Write balanced chemical equations for the following...

Write balanced chemical equations for the following reactions. (a) The reaction of aluminum and iron(III) oxide to form iron and aluminum oxide (known as the thermite reaction). (IMAGE CANNOT COPY) (b) The reaction of carbon and water at high temperature to form a mixture of gaseous $\mathrm{CO}$ and $\mathrm{H}_{2}$ (known as water gas and once used as a fuel). (c) The reaction of liquid silicon tetrachloride and magnesium forming silicon and magnesium chloride. This is one step in the preparation of ultrapure silicon used in the semiconductor industry.

Write balanced chemical equations for the following reactions.
(a) The reaction of aluminum and iron(III) oxide to form iron and aluminum oxide (known as the thermite reaction). (IMAGE CANNOT COPY)
(b) The reaction of carbon and water at high temperature to form a mixture of gaseous $\mathrm{CO}$ and $\mathrm{H}_{2}$ (known as water gas and once used as a fuel).
(c) The reaction of liquid silicon tetrachloride and magnesium forming silicon and magnesium chloride. This is one step in the preparation of ultrapure silicon used in the semiconductor industry.

Key Concepts

Oxidation-Reduction Reactions

Redox reactions, or oxidation-reduction reactions, involve the transfer of electrons between chemical species. Understanding the changes in oxidation states is crucial for writing and balancing such equations, as it ensures that both mass and charge are balanced in the overall reaction.

Stoichiometry and Balancing

Stoichiometry involves the quantitative relationships between reactants and products in chemical reactions. Balancing equations requires adjusting the stoichiometric coefficients so that the number of atoms of each element is conserved, ensuring that the mathematical representation adheres to the conservation of mass.

Chemical Equation Representation

Chemical equations are symbolic representations of chemical reactions where reactants are converted into products. These equations use chemical formulas and an arrow to denote the direction of the reaction, serving as a fundamental language for describing chemical processes.

Conservation of Mass

The principle of conservation of mass states that in any chemical reaction, matter is neither created nor destroyed. This means that the total number of atoms for each element must be identical on both sides of the equation, a foundational concept in balancing chemical equations.

Transcript

00:01 Hello everyone and thanks for joining me as we practice writing balanced chemical equations from word equations.

00:06 I'm going to have three equations that we're going to work with today and i'm going to summarize these for you.

00:13 Let's start with our first equation.

00:16 In this equation, we are told that we have a reaction of aluminum and iron three oxide.

00:23 So our reactants are aluminum and iron -3 oxide.

00:41 And we form, so this will be our products, we form iron and aluminum oxide.

00:57 Now for those of you who are interested, this is called the thermite reaction.

01:02 And i might not have a lot of room here so i'm going to switch colors.

01:05 Aluminum, we know, is a -l, and it's an s.

01:10 Iron is fe, it's also a solid.

01:15 Iron 3 oxide is f .e .2 .03.

01:23 And this is a solid as well.

01:26 And last but not least, aluminum oxide is al2 .03.

01:32 And this is also a solid.

01:35 So let's start.

01:37 We are going to, i'm going to put this in the middle so that i know what i'm doing.

01:42 I'm going to start by our reactants.

01:45 Aluminum reacts with iron three oxide.

01:55 And my products are iron, elemental iron, and aluminum oxide.

02:05 Okay, so i have three substances, aluminum, iron, and oxygen.

02:12 And let's do a quick inventory of how many of each of these we have.

02:15 I will use this color on this side.

02:19 So i have two aluminums, excuse me, not yet.

02:23 I have one aluminum, two irons, and three oxygens.

02:30 And let's use orange for this side.

02:35 Here i have one iron, two aluminums, and three oxygens.

02:41 So i have an unbalanced chemical equation.

02:45 And i'm going to put in black the four places that i can put a coefficient to balance this.

02:55 And then we're going to pick something that doesn't work out here.

02:57 In this case, aluminum's first.

03:00 I usually leave oxygens and or hydrogens till last, so i'm just going to pick aluminum.

03:05 We're going to balance aluminum first.

03:08 I have two aluminums on the product side and one here, so i will balance this by putting a two.

03:15 That means that this is now two, so aluminums are balanced.

03:20 Next, let's fix our fix, if you will, our irons.

03:26 Our irons, i have two on this side, one on this side, so i need a two right here.

03:33 And that will fix this.

03:35 Lo and behold, i'm done.

03:37 The balanced chemical equation, i'll write the whole thing out one more time.

03:44 That's an s.

03:45 I can't read my own writing...

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