The Extraction of Iron (GCSE Chemistry)
Summary
TLDREste vídeo educativo, dirigido a estudiantes de GCSE, explica el proceso de extracción del hierro en un alto horno, una de las industrias más importantes del mundo. Cubre los materiales necesarios como el mineral de hierro, coque, cal y aire caliente, y describe las reacciones de combustión, reducción, descomposición y neutralización que ocurren. Detalla cómo el coque actúa como combustible y agente reductor, y cómo la cal elimina impurezas formando escoria. Además, se menciona el papel del hierro en la fabricación del acero y cómo la variación de carbono y otros elementos afecta sus propiedades.
Takeaways
- 🔍 El proceso de extracción de hierro en un alto horno es fundamental para comprender la industria del acero.
- 🌟 Los materiales básicos necesarios para la producción de hierro son el mineral de hierro (hematites), coque, cal y aire caliente.
- 🔥 El coque actúa como combustible y agente reductor, proporcionando el calor necesario para alcanzar temperaturas de 1500 grados Celsius.
- ⚛️ La reacción química clave en el alto horno es la reducción del óxido de hierro por monóxido de carbono, lo que produce hierro y dióxido de carbono.
- 📝 Se deben poder escribir ecuaciones químicas y de palabras para describir las reacciones ocurriendo en el alto horno.
- 🔄 El proceso del alto horno es continuo, operando las 24 horas del día para evitar enfriamientos y mantener la temperatura óptima.
- 🏗️ El resultado final son dos líquidos: el hierro fundido y la escoria, donde la escoria es un subproducto que se puede vender para la construcción de carreteras y otros usos.
- 🗻 La cal se utiliza para eliminar las impurezas presentes en el mineral de hierro, reaccionando con el dióxido de silicio para formar escoria.
- 🔩 La producción de acero es un proceso que sigue al del alto horno, donde se añade oxígeno para reducir el contenido de carbono y a veces se añaden otros metales para dar propiedades específicas.
- 🛠️ Las propiedades del acero varían según el contenido de carbono y otros elementos, lo que permite adaptar el acero a una amplia gama de aplicaciones.
Q & A
¿Cómo se extrae el hierro del mineral de hierro en un alto horno?
-El hierro se extrae del mineral de hierro en un alto horno a través de un proceso de reducción que utiliza carvón como agente reductor y combustible, y caliza para eliminar impurezas.
¿Cuáles son los productos finales del proceso de extracción de hierro en el alto horno?
-Los productos finales del proceso de extracción de hierro en el alto horno son el hierro fundido y la escoria, que es un subproducto que se puede vender para su uso en la construcción de carreteras, en la fabricación de cemento y concreto, e incluso como fertilizante para pastizales.
¿Qué es la escoria y cómo se forma?
-La escoria es un subproducto que se forma durante el proceso de extracción del hierro en el alto horno debido a las impurezas presentes en el mineral de hierro. Se forma cuando el óxido de silicio y otros minerales impuros reaccionan con el óxido de calcio proveniente de la caliza para formar silicio y calcio silicado.
¿Cuál es el papel de la cal en el proceso de extracción de hierro?
-La cal, en forma de cálculo de calcio (CaCO3), se descompone en el alto horno debido al calor intenso para formar óxido de calcio (CaO), que luego reacciona con las impurezas de dióxido de silicio para formar escoria. Este proceso es una reacción de descomposición térmica.
¿Cómo se produce el agente reductor, el monóxido de carbono, en el alto horno?
-El monóxido de carbono se produce cuando el dióxido de carbono reacciona con más carbón en presencia de altas temperaturas en el alto horno. Este monóxido de carbono es el agente reductor que permite que el óxido de hierro se reduzca a hierro.
¿Qué tipo de reacciones químicas ocurren dentro del alto horno durante el proceso de extracción de hierro?
-Dentro del alto horno se producen reacciones de combustión, reducción, descomposición y neutralización. La combustión se da cuando el carvón quema en oxígeno, la reducción cuando el monóxido de carbono reacciona con el óxido de hierro, la descomposición cuando la caliza se calienta y se convierte en óxido de calcio y dióxido de carbono, y la neutralización cuando el óxido de calcio reacciona con el dióxido de silicio para formar escoria.
¿Por qué se requiere aire caliente en el proceso de extracción de hierro en el alto horno?
-El aire caliente es necesario para que el carvón queme eficientemente y alcance las altas temperaturas requeridas en el alto horno (aproximadamente 1500 °C). Estas temperaturas son esenciales para que los procesos químicos se realicen correctamente y se produzca hierro fundido.
¿Cuál es la importancia del hierro en la industria y para qué se usa?
-El hierro es uno de los metales más importantes en la industria y se usa para producir acero, que a su vez es fundamental en la fabricación de una amplia variedad de productos, como automóviles, puentes, edificios, hornos, microondas, lavadoras, etc.
¿Cómo se transforma el hierro extraído en el alto horno en acero?
-El hierro extraído en el alto horno contiene alrededor del 3 al 4% de carbón y otros no metales, lo que lo hace muy frágil. Para transformarlo en acero, se le oxigena para quemar el carbón y se le añaden otros metales para darle propiedades específicas, como en el caso del acero inoxidable, que contiene cromo y níquel para resistir la corrosión.
¿Cuál es la relación entre el contenido de carbón en el acero y sus propiedades mecánicas?
-El contenido de carbón en el acero afecta sus propiedades mecánicas; un contenido más alto de carbón hace que el acero sea más duro pero también más frágil. Por otro lado, un contenido más bajo de carbón produce un acero que no es tan frágil y puede ser moldeado más fácilmente.
Outlines
🔥 Proceso de extracción de hierro en un alto horno
Este párrafo introduce el proceso de extracción de hierro en un alto horno, adecuado para estudiantes de GCSE. Se espera que los estudiantes puedan explicar cómo se extrae el hierro del mineral de hierro en un alto horno, identificar las reacciones de combustión, reducción, descomposición y neutralización que ocurren dentro del mismo, y escribir ecuaciones químicas y de palabras para describir dichas reacciones. Se discute la relación entre la reactividad de un metal y la facilidad de su extracción, destacando que los metales del medio de la serie de reactividad pueden ser extraídos por reducción usando un agente reductor. El vídeo se centra en el hierro, uno de los metales más importantes utilizados en la producción de aceros. Los materiales necesarios para la producción de hierro incluyen mineral de hierro (hematita), coque,石灰石 y aire caliente. Se describen brevemente estos materiales y su papel en el proceso.
📚 Reacciones químicas en el alto horno
En este segundo párrafo, se explica con más detalle las reacciones químicas que ocurren en el alto horno durante la extracción de hierro. Se mencionan las ecuaciones químicas y de palabras para las reacciones de combustión del coque, la formación de monóxido de carbono y su reacción con el óxido de hierro para producir hierro y dióxido de carbono. Se destaca la importancia de las ecuaciones químicas para los estudiantes de nivel superior de GCSE y se ofrece orientación sobre cómo practicar la escritura de estas ecuaciones. Se presenta un diagrama del alto horno y se describe el proceso continuo de extracción, incluyendo la formación de slag debido a las impurezas en el mineral de hierro y su eliminación. Además, se discute el papel de la limestone en la eliminación de las impurezas, su descomposición en el alto horno y su reacción con la sílice para formar slag.
🛠 Uso del slag y la producción de acero
Este tercer párrafo explora el uso del slag, un subproducto del proceso de extracción de hierro, que se puede vender para su uso en la construcción de carreteras, en cemento y concreto, e incluso como fertilizante para pastizales. Se presentan ecuaciones químicas y de palabras que describen cómo la calcita se descompone en el alto horno para formar óxido de calcio y dióxido de carbono, y cómo el óxido de calcio reacciona con la sílice para formar slag. Se describe la slag como un producto económico importante. Además, se menciona la transformación del hierro extraído en el alto horno, que contiene alrededor del 3-4% de carbono, en acero a través del proceso de oxidación y la adición de otros metales para mejorar sus propiedades, como el cromo y el níquel en el acero inoxidable.
📊 Propiedades del acero y prácticas de preguntas
Este cuarto párrafo se enfoca en cómo las propiedades del acero varían con el contenido de carbono y la adición de otros elementos, como el cromo y el níquel, para crear acero inoxidable. Se presenta una tabla que muestra los efectos del contenido de carbono en las propiedades del acero, incluyendo la dureza y la fragilidad. Además, se presentan preguntas de práctica para los estudiantes, incluyendo la identificación de los materiales de entrada y su uso en el proceso de extracción de hierro, la escritura de ecuaciones químicas y la descripción de cómo el tensión changes strength varía con el aumento del porcentaje de carbono en el acero. Se utiliza un gráfico para ilustrar estos cambios y se ofrece orientación sobre cómo los diferentes tipos de acero se utilizan en aplicaciones específicas, como el uso de acero inoxidable para la fabricación de recambios de cadera.
🏆 Resumen y recursos adicionales
El último párrafo resume los objetivos del vídeo y proporciona un recordatorio de lo que los estudiantes deberían ser capaces de hacer al final de la lección, como explicar el proceso de extracción de hierro, identificar las reacciones químicas que ocurren en el alto horno y escribir ecuaciones químicas y de palabras para describir estas reacciones. Además, se invita a los estudiantes a explorar el canal de YouTube y la cuenta de Twitter del presentador para obtener más información y recursos sobre química.
Mindmap
Keywords
💡Extracción de hierro
💡Alto horno
💡Reacciones químicas
💡Agente reductor
💡Óxido de hierro
💡Coque
💡Cal
💡Escoria
💡Acero
💡Reacciones de combustión y oxidación
Highlights
Extracción de hierro a través del proceso de alto horno es fundamental para estudiantes de GCSE.
El proceso de alto horno involucra reacciones de combustión, reducción, descomposición y neutralización.
Los metales del medio de la serie de reactividad pueden ser extraídos por reducción usando un agente reductor.
El hierro es un metal clave en la industria y es fundamental para la fabricación de acero.
El proceso de alto horno requiere de mineral de hierro, coque, cal y aire caliente.
El coque actúa como combustible y agente reductor en el proceso de alto horno.
La cal se utiliza para eliminar impurezas del mineral de hierro.
El aire caliente es esencial para quemar el coque y alcanzar temperaturas altas en el alto horno.
La descomposición térmica de la cal en el alto horno produce óxido de calcio y dióxido de carbono.
El óxido de calcio reacciona con las impurezas de dióxido de silicio para formar escoria.
La reducción del óxido de hierro por monóxido de carbono produce hierro y dióxido de carbono.
El proceso de alto horno es continuo y opera las 24 horas del día.
La escoria es un subproducto del proceso que se puede vender para construir carreteras y otros usos.
El hierro producido en el alto horno contiene alrededor del 3% a 4% de carbono y es muy frágil.
El hierro del alto horno se convierte en acero, una aleación de hierro y otros elementos, para mejorar sus propiedades.
El contenido de carbono en el acero afecta significativamente sus propiedades mecánicas.
El acero inoxidable contiene cromo y níquel, lo que le confiere propiedades anti corrosivas.
Las reacciones químicas en el alto horno incluyen la combustión del coque, la reducción del óxido de hierro y la formación de escoria.
Los estudiantes deben ser capaces de escribir ecuaciones químicas y descriptivas para las reacciones del proceso de alto horno.
Transcripts
welcome to our latest video on the
extraction of iron the blast furnace
process this video is suitable for GCSE
students
by the end of this video lesson you
should be able to explain how iron can
be extracted from iron ore in a blast
furnace you should be able to identify
that within the blast furnace we have
combustion reduction decomposition and
neutralization reactions and you should
be able to write word and chemical
equations to describe the reactions
taking place
in our previous videos we discussed the
relationship between the reactivity of a
metal and the ease at which it can be
extracted from its source and we learnt
that metals at the bottom of the
reactivity series are the easiest to
extract because they are found as
elements metals at the top of the
reactivity series at a hardest to
extract they found as compounds and
they're also found as most stable
compounds so elements such as potassium
sodium calcium magnesium aluminium they
have to be extracted using electricity
by a process called electrolysis now
it's these metals in the middle of
reactively series that can be extracted
by reduction using a reducing agent and
we're going to focus on one of these
metals iron in this video lesson
the extraction of iron is one of the
world's most important industrial
processes iron is one of the most
important metals and it's used to make
the alloy steel now steel is an alloy
because it's a mixture of iron and other
elements now we rely on steel to make
cars bridges buildings ovens microwaves
washing machines etc iron is made in a
process called the blast furnace process
and the raw materials that we need to
make iron are iron ore coke limestone
and hot air before we talk in detail
about how this process works let's
discuss some of these raw materials so
if we start with the iron ore so that
obviously is our source of iron and the
all that they use to extract iron is
called hematite and we've discussed that
all previously coke is a form of carbon
and this is used in the process as a
fuel because we need a lot of heat in a
blast furnace you're talking about
temperatures around 1500 degrees C so
burn in coke burning carbon releases a
lot of heat and it's also used to make
carbon monoxide which is the reducing
agent in this process now you remember a
reducing agent is a substance that
causes another to lose oxygen look at
the overall equation we have iron oxide
reacting with carbon monoxide to form
iron and carbon dioxide so the carbon
monoxide is classed as a reducing agent
because it causes the iron oxide to be
reduced to lose oxygen to form iron
now the other raw materials are
limestone which is used to remove
impurities and we'll discuss this later
and hot air now hot air is needed for
the coke to burn and remember the coke
is a fuel that supplies the high
temperatures needed for the blast
furnace to work and it also makes carbon
monoxide
when the coke burns so that's what the
hot air does and the reason that we need
hot air and not air is because high
temperatures mean a faster reaction and
the furnace operates around about 1,500
degrees C
so on this slide we have some of the
chemical reactions taking place in the
blast furnace so coke carbon burns in
oxygen to form carbon dioxide and when
it does so it releases heat energy and
obviously that's why we're able to get
such high temperatures in the blast
furnace and Coke is our fuel now this
reaction is a combustion reaction
because we burnt a fuel in a good supply
of oxygen and we've generated heat
energy now the carbon dioxide reacts
with more carbon to form carbon monoxide
and it's the carbon monoxide that reacts
with our iron oxide to form iron and
carbon dioxide now we've written down
both the chemical and word equations
here and if you are a student studying
higher GCC you would be expected to
write chemical equations to describe
these reactions you should also be able
to spot reduction and oxidation taking
place so if we look at the first
equation you can see carbon is gained in
oxygen when it forms carbon dioxide it's
being oxidized oxidation is a gain of
oxygen and once again if we look at the
overall equation we see that iron oxide
loses oxygen it's reduced to form iron
what causes this reduction the reducing
agent carbon monoxide and the carbon
monoxide gains oxygen to form carbon
dioxide and the carbon monoxide is
oxidized
now in this video I've written the
chemical equations for you however you
would be expected to write chemical
equations in the GCC exam if you're a
higher tier student therefore it's
important you practice a skill now to
help you we have made a series of videos
on the YouTube channel to enable you to
practice how to write chemical equations
and how to write balanced chemical
equations please look at these videos
because this skill is a very important
skill that you need to master
so now let's look at a diagram of a
blast furnace
so in the top of the blast furnace you
put the raw materials iron ore in the
form of hematite coke and limestone and
hot air is blasted into the furnace
now when the coke is in the furnace it
burns in the form of a combustion
reaction and produces carbon dioxide and
when it reacts then with more carbon it
forms carbon monoxide and it's the
carbon monoxide that reacts with the
iron oxide from the iron ore to produce
iron and carbon dioxide now this is a
continuous process and what we mean by
that is it operates 24 hours a day
we don't cool the furnace down it's kept
at 1500 degrees C the coke remember is
our fuel is producing lots and lots of
heat and we end up with liquid iron
molten iron melted iron and a material
called slag now the slag forms because
of impurities in the iron ore now
remember iron all is iron oxide and then
you have the rock so you are going to
get impurities and the slag is formed in
this process and has to be removed from
the iron now the slag itself is a
byproduct of this process so it's a
product that we can actually sell and we
can actually make money from it so it's
economically important now the iron that
is produced is in the liquid state and
when you look at your diagram you can
see that the molten iron is heavier than
the slag and therefore the slag is on
top of the molten iron so the slag would
be removed and the molten iron would be
removed and the liquid iron then could
be cooled down in various castes
and you could form like slabs or strips
of iron
now let's focus on the role of limestone
so limestone is used to remove the
impurities that exist in iron ore and
limestone is calcium carbonate and has a
formula caco3 and as I mentioned iron
ore contains impurities of silicon
dioxide and in a blast furnace these are
removed in a two-part stage so the first
thing that happens it in a blast furnace
calcium carbonate limestone breaks down
because of the intense heat into calcium
oxide and carbon dioxide and it's the
calcium oxide then reacts with the sand
impurities the silicon dioxide
impurities to form the substance called
slag which can then be removed now when
calcium carbonate breaks down into
calcium oxide and carbon dioxide this is
called a thermal decomposition reaction
and this is a type of reaction you would
have studied previously
so this picture shows molten slag that
has been removed from the blast furnace
and it will cool down and solidify and
then the slag can be sold to various
companies because it's a product for
road building is used as an aggregate in
cement and concrete and it even has
fertilizer properties and it could be
used to act as a fertilizer for
grassland now on the slide we have the
word equations and the chemical
equations to describe how this process
works so calcium carbonate breaks down
into calcium oxide and carbon dioxide
because of the intense heat in a blast
furnace now this reaction is called
thermal decomposition because you're
breaking a compound down using heat the
calcium oxide then can react with the
silicon dioxide the sand impurities and
form calcium silicate which is commonly
known as slag
now calcium oxide is a metal oxide and
metal oxides are bases now you remember
that a base is the opposite of an acid
silicon dioxide is a non-metal oxide and
non metal oxides are either acidic or
neutral now silicon dioxide is acidic so
if you react calcium oxide a basic oxide
with silicon dioxide an acidic oxide the
acid and base cancel each other out and
we have a neutralization reaction taking
place now once again I've included both
the chemical equations and the word
equations to describe the reactions
taking place now you will be required to
be able to write chemical equations and
word equations for these reactions now
this slide is a nice summary of all the
chemical reactions that take place in
the blast furnace and you can see that
iron ore coke and limestone are put into
the top of the furnace now if you work
in the blast furnace process they call
this the charge and hot air is blasted
into the furnace you can see the
temperature in the furnace gets as hot
as 1500 degrees C molten slag and iron
ore are the products here and these are
both in liquid state the role of the
limestone is shown clearly here it
breaks up into calcium oxide and carbon
dioxide and the calcium oxide reacts
with the sand impurities to form slag
and you can see also how the reducing
agent carbon monoxide is also formed
go back to our original diagram the
blast furnace you can see that the
molten iron and the slag are formed and
the slag forms on top of the molten iron
and these would both be removed the
molten iron could be removed for further
processing to make steel and the slag
can be removed cooled down and then used
as a byproduct and sold to companies as
road building material or as an
aggregate for concrete or as I mentioned
previously
sometimes slag can be used as a form of
fertilizer so this slide summarizes the
different uses of slag and also it
reinforces the fact that the blast
furnace process is a continuous process
with new raw materials added and
products removed all the time due to the
time and cost associated with getting
the furnace up to a temperature of 1500
degrees C remember that iron oxide is
reduced in the process as it loses
oxygen and the carbon monoxide is
oxidized as it gains oxygen and the
carbon monoxide is a reducing agent
now I mentioned at the start of the
video that iron is used to make steel
and the iron you get from the blast
furnace is impure it contains around 3
to 4 percent carbon and some other
nonmetals and the impure iron is very
brittle it means that if you try and
shape it it sort of shatters now most of
the iron that's made in the blast
furnace does get turned into the alloy
steel and remember steel is a mixture of
iron and other elements and that's what
an alloy is it's a mixture of a metal
and other elements and in steel usually
there's over 98% iron content and it
will also have tiny amounts of carbon
left in it in most Steel's and some
other metals can be added to it as well
now the amount of carbon and other
elements in the steel dramatically
affect the properties
now this is a good thing and this is why
steel is more useful an iron because we
can vary the amount of carbon and we can
vary the amount of other elements
present in the steel and we can
fine-tune the properties to what we want
and different customers for steel will
require different properties having a
high carbon content in the steel
constraint ffunny and it gives the
ability to harden it by heat treatment
however it makes it less ductile and
more brittle as a result
although you're not required to know how
to make steel in any great detail I do
think it's useful to know that the iron
that you make in the blast furnace has
around three to four percent carbon in
it and it's important to remove that
carbon to get steel that is less brittle
and they do that simply by just blowing
in oxygen and then the carbon gets
removed because it burns to form carbon
dioxide and other metals are added to
the steel to give it other properties so
you might add a bit of chromium in a bit
of nickel because you might not want the
steel to rest if you make in stainless
steel and that would be useful if you
were making say cutlery because you
would want steel that didn't rest when
it came into contact with water so that
is essentially what they do when they
make steel
so the following table shows what
happens to the properties of Steel when
you all to the carbon content so you can
see that mild steel has only about
naught point two five percent carbon and
the result of that is it's not brittle
and it can be shaped whereas if you had
a high carbon steel although it would be
very hard it would also be quite brittle
as well we mean it would be difficult to
shape and you can see if you add
elements such as chromium and nickel you
can end up with stainless steel and
that's a lot tougher and it doesn't
corrode it doesn't rest and that would
be useful for certain products so now
we're going to test your understanding
of this video lesson with some practice
questions so here's the first practice
question and this comes in two parts so
we like to pause the video
have a go this part of the question and
then we'll then look at the second part
of the question pause the video have a
go the question now this is the second
part of question one once again pause
the video have a good the question and
then we'll go for the answers to the
whole question see how you got on with
question one you asked to match the raw
materials to its use so iron ore is a
source of iron a limestone removes
impurities and coke acts as a fuel if
you've got all three correct two marks
any one correct one mark now let's look
at the word equation so you had carbon
plus oxygen goes to carbon dioxide one
mark for that
so let's look at the second part of
question one you're asked to give the
letter of the arrow which shows
reduction taking place
it's arrow a and this is because iron
oxide loses oxygen you get one mop for
saying a and one mark for the idea that
it's iron oxide losing oxygen or if you
said there's a loss of oxygen taking
place that would give you the mark now
Part D is asking you to choose a term
from the box which best describes an
alloy well that would be mixture because
alloys are mixtures they're mixtures of
metals and other elements
so now have a go at question two so read
the question pause the video and have a
go at it and this question is in three
parts once you've done all three parts
we'll go for the answers
so here is the second part of question
to pause the video and have a go at this
question
and here's the final
question two once again pause the video
and have a go at this last part of
question two
so now let's go for the answers to
question two so the reason that we add
coke to the blast furnace is because it
acts as a fuel or you can say it makes
the reducing agent carbon monoxide and I
think they would also accept if you said
that it releases heat and we need a high
temperature in the blast furnace that
would be fine as well
that gets you one mark for that now the
reason that we need limestone is it
removes impurities and you could say
remove sand or and remove silica but
this idea of removing impurities gets
you a mark for that and to balance the
chemical equation we need to put a 3 in
front of carbon monoxide CO so it's fe 2
o 3 + 3 Co and we have 2 fe 2 iron and 3
carbon dioxide molecules and if you do
this the equation is balanced now this
equation is balanced because I have a
total of 2 iron atoms on either side of
the equation I have a total of 6 oxygens
on the left because I have oh 3 in Fe 2
O 3 + 3 Co so that's six oxygens and I
have six oxygens now on the right
because it's three co 2 so 3 times 2 is
6 and the carbons are also balanced
because I have 3 carbons on the left and
3 on the right now given chemical name
of the substance which is reduced in the
furnace it is iron oxide or you could
say iron 3 oxide because remember the
iron in iron oxide is fe 3 plus the most
stable form of iron so they will accept
iron oxide or iron 3 oxide
now let's go through this second part of
question two it's asking you to describe
how the tensile strength changes as a
percentage of carbon present increases
well you can see from the graph there it
increases and then decreases so that
would get you a mark for saying that but
there's two marks for this question so
you need to use numerical data to get
the two marks so if you said that the
tensile strength increases to a maximum
with naught point eight percent carbon
and then decreases that would get you
the second mark or alternatively you
could say that it increases to a tensile
strength of 800 MPA and then decreases
both would be fine for the second mark
now for the final part of question two
you're asked to use the graph and the
table two namely alloy which has the
lowest tensile strength now you remember
that tensile strength increases up to a
maximum when you get tuned or 0.8
percent carbon and then it decreases
after that so the alloy which has the
lowest tensile strength will be cast
iron because that's got three point six
percent carbon and if you go to your
graph you will see that three point six
percent carbon has a tensile strength of
just over 200 MPA which is the lowest of
those alloys listed in the table
so here's a final question we would like
you to either go up so pause the video
read through the question have a go at
it and then we'll go for the answers
so in question three you're asked to use
the table to answer the questions so two
effects of increasing the percentage of
carbon in steel you increase the
hardness when you increase the
percentage of carbon and you make it
more brittle so one mark for if you said
it gets harder or increases hardness and
the second mark if you said it becomes
more brittle so for part two you had to
choose which type of steel you would use
to make our bodies and hip replacement
joints so you would use mild steel for
car bodies because it's important that
you can shape them and that's the form
of Steel that's easy to shape so that's
why you use mild steel and the reason
it's easily shaped and for hip
replacement joints you would use
stainless steel because it's tough and
doesn't corrode it doesn't rest
a video lesson and all this left is
first to recap the lesson objectives so
you should now be able to explain how
iron can be extracted from iron ore in a
blast furnace you should be able to
identify that within the blast furnace
we have combustion reduction
decomposition and neutralization
reactions and you should be able to
write word and chemical equations to
describe the reactions taking place
so that concludes our video please check
out our YouTube channel Doctorow
chemistry and our Twitter site which
contains lots of chemistry information
and links at radder chemistry
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