Balancing Chemical Equations

Balancing Chemical Equations Objectives: I will be able to: describe the steps for writing a balanced chemical equation. balance chemical equations with adherence to law of conservation of matter.

If a chemical equation does not obey the law of conservation of mass the equation is said to be what? NOT BALANCED So Let’s look at the steps we need to take to BALANCE chemical equations Let’s work with the following equation: Fe + O2  Fe2O3

Step 1. Create a RAP table (what’s a RAP table ??) A table that shows us what atoms are present in this reaction, how many there are and are they reactants or products? For example: Fe + O2  Fe2O3 #R atom #P Fe 2 O 3

Step 2. Go to the first atom that’s not balanced and balance it! Since Fe atoms are not balanced what do we need to do to balance it? Right! Multiply it by 2 (Only multiply) #R atom #P 1 Fe 2 2 O 3 2x

In step 2 we balanced the number of Fe atoms by multiplying the reactant side by 2. This now becomes the new coefficient in the chemical equation. Modify the equation to reflect the change #R atom #P 1 Fe 2 2 O 3 2Fe + O2  Fe2O3 2x Are all atoms balanced?

Step 3. Move to the next unbalanced atom. What is it? #R atom #P 2 Fe 2 2 O 3 How can we balance the Oxygen? Multiply Reactants by 3 and Products by 2 Adjust the equation to reflect your changes #R atom #P 2 Fe 2 3x2 O 3x2 2Fe + 3O2  2Fe2O3 But notice that by changing Oxygen we also Changed Iron. We need to go back and fix this.

Step 4. Write out the updated RAP table. How can we balance the Iron? #R atom #P 2 Fe 4 6 O 6 Sure! Multiply the # of Reactant Fe atoms by 2 ! 2x Re-write the equation reflecting The new changes you’ve made. 4Fe + 3O2  2Fe2O3 Do we have a balanced Chemical Equation now? Yes we do!

2AgNO3 + MgCl2  2AgCl + Mg(NO3)2 Polyatomic Molecules polyatomic molecule: a molecule that consists of more than two atoms 1. When an equation has Polyatomics in it, such as in this balanced chemical equation 2AgNO3 + MgCl2  2AgCl + Mg(NO3)2 2. And the polyatomic appears on BOTH the reactant and product side of the equation Count the polyatomic as an “ATOM” So the above reactant atoms would be: #R atom #P 2 Ag 2 2 NO3 2 Mg 1 2 Cl 2 If the same polyatomic does not appear on both sides break the Polyatomic down into single atoms!

Let's try solving some Problems

Is this equation balanced? NaOH + CaBr2  Ca(OH)2 + NaBr What atoms do we have in this equation? Count atoms & Start the RAP table #R atom #P NA 1 1 OH 2 Ca 1 2 Br 1 2) Do the #Reactant atoms = the # of Product atoms? 3) So pick the 1st unbalanced atom & begin balancing

We’ll start with balancing Hydroxide (OH) NaOH + CaBr2  Ca(OH)2 +NaBr How can we make both Hydroxides equal? #R atom #P 1 Na 1 1 OH 2 1 Ca 1 2 Br 1 Sure we’ll multiply #R OH by 2 Next step> rewrite the modified eqn. 2x 2NaOH + CaBr2  Ca(OH)2 + NaBr Hydroxide is now balanced so let’s move to the next Unbalanced atom, which is? …

What can we do to balance the Bromine? Sure! Multiply the #P Bromine by 2 Now adjust the table to reflect The changes and then rewrite the Eqn. #R atom #P 2 Na 1 2 OH 2 1 Ca 1 2 Br 1 x2 2NaOH + CaBr2  Ca(OH)2 + 2NaBr

Let’s update the RAP table with the new #’s Based on our updated equation. 2NaOH + CaBr2  Ca(OH)2 + 2NaBr #R atom #P 2 Na 2 2 OH 2 1 Ca 1 2 Br 2 Are we now balanced? Sure!

Ok Try Balancing this equation: C2H6 + O2  CO2 + H2O #R atom #P 2 C 1 6 H 2 2 O 3 Step 1. Total up the atoms Step 2. Balance the #P Carbon #R atom #P 2 C 2 6 H 2 2 O 5 & Re-write the equation C2H6 + O2  2CO2 + H2O Are we done?

Step 3. Carbons are balanced now but Hydrogen isn’t. So, balance Hydrogen atoms next #R atom #P 2 C 2 6 H 2 2 O 5 Multiply #P Hydrogen by 3 x3 Step 4. Re-write the eqn. & Retotal the number of atoms #R atom #P 2 C 2 6 H 6 2 O 7 C2H6 + O2  2CO2 + 3H2O Carbon and Hydrogen are now balanced but oxygen isn’t.

Step 5. To balance Oxygen multiply O by 3½ #R atom #P 2 C 2 6 H 6 2 O 7 Step 6. Re-write the eqn. & Retotal the number of atoms 3 ½ x C2H6 + 3½ O2  2CO2 + 3H2O It looks like we’re balanced. But, are we? No! We can’t have 3 ½ Oxygen molecules! Only whole Numbers are allowed. So what do we need to do to fix this?

Step 7. Let’s clean this up by Multiply everything by 2 C2H6 + 3½ O2  2CO2 + 3H2O x 2 2C2H6 + 7 O2  4CO2 + 6H2O Step 8. Retotal #R and the #P atoms #R atom #P 4 C 4 12 H 12 14 O 14 YES! Are we balanced?

Try this problem NH4OH + FeCl3  Fe(OH)3 + NH4Cl Start here. Recognize we have polyatomics, but they appear on both sides of the equation. #R atom #P 1 NH4 1 1 OH 3 1 Fe 1 3 Cl 1 OK … Now finish it up

Answer to previous problem 3NH4OH + FeCl3  Fe(OH)3 + 3NH4Cl

Balancing Equations Summary Step 1. Create a RAP table Step 2. Total up the atoms Step 3. Determine the first unbalanced atom Step 4. Multiply the side (#R or #P) with fewer atoms to balance that atom and add your multiplier as a coefficient to the equation Step 5. Re-write the eqn. & retotal the number of atoms Step 6. Repeat steps 4 & 5 for the next unbalanced atom, continue until equation is balanced