselves.

39
Q

What is the increased acidity of oceans doing to the aquatic ecosystem

A

-this causes acid to react with invertebrates protective layer and dissolve away their protective layer.

Deep dive=
-reduced carbonate ion concentration impairs the ability of some organisms to build and maintain calcium carbonate structures(shells), disallowing creatures to protect themselves from pray, or grant them enough protection to survive in the harsh aquatic environments their habitat is situated.

Decreasing ocean pH levels can cause food chains to be affected as plankton populations will decrease, depleting a major food source for many predators.

-Lower biomass, diversity and complexity of algae present
-Loss of large algal habitats and the spread of fast-growing, small opportunistic species.

-habitat degradation and loss of biodiversity

40
Q

Are all acid base
reactions reversible(DON’T TAKE THIS ANSWER TO HEART BUT ITS GOOD FOR UNDERSTANDING)

A

Acid base reactions are reversible and therefore equilibrium reactions.

https://www.alchem.ie/blog/equilibrium-acid-base#:~:text=Acid%20base%20reactions%20are%20reversible,we%20look%20at%20the%20Ka.

Neutralization reactions are reversible. In theory, at least, even if not so much in practice, all reactions are reversible.

https://chemistry.stackexchange.com/questions/57814/why-arent-neutralisation-reactions-reversible#:~:text=Neutralization%20reactions%20are%20reversible.,that’s%20a%20one%2Dway%20door.

41
Q

Acids with one
replaceable hydrogen is called(two names)

A

Monoprotic or
Monobasic acids.

-theses names
interlinked with=
:The
number of replaceable hydrogens in the formula of an inorganic acid is called
Basicity.Basicity is also known as Proticity

42
Q

Monoprotic
definition

A

Acids with one replaceable hydrogen

43
Q

Monobasic
definition

A

Acids with one
replaceable hydrogen

44
Q

What does red
litmus paper indicate

A

Red litmus paper
can only indicate whether the soil has a pH of above or below 7(EMPHASIS ON
7)

45
Q

Indicator vs
Calibrated pH meter accuracy and precision

A

Indicator=
-Accuracy: low
-Precision: low

Calibrated pH
meter=
-Accuracy: high
-Precision: high

46
Q

What is rain’s
natural ph

A

-rain naturally
has a ph of 5-6

47
Q

Why does CO2
dissolve in oceans

A

Oceans are
slightly basic, allowing CO2 to dissolve within it.

48
Q

Calcification
chemical formula simplified

A

Ca 2+(aq) + CO3
2-(aq) → CaCO 3-(s)

49
Q

Decalcification
chemical formula simplified

A

CO2(g) + H2O(l) + CaCO3(s)⇌2HCO3-(aq)+ +
Ca 2+(aq)

50
Q

THIS HAS NOTHING TO DO WITH THIS CHPT!!!

What does the introduction of a different metal or carbon have on a metals structure???

A

The different atoms in an alloy are not identical in size and shape, which means they do not fit together as perfectly as the atoms in a pure metal. This results in a more irregular arrangement of atoms, which disrupts the crystal lattice structure.

51
Q

Take note of these

A

Heat conduction is
the ability for a substance to transfer heat.1Metals are good heat
conductors due to the delocalised electrons and close proximity of metal ions
to each other which enables heat, often in the form of kinetic energy, to be
rapidly transferred throughout the metal by the electrons moving about or by
vibrating metal ions.2

Specific heat capacity is the amount
of energy required to raise the temperature of 1 g of a substance by 1 ℃.1Metals have a low
specific heat capacity because they conduct heat very effectively which means
they require a small amount of heat energy to raise their temperature.2

52
Q

example of super acid

A

Perchloric acid, HClO4,->‘super acid’

53
Q

Example of super base

A

• Butyl lithium (n-BuLi )

54
Q

when pH increases by one, what factor does the strength of an acid or base change by

A

Since pH is a log function, a pH
decrease/increase by 1, means a change of a factor of 10

55
Q

What is the use of Limewater in lab experiments

A

Limewater is a saturated solution of calcium hydroxide, Ca(OH)2(aq), that will transition to a white ‘milky’ or ‘cloudy’ solution if CO2(g) is present. This is due to the precipitation of insoluble calcium carbonate, CaCO3(s), that becomes suspended in the solution.

56
Q

Kw at different
temperatures and the pH of water at different temperatures

A

-°C=0
-Kw(mol^2dm^-6)=0.114x10^-14
-pH=7.47

-°C=10
-Kw(mol^2dm^-6)=0.293x10^-14
-pH=7.27

-°C=20
-Kw(mol^2dm^-6)=0.681x10^-14
-pH=7.08

-°C=25
-Kw(mol^2dm^-6)=1.008x10^-14
-pH=7.00

-°C=30
-Kw(mol^2dm^-6)=1.471x10^-14
-pH=6.92

-°C=40
-Kw(mol^2dm^-6)=2.916x10^-14
-pH=6.77

-°C=50
-Kw(mol^2dm^-6)=5.476x10^-14
-pH=6.63

-°C=100
-Kw(mol^2dm^-6)=51.3x10^-14
-pH=6.14

57
Q

Why does the deprotonation of HSEO3- happen at a much lower extent to the deprotonation of H2SeO3

A

The deprotonated selenous acid, $$
, has a negative charge that can be thought of as electrostatically attracting and ‘holding on’ to the positive $$ion.1As such, it becomes more difficult for the positive $$ion to escape the pull of the remaining compound’s negative charge, resulting in fewer $$ molecules successfully losing both protons.2

chem unit 2 (7 decks)

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