5 Steps for Balancing Chemical Equations

5 Steps for Balancing Chemical Equations Being able to balance chemical equations is a vital skill for chemistry. Heres a look at the steps involved in balancing equations, plus a worked example of how to balance an equation. Steps of Balancing a Chemical Equation Identify each element found in the equation. The number of atoms of each type of atom must be the same on each side of the equation once it has been balanced.What is the net charge on each side of the equation? The net charge must be the same on each side of the equation once it has been balanced.If possible, start with an element found in one compound on each side of the equation. Change the coefficients (the numbers in front of the compound or molecule) so that the number of atoms of the element is the same on each side of the equation. Remember, to balance an equation, you change the coefficients, not the subscripts in the formulas.Once you have balanced one element, do the same thing with another element. Proceed until all elements have been balanced. Its easiest to leave elements found in pure form for last.Check your work to make certain the charge on both sides of the equation is also balanced. Example of Balancing a Chemical Equation ? CH4 ? O2 → ? CO2 ? H2O Identify the elements in the equation: C, H, OIdentify the net charge: no net charge, which makes this one easy! H is found in CH4 and H2O, so its a good starting element.You have 4 H in CH4 yet only 2 H in H2O, so you need to double the coefficient of H2O to balance H.1 CH4 ? O2 → ? CO2 2 H2OLooking at carbon, you can see that CH4 and CO2 must have the same coefficient.1 CH4 ? O2 → 1 CO2 2 H2OFinally, determine the O coefficient. You can see you need to double the O2 coefficient in order to get 4 O seen on the product side of the reaction.1 CH4 2 O2 → 1 CO2 2 H2OCheck your work. Its standard to drop a coefficient of 1, so the final balanced equation would be written:CH4 2 O2 → CO2 2 H2O Take a quiz to see if you understand how to balance simple chemical equations. How to Balance a Chemical Equation for a Redox Reaction Once you understand how to balance an equation in terms of mass, youre ready to learn how to balance an equation for both mass and charge. Reduction/oxidation or redox reactions and acid-base reactions often involve charged species. Balancing for charge means you have the same net charge on both the reactant and product side of the equation. This isnt always zero! Heres an example of how to balance the reaction between potassium permanganate and iodide ion in aqueous sulfuric acid to form potassium iodide and manganese(II) sulfate. This is a typical acid reaction. First, write the unbalanced chemical equation:KMnO4  Ã‚  KI  Ã‚  H2SO4  Ã¢â€ â€™Ã‚  I2  Ã‚  MnSO4Write down the oxidation numbers for each type of atom on both sides of the equation:Left hand side: K 1; Mn 7; O -2; I 0; H 1; S 6Right hand side: I 0; Mn 2, S 6; O -2Find the atoms that experience a change in oxidation number:Mn: 7 → 2; I: 1 → 0Write a skeleton ionic equation that only covers the atoms that change oxidation number:MnO4- → Mn2I- → I2Balance all of the atoms besides the oxygen (O) and hydrogen (H) in the half-reactions:MnO4- → Mn22I- → I2Now add O and H2O as needed to balance oxygen:MnO4- → Mn2 4H2O2I- → I2Balance the hydrogen by adding H as needed:MnO4- 8H → Mn2 4H2O2I- → I2Now, balance charge by adding electrons as needed. In this example, the first half-reaction has a charge of 7 on the left and 2 on the right. Add 5 electrons to the left to balance the charge. The second half-re action has 2- on the left and 0 on the right. Add 2 electrons to the right.MnO4- 8H 5e- → Mn2 4H2O2I- → I2 2e- Multiply the two half-reactions by the number that yields the lowest common number of electrons in each half-reaction. For this example, the lowest multiple of 2 and 5 is 10, so multiply the first equation by 2 and the second equation by 5:2 x [MnO4- 8H 5e- → Mn2 4H2O]5 x [2I- → I2 2e-]Add together the two half-reactions and cancel out species that appear on each side of the equation:2MnO4- 10I- 16H → 2Mn2 5I2 8H2O Now, its a good idea to check your work by making sure the atoms and charge are balanced: Left hand side:  2 Mn; 8 O; 10 I; 16 HRight hand side:  2 Mn; 10 I; 16 H; 8 O Left hand side:  Ã¢Ë†â€™2  Ã¢â‚¬â€œÃ‚  10  16  Ã‚  4Right hand side:  4