Write chemical equations for each of the following...

Write chemical equations for each of the following decomposition reactions. One or more products might be identified. $$\begin{array}{l}{\text { a. magnesium bromide } \rightarrow} \\ {\text { b. cobalt(II) oxide } \rightarrow} \\ {\text { c. titanium(IV) hydroxide } titanium (IV) oxide + water \rightarrow} \\ {\text { d. barium carbonate } \rightarrow \text { barium oxide }+\text { carbon dioxide }}\end{array}$$

Write chemical equations for each of the following
decomposition reactions. One or more products might
be identified.
$$\begin{array}{l}{\text { a. magnesium bromide } \rightarrow} \\ {\text { b. cobalt(II) oxide } \rightarrow} \\ {\text { c. titanium(IV) hydroxide } titanium (IV) oxide + water \rightarrow} \\ {\text { d. barium carbonate } \rightarrow \text { barium oxide }+\text { carbon dioxide }}\end{array}$$

Key Concepts

Decomposition Reaction

A decomposition reaction is a type of chemical reaction in which a single compound breaks down into two or more simpler substances. This type of reaction is typically achieved by applying heat, light, or electricity, and it is one of the fundamental reaction types in chemistry that helps illustrate how complex compounds are formed from or broken down into simpler components.

Chemical Equations

Chemical equations serve as a symbolic representation of what occurs during a chemical reaction. They use formulas to denote reactants and products, providing a concise way to visually communicate the substances involved in the reaction and the transformation process that takes place.

Balancing Chemical Equations

Balancing chemical equations is a crucial process in chemistry that ensures the law of conservation of mass is maintained. This involves adjusting the coefficients of reactants and products so that the number of atoms for each element is equal on both sides of the equation. It provides an accurate depiction of the stoichiometry involved in the reaction.

Reactants and Products

In any chemical reaction, reactants are the starting materials that undergo change, while products are the substances formed as a result of the reaction. Understanding the roles of reactants and products is key to analyzing how and why chemical reactions occur, and it forms the basis of predicting the outcomes of reactions.

Transcript

00:01 Okay, now we do problem 87.

00:03 Because this is decomposition, so one product gives us two more products, right? so the first one, we have magnesium bromide.

00:13 So magnesium doesn't matter, so we'll buy magnesium first, right? and bromide, that's ebr.

00:20 And we know magnesium gets two, right? and barium bromide, bromine get only one, so get two right here.

00:29 Keep in mind the formula right here.

00:32 A, b, so you go get the ab, right? the chart right here, so you will get a, b, and b, a.

00:42 So get two right here, and one right here.

00:46 Let me two plus right here, right? and minus in the group of the iron, so you have to remember all of them.

00:57 So one, we don't need to write.

00:59 So one will come here.

01:02 And one, you got to one here, right? so, but you don't need to write one.

01:08 Two, you will come here.

01:11 You have to write two, two, three, four, five, whatever.

01:13 You have to write.

01:14 One, we don't need to write.

01:16 And then manoeium bromide.

01:18 So mannesium bromide, when they did this compose, they will give you magnesium and bromine.

01:27 And after you try this, you have to balance, right? okay, so magnesium, that's equal, both sides equal.

01:43 So couple two oxide.

01:46 Couple two oxide.

01:48 So couple two right here.

01:49 Couple oxide.

01:52 Okay.

01:54 Because oxygen get two.

01:56 So couple get two.

01:58 So both of them two so you need to write because that equal...

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