Fundamentals of Balancing Chemical Equations |
Posted: April 15, 2019 |
What is a chemical equation?A method of writing a chemical reaction using chemical symbols where by convention, the reactants are represented on the left-hand side and the products on the right-hand side are called chemical reactions. An arrow between them signifies the type of reaction. A single arrow denotes an irreversible reaction whereas a double arrow denotes a reversible reaction. As per the law of conservation of matter, every atom on the left-hand side appears on the right-hand side but their combinations and arrangements change. Example, the formation of two water molecules from one oxygen molecule and two hydrogen molecule is written as follows: 2H2 + O2 → 2H2O How to Balance Chemical Equation?Below we have discussed the steps to balance any chemical reaction. Step 1: It is important to identify each element in the equation as the number of atoms must be the same on both the sides of the equation once it is balanced. Step 2: The net charge on both the sides of the equation must be the same once it is balanced. Step 3: It is always a good idea, to begin with, an element found in the compound on both the sides of the equation. Adjust the numbers written in front of the compound to balance the number of atoms on both the sides of the equation. Remember not to change the subscripts while balancing the equation. Step 4: Balance all the elements similarly. Leave the elements in pure form to balance at the last. Step 5: Make sure the charge on both sides of the equation is also balanced equally. Types of Chemical Reactions and EquationsThe four major types of reactions are discussed below along with the examples for each. Type 1: Synthesis or combustion In this type of reaction, two or more reactants combine to form one product. The reaction is as follows: A + B ----------> AB For example, the formation of sulfur dioxide S + O2 ----------> SO2 (Sulfur) (Oxygen) (Sulfur dioxide) Type 2: Decomposition These reactions are the opposite of combination or synthesis reactions. In this type of reaction, one compound breaks down into two or more products (simpler substances) The reaction is as follows: AB ----------> A + B For example, the decomposition of calcium carbonate into calcium oxide and carbon dioxide CaCO3 ----------> CaO + CO2 (calcium carbonate) (Calcium oxide) (Carbon dioxide) Type 3: Single Replacement or Substitution In this type of reaction, a less active element is displaced by a more active element of a compound. The reaction is as follows: A + BC ----------> B + AC For example, Zinc reacts with hydrochloric acid to give hydrogen and zinc chloride as products. Zn + 2 HCl ----------> H2 + ZnCl2 (Zinc) (Hydrochloric acid) (Hydrogen) (Zinc chloride) Type 4: Double Displacement or Metathesis In this type of reaction, two species are displaced. These reactions usually occur in solution, either as a precipitation reaction or neutralization reaction. The reaction is as follows: AB + CD ----------> AD + CB For example, Hydrochloric acid reacts with sodium hydroxide to give sodium chloride and water as products. HCl + NaOH ----------> NaCl + HOH (Hydrochloric acid) (sodium hydroxide) (sodium chloride ) (water) To learn various other chemistry concepts such as Inductive effect, Atomic Structure, Transition Elements and more, in an interesting and engaging way subscribe to BYJU’S YouTube channel
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