Chemical Equation – Some Basic Concept
In this topic we will discuss Chemical Equation – Some Basic Concept along with probable question asked in the examination which helps to get a clear concept about this topic.
|1.What is a chemical equation?|
|2.Example of Chemical equation|
|3.What are unbalanced equations?|
|4.Steps to balancing a chemical equation|
1.What is a chemical equation
A chemical equation is a process of representing a chemical reaction with symbols and formulas.
2.Example of Chemical equation
Let us take an example of a chemical reaction –
HCL + NaOH ————> NaCl +H2O
We write the reactant on the left side by putting a plus (+) sign between them.
We write the products on the right side by putting a plus (+) sign between them.
A chemical equation is a short-hand method of representing a chemical reaction.
A chemical equation is called balanced when it has an equal number of an atom on both side i.e.
Number of atom in reactant = Number of atom in product.
What are Unbalanced Equation ?
A chemical equation is called unbalanced if it has unequal atom for the element in reactant and product side.
Let us take an example of unbalanced equation.
Al + O2 —-> Al2O3
Here Number of O and Al atom in Reactant side and Number of O atom in product side is not equal. Hence it is called an unbalanced equation.
So we need to balance this chemical equation. Below we are discussing the method to balance a chemical equation
4.Steps To Balancing a Chemical Equation
To balance a chemical equation we follow 5 steps.
- Keeping the reactant left-hand side & products on the right-hand side we write down the chemical equation as a word equation.
- Next, we write all the formulas and symbols of the product and reactant in a word equation.
- We balance the equation by multiplying the symbols and formula by the smallest numbers
- Next, we put physical state, heat change, reaction condition under the reactant and product to make the equation more informative.
- To do this we write physical state with symbols such as For liquid (l), solid(s), Gas(s), Enthalpy Change (ΔH), etc.