What is Stoichiometry and How to Explain it With Examples?

Stoichiometry is a process of balancing the coefficient of the chemical equation. It’s a simple technique of balancing the proportional qualities of the chemical and their number of moles. It is a technique implemented according to the law of conservation of mass. Get details about What is Stoichiometry and How to Explain it With Examples?.

“Stoichiometric studies are the special beach of chemistry to balance the reactants and the products of the chemical reaction. To find and determine the proportional quantities of the reactant and the products in a chemical reaction”.

If you are not able to maintain the proportional ratio of the reactants then it can be difficult to produce the required quality of the products. Use the stoichiometry calculator to produce fixed-quality products. When you are maintaining the precise quantity of the chemical, then it is essential to mix the reactants in a predefined ratio.

In this article, we are elaborating the Stoichiometric by presenting a practical example of the concepts:

What is Stoichiometry?

“It is a special branch and field of chemistry to identify the desired quantitative product, you need to mix the specific proportional quantities of reactant.”

In the Greek language, You can find “Stoikhein” means the elements, and the “Metron” is Number The of elements in a chemical reaction.When using the stoichiometry calculator, then you are easily able to determine what is the molar concentration of the reactant required. The above reaction needs to follow the stoichiometry ratios.

Examples of the Stoichiometry:

Practical Example 1:

For example, if you want to produce 1 mole of water, then it is essential to mix the 2 moles of hydrogen and 1 mole of water. When you are producing the 2 moles of water, you are producing 36 grams of water.

2H2+O2→2H2O
Use the stoichiometry calculator for determining what is the proportional ratio of the reactant and the products in a chemical reaction.

the molar concentration of water = 2H2O
Atomic weight of water = 2(1)+(16)= 18 grams
2 moles of water are = 2(18) = 36 grams.
Have noticed the molar concentration of the reactants and products is equal on both sides of the chemical equation.
The molar concentration can be determined by the stoichiometry calculator

Practical Example 2:

Now rusting of the iron metal is the iron oxide Fe2O3, when you are going to produce the iron oxide in the laboratory, need to mix the 4 moles of the iron with 3 moles of the oxygen

Fe+O2→Fe2O3

Just use the ratios to balance the chemical equation. When using the Balance the molar ratios of the reactant and the products are. It is easy to produce a specific quantity of products.

4Fe+3O2→2Fe2O3

Need to understand that the whole chemical reaction is going to work according to the law of mass of action, and it is essential to use the predetermined ratios of the chemical. The reactant and the product of the chemical reaction are going to produce in the predefined molar concentration.

• 4 moles of the iron are4(26) =104 grams.
• 3 moles of the Oxygen are 3(16*2) =96 grams
• 2 moles of the Iron Oxide are Fe2O3 = 2[2(26)+3(16)]
• 2 moles of the Iron Oxide are 204 grams of Fe2O3

Notice here the 104 grams of iron is going to react with the 96 grams of the 204 grams of Iron oxide. It’s a simple technique of balancing the proportional qualities of the chemical and their number of moles. The Stoichiometric technique is implemented according to the law of conservation of mass.

“Stoichiometric studies are the special beach of chemistry to balance the reactants and the products of the chemical reaction. To find and determine the proportional quantities of the reactant and the products in a chemical reaction”

Conclusion:

The online stoichiometry calculator makes it possible to find the molar concentration of the reactant and the product. The stoichiometric ratio is specific for a chemical reaction, by changing the molar concentration of the reactant, it may be possible we are not able to produce a specific product in the lab. For example, H2O2 is not water but Hydrogen peroxide and it is a pungent chemical but have the same reactant