This equation is more complex than the previous examples and requires more steps. Example #3 (Complex) C 2H 5OH + O 2 = CO 2 + H 2O The equation is now balanced because there is an equal amount of substances on the left and the right hand side of the equation. To fix this unbalanced equation a 5 in front of the O 2 on the left hand side is added to make 10 O's on both sides resulting in P 4 + 5O 2 = 2P 2O 5 The left hand side has 2 O's and the right hand side has 10 O's. The left hand side has 4 P's and the right hand side has 4 P's. This equation is not balanced because there is an unequal amount of O's on both sides of the equation. This equation is a balanced equation because there is an equal number of atoms of each element on the left and right hand sides of the equation. The equation will now look like this: 4Na + O 2 = 2Na 2O To fix this 2 more Na's are added on the left side. Again, this is a problem, there must be an equal amount of each chemical on both sides. The right hand side has 4 Na's total and 2 O's. Currently the left hand side of the equation has 2 Na atoms and 2 O atoms. Notice that the 2 on the right hand side is "distributed" to both the Na 2 and the O.
Now the equation reads: 2Na + O 2 = 2Na 2O
To fix this a 2 is added in front of the Na 2O on the right hand side. On the left hand side there are 2 O atoms and the right hand side only has one. In the next step the oxygen atoms are balanced as well. In this there are 2 Na atoms on the left and 2 Na atoms on the right. This problem is solved by putting a 2 in front of the Na on the left hand side: 2Na + O 2 = Na 2O As it stands now, there is 1 Na on the left but 2 Na's on the right. In order for this equation to be balanced, there must be an equal amount of Na on the left hand side as on the right hand side. Hydrogen and oxygen are usually balanced last.
Generally, it is best to balance the most complicated molecule first.
BALANCED NET IONIC EQUATION CALCULATOR TRIAL
Simple chemical equations can be balanced by inspection, that is, by trial and error. Using Trial and Error/Inspection Example #1 (Simple) By changing the scalar number for each molecular formula, the equation may be balanced. In case of net ionic reactions, the same charge must be present on both sides of the unbalanced equation. Thus, each side of the equation must represent the same quantity of any particular element. This is the net ionic equation that characterizes a neutralization reaction that takes place between a strong acid and a strong base.In a chemical reaction, the quantity of each element does not change. the ions that are present on both sides of the equation. To get the net ionic equation, you must eliminate the spectator ions, i.e. Sodium bromide is soluble in water, which is why it exists as dissociated ions in aqueous solution. This means that the complete ionic equation looks like this Similarly, the fact that sodium hydroxide is a strong base means that you can write Now, because hydrobromic acid is a strong acid, it will ionize completely in aqueous solution, which means that you can write The balanced molecular equation looks like this In this case, the salt is sodium bromide, #"NaBr"#. When an acid and a base react, the neutralization reaction produces water and an aqueous salt. This should tell you that the net ionic equation will involve the hydrogen cations-or hydronium cations, #"H"_3"O"^(+)#-produced by the strong acid and hydroxide anions produced by the strong base. Hydrobromic acid, #"HBr"#, is a strong acid and sodium hydroxide, #"NaOH"#, is a strong base, so right from the start, you know that you're dealing with a neutralization reaction.
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