Balancing Equations

<a name="top"></a> <center> <h1><font color="#000099"><img src="../../media/balequa/balequatitle.gif" alt="balequatitle.gif" width="292" height="102"></font></h1> </center> </font><table border="0" cellpadding="0" cellspacing="0" width="100%"> <tr><td valign="baseline" width="42"><img src="../../../../_themes/education/blbull1.gif" width="15" height="15" hspace="13"></td><td valign="top" width="100%"><a href="#what">What are Chemical Equations</a> <tr><td valign="baseline" width="42"><img src="../../../../_themes/education/blbull1.gif" width="15" height="15" hspace="13"></td><td valign="top" width="100%"><a href="#bal">Balancing Equations</a> <tr><td valign="baseline" width="42"><img src="../../../../_themes/education/blbull1.gif" width="15" height="15" hspace="13"></td><td valign="top" width="100%"><a href="#rxn">Types of Reactions</a> </table> <p align="center"><img src="../../../../_themes/education/blrule.gif" width="600" height="10"></p> <a name="what"></a> <center> <h2><font color="#0033CC">What are chemical equations?</font></h2> </center> <br> <p>A chemical equation is a symbolic representation of a chemical reaction in terms of chemical formulas. An example of a chemical equation would be:</p> <br> <center> 2Na + Cl<sub>2</sub> -> 2NaCl </center> <br> <p>This chemical equation would stand for the burning of sodium in chlorine to produce sodium chloride. The formulas on the left side of the equation would stand for the reactant. A reactant is the starting substance in a compound. The arrow, ->, means either "yields" or "reacts to form." The formulas to the right of the arrow stand for the product formed in the chemical reaction. A product is the substance that results from a chemical reaction. The coefficient in front of the Na, 2, give the number of molecules or formula units involved in the reaction. Coefficients of one are usually understood, so they are not written.</p> <p>Sometimes it helps to indicate the states or phases of the substances in a chemical reaction. We can do this by placing certain labels, which stand for the various phases, following the formula of a substance in a chemical equation. Here are the labels:</p> <center> </font><table border=0 cellspacing=4 > <tr> <td>(g)=gases</font></td> <td>(l)=liquid</font></td> <td>(s)=solid</font></td> <td>(aq)=aqueous solution</font></td> </tr> </table> </center> <p>When we use the labels which we have just learned our former equation becomes:</p> <br> <center> 2Na(s) + Cl<sub>2</sub>(g) -> 2NaCl(s) </center> <br> <p>In a chemical equation we can also indicate the conditions under which the reaction takes place. If the reactants in the chemical reaction are heated, we indicate this with the Greek symbol delta, <IMG src="../../media/balequa/lildelta.gif" alt="Little Delta" width="8" height="10">, over the arrow. Below is the equation that indicates that solid sodium nitrate, NaNO<sub>3</sub> decompposes when heated to give us solid solium nitrate, which is NaNO<sub>2</sub>, and good ole oxygen, which is O<sub>2</sub>.</p> <center> <IMG src="../../media/balequa/firstform.gif" alt="Equation" width="182" height="19"> </center> <br> <p>Oftentimes in chemical reactions there will be the addition of a catalyst. A catalyst speeds up a chemical reaction without being consumed in the overall reaction. Guess what, as you probably expected, there is a way to represent the addition of a catalyst to a chemical reaction. We do this by writing the catalyst involved in the reaction over the arrow. Here is an example, say that we have an aqueous solution of hydrogen peroxide, which is H<sub>2</sub>O<sub>2</sub>. When this solution of hydrogen peroxide is exposed to platinum metal (Pt), the hydrogen peroxide decomposes into water and oxygen gas. The platinum speeds up the reaction of the decomposition of H<sub>2</sub>O<sub>2</sub> into H<sub>2</sub>O and O<sub>2</sub> and acts as a catalyst in this reaction (you see, hydrogen peroxide gradually decomposes on its own over time). We would represent the equation below:</p> <center> <IMG src="../../media/balequa/formula2.gif" alt="Equation 2" width="174" height="16"> </center> <br> <a name="bal"></a> <p align="center"><img src="../../../../_themes/education/blrule.gif" width="600" height="10"></p> <center> <a href="#what">What are Chemical Equations</a> | <a href="#bal">Balancing Equations</a> | <a href="#rxn">Types of Reactions</a> | <a href="#top">Top of Page</a> </center> <p align="center"><img src="../../../../_themes/education/blrule.gif" width="600" height="10"></p> <center> <h2><font color="#0033CC">Balancing Equations</font></h2> </center> <br> <p>When the coefficients in a chemical equation are balanced, there are equal numbers of atoms of each element on both sides of the equation. We say that the chemical equation is balanced. You might ask, well, why does the chemical equation have to be balanced? Well, the answer to this stems from the atomic theory. In a chemical reaction, there is only a recombination of the atoms, no atoms are destroyed or created. Take our first equation:</p> <br> <center> 2Na + Cl<sub>2</sub> -> 2NaCl </center> <br> <p>In this reaction you have 2 atoms of sodium + 1 molecule of chlorine reacting to form 2 molecules of sodium chloride, which is salt.</p> <p>In our next example we have:</p> <br> <center> H<sub>3</sub>PO<sub>3</sub> -> H<sub>3</sub>PO<sub>4</sub> + PH<sub>3</sub> </center> <br> <p>Since the coefficients that give us the number of molecules have not yet been determined, this chemical equation is not balanced. To balance this equation, we select coefficients that will make the numbers of atoms of each element equal on both sides of the equations. It is best to write the coefficients so that they are the smallest whole numbers possible. To balance the previous equation we first want to look at the pieces which comprise the overall chemical equation. We find that oxygen occurs in only one of the products, so it would probably be the easiest to balance first. We get:</p> <br> <center> <b>4</b>H<sub>3</sub>PO<sub>3</sub> -> <b>3</b>H<sub>3</sub>PO<sub>4</sub> + PH<sub>3</sub> </center> <br> <p>Doing this also balanced the number of P and H atoms. So this means that in just one step we arrived at the balanced equation. You see, we now have 12 atoms of oxygen, 12 atoms of hydrogen, and 4 atoms of phosphorus on both sides of the equation. Before we balanced the equation, we had 3 atoms of oxygen, 3 atoms of hydrogen, and 1 atom of phosphorus on the reactants side, and 4 atoms of oxygen, 6 atoms of hydrogen, and 2 atom of phosphorus on the products side.</p> <p align="center"><img src="../../../../_themes/education/blrule.gif" width="600" height="10"></p> <center> <a href="#what">What are Chemical Equations</a> | <a href="#bal">Balancing Equations</a> | <a href="#rxn">Types of Reactions</a> | <a href="#top">Top of Page</a> </center> <p align="center"><img src="../../../../_themes/education/blrule.gif" width="600" height="10"></p> <a name="rxn"></a> <center> <h2><font color="#0033CC">Types of Reactions</font></h2> </center> <p>When we delve deeper into the study of chemistry, we find that there are several different types of reactions. There are several different ways to classify these reactions, mainly based on the patterns of similarity among them. There are 5 basic types of reactions we will be studying, and the way they are classified is based on how atoms or groups of atoms are rearranged during a particular reaction. These reactions are:</p> <center> </font><table border=0 cellspacing=4 > <tr> <td>1. Combination reactions</font></td> </tr> <tr> <td>2. Decomposition reactions</font></td> </tr> <tr> <td>3. Displacement reactions</font></td> </tr> <tr> <td>4. Metathesis reactions</font></td> </tr> <tr> <td>5. Combustion reactions</font></td> </tr> </table> </center> <br> <br> <br> <center>Combination Reactions</center> <p>A combination reaction is a reaction in which two substances combine to form a third substance. A simple example would be where two elements react to form a compound of the elements. A good example of this would be:</p> <br> <center> 2Na(s) + Cl<sub>2</sub>(g) -> 2NaCl(s) </center> <br> <p>Combination reactions can also have compounds as the reactants. An example of this would be where phosphorus trichloride reacts with chlorine to form phosphorus pentachloride:</p> <br> <center> PCl<sub>3</sub>(l) + Cl<sub>2</sub>(g) -> PCl<sub>5</sub>(s) </center> <p>Here is another combination reaction, the burning of copper and oxygen to produce copper(II) oxide:</p> <br> <center> 2Cu + O<sub>2</sub> -> 2 CuO </center> <br> <center>Decomposition Reactions</center> <p>A decomposition reaction is a reaction in which a single compound reacts to give two or more substances. In order to decompose a compound, it is often necessary to raise the temperature. An example of a decomposition reaction would be the decomposition of mercury (II) oxide into mercury and oxygen when the compound is heated.</p> <br> <center> <IMG src="../../media/balequa/merform.gif" alt="Mercury Decomposition" width="144" height="23"> </center> <br> <p>A compound can also decompose into a compound and an element, or two compounds.</p> <br> <center>Displacement Reactions</center> <p>Displacement reactions (sometimes referred to as single replacement reactions) are reactions in which an element reacts with a compound displacing an element from it. An example of this would be when a copper metal strip is dipped into a solution of silver nitrate. When this happens, crystals of silver metal are produced.</p> <center> Cu(s) + 2AgNO<sub>3</sub> (aq) -> 2Ag (s) + Cu(NO<sub>3</sub>)<sub>2</sub> (aq) </center> <p>In this reaction, copper replaces the silver in silver nitrate. In the process it produces copper(II) nitrate solution and silver metal.</p> <p>A fun fun fun single replacement reaction is one that we call "burning magnesium".</p> <br> <center> 2Mg + CO<sub>2</sub> -> 2MgO + C </center> <br> <center> <IMG src="../../media/balequa/maghigh.gif" alt="magnesium and dry ice" width="538" height="194" > </center> <p> <center>Metathesis Reactions</center> <p>A metathesis reaction is a reaction that appears to involve the exchange of parts of the reactants. Metathesis reactions are also referred to as double-replacement reactions. When the reactants in the reaction are ionic compounds in solution, cations and anions of the compounds are the parts exchanged. An example of a metathesis reaction would be the reaction of potassium iodide solution and lead (II) nitrate solution. The reactants are colorless liquids, yet one of the products of this reaction is lead (II) iodide, which forms a yellow precipitate. A precipitate is a solid compound formed during a reaction in solution.</p> <center> 2KI(aq) + Pb(NO<sub>3</sub>)<sub>2</sub>(aq) -> 2KNO<sub>3</sub>(aq) + PbI<sub>2</sub>(s) </center> <p>What happens in this metathesis reaction is that iodide ions in potassium iodide switch with the nitrate ions in lead (II) nitrate. What happens is that we get potassium nitrate (2KNO<sub>3</sub>) and lead (II) iodide (PbI<sub>2</sub>) as the products. <p>Here is another example of a double replacement reaction in which iron(III) chloride and sodium hydroxide are combined to produce a precipitate:</p> <br> <center> FeCl<sub>3</sub> + 3NaOH -> 3NaCl + Fe(OH)<sub>3</sub> </center> <br> <center>Combustion Reactions</center> <P>So far, all the reactions which we have studied have been classified by the type of atom rearrangement that happens in the reaction. Combustion reactions are different in that they are characterized by the fact that one of the reactants is always oxygen. A combustion reaction is a reaction of a substance with oxygen, usually with the rapid release of heat to produce a flame. Organic compounds burn in oxygen to produce carbon dioxide and water vapor. Here is the formula for the chemical reaction involving butane burning in air to produce carbon dioxide and water vapor.</p> <center> 2C<sub>4</sub>H<sub>10</sub>(g) + 13O<sub>2</sub>(g) -> 8CO<sub>2</sub>(g) + 10H<sub>2</sub>O(g) <p>Here is an example of a combustion reaction. It involves burning methane. This results in carbon dioxide and water being formed from the reaction:</p> <br> CH<sub>4</sub> + 2O<sub>2</sub> -> CO<sub>2</sub> + 2H<sub>2</sub>O <p align="center"><img src="../../../../_themes/education/blrule.gif" width="600" height="10"></p> <a href="#what">What are Chemical Equations</a> | <a href="#bal">Balancing Equations</a> | <a href="#rxn">Types of Reactions</a> | <a href="#top">Top of Page</a> | <a href="../../index.html">Home</a> | <a href="../search.htm">Search</a> | <a href="../../glossary.htm">Main Glossary</a> <p align="center"><img src="../../../../_themes/education/blrule.gif" width="600" height="10"></p> <layer src="http://www.spidersoft.com/ads/bwz468_60.htm" visibility=hidden id=a1 width=600 onload="moveToAbsolute(ad1.pageX,ad1.pageY); a1.clip.height=60;visibility='show';"></layer> </center> </frameset>