Balance the following equations: (a) for the synthesis of...

Balance the following equations: (a) for the synthesis of urea, a common fertilizer $$\mathrm{CO}_{2}(\mathrm{g})+\mathrm{NH}_{3}(\mathrm{g}) \rightarrow \mathrm{NH}_{2} \mathrm{CONH}_{2}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\ell)$$ (b) for the reactions used to make uranium(VI) fluoride for the enrichment of natural uranium $$\begin{array}{c}\mathrm{UO}_{2}(\mathrm{s})+\mathrm{HF}(\mathrm{aq}) \rightarrow \mathrm{UF}_{4}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\ell) \\\mathrm{UF}_{4}(\mathrm{s})+\mathrm{F}_{2}(\mathrm{g}) \rightarrow \mathrm{UF}_{6 (\mathrm{s})\end{array}$$ (c) for the reaction to make titanium(IV) chloride, which is then converted to titanium metal $$\begin{array}{c}\mathrm{TiO}_{2}(\mathrm{s})+\mathrm{Cl}_{2}(\mathrm{g})+\mathrm{C}(\mathrm{s}) \rightarrow \mathrm{TiCl}_{4}(\ell)+\mathrm{CO}(\mathrm{g}) \\ \mathrm{TiCl}_{4}(\ell)+\mathrm{Mg}(\mathrm{s}) \rightarrow \mathrm{Ti}(\mathrm{s})+\mathrm{MgCl}_{2}(\mathrm{s})\end{array}$$

Balance the following equations:
(a) for the synthesis of urea, a common fertilizer $$\mathrm{CO}_{2}(\mathrm{g})+\mathrm{NH}_{3}(\mathrm{g}) \rightarrow \mathrm{NH}_{2} \mathrm{CONH}_{2}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\ell)$$
(b) for the reactions used to make uranium(VI) fluoride for the enrichment of natural uranium
$$\begin{array}{c}\mathrm{UO}_{2}(\mathrm{s})+\mathrm{HF}(\mathrm{aq}) \rightarrow \mathrm{UF}_{4}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\ell) \\\mathrm{UF}_{4}(\mathrm{s})+\mathrm{F}_{2}(\mathrm{g}) \rightarrow \mathrm{UF}_{6 (\mathrm{s})\end{array}$$
(c) for the reaction to make titanium(IV) chloride, which is then converted to titanium metal
$$\begin{array}{c}\mathrm{TiO}_{2}(\mathrm{s})+\mathrm{Cl}_{2}(\mathrm{g})+\mathrm{C}(\mathrm{s}) \rightarrow \mathrm{TiCl}_{4}(\ell)+\mathrm{CO}(\mathrm{g}) \\
\mathrm{TiCl}_{4}(\ell)+\mathrm{Mg}(\mathrm{s}) \rightarrow \mathrm{Ti}(\mathrm{s})+\mathrm{MgCl}_{2}(\mathrm{s})\end{array}$$

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Key Concepts

Conservation of Mass

This fundamental principle states that matter is neither created nor destroyed in a chemical reaction, meaning the number of atoms for each element must be the same on both sides of the equation. This concept forms the basis for balancing chemical equations.

Stoichiometry

Stoichiometry involves the quantitative relationship between reactants and products in a chemical reaction. It uses the coefficients in a balanced equation to calculate the amounts of substances consumed and produced, ensuring that the proportions reflect the law of conservation of mass.

Balancing Chemical Equations

Balancing chemical equations is the method of finding the correct coefficients for reactants and products so that the number of atoms of each element is equal on both sides. This skill is essential for accurately representing chemical reactions and reactions' stoichiometry.

Sequential Reactions Balancing

In cases where a product of one reaction is used as a reactant in a subsequent reaction, each individual reaction must be balanced independently, while also ensuring that the overall process maintains a consistent count of atoms. This concept is particularly important in multi-step synthesis processes.

Transcript

00:01 Hello everyone.

00:02 We're going to be balancing some chemical equations and these are actually pretty easy to balance and we've got a total of five that we're going to be looking at.

00:10 For the first reaction, we're looking at the production of urea, a common fertilizer.

00:16 That's this substance right here.

00:19 And if i do a quick visual atom inventory of this and i'll write it down for you.

00:26 I have one nitrogen on this side and i have two nitrogen right here and right here.

00:32 Can see i need a two here.

00:34 Now i will let you go through and do the rest of this atom inventory and you'll see that this one i believe is already balanced with just the addition of that one coefficient.

00:48 For the next set, this is the set of reactions, we're looking at the two reactions used to make the uranium six fluoride and that's used for enrichment of natural uranium.

01:02 So for my first reaction, i'm going to look at the fluorine.

01:08 I have one on this side.

01:09 I have four on this side, which means i need a four right there, and i believe that would give me a two right here.

01:22 And that should be good for this reaction.

01:26 Now let's look at the second reaction.

01:28 Oh, magic.

01:30 It's already balanced.

01:32 A, b, for already balanced...