Types of Stoichiometric Problems

Numerous valuable things can be discovered through the application of stoichiometry, including the presence of a limiting reagent in a reaction, the amount of a product that will be created when a specific reaction occurs, and many other things.

According to the law of conservation of mass, the increased mass must have arisen from the presence of the oxygen. 

To get the mass of oxygen, we may easily remove the initial mass of iron from the end mass of rust, as shown in the figure below. 

This tells us how much oxygen is coupled with iron during the course of the process. Nevertheless, how could we forecast the quantity of rust produced by the reaction of grams10.00 grammes of iron with enough oxygen without first doing a laboratory experiment? We do it in accordance with stoichiometry.

The Fundamentals of Stoichiometry

The first thing we always do is convert the mass of the chemical we have to the molar amount of it by using the molecular weight of the element in question.

In mathematics, a mole is a specified number of something – 6.0221023 of something, to be precise.

Balancing Chemical Reactions 

Despite the fact that the reaction described above appropriately produces the reactants and products, it remains imbalanced.

This is due to the fact that, if we look closely, the total mass of all atoms on the right does not equal the total mass of all atoms on the left.

As a result, this reaction is in violation of the Law of Conservation of Mass and, as a result, is incorrect. 

What we need to do to correct the situation is to ensure that the number of identical atoms on both sides of the equation is the same.

The Fe(s)+O2(g)—>FeO(s) 

Gas Law

Gas law is defined as the collection of empirical gas evidence was compiled in one equation after many experiments and scientific observations were made over the course of the next hundred years. 

This equation related all the different characteristics of gas to one another under ideal conditions. 

The Ideal Gas Law is the name given to this equation.

PV=nRT,

Where, R=0.08206 and T is temperature. 

Gas Pressure

Gas Pressure is a term used to describe the force exerted by gas in a closed system.

The ideal gas law states that the pressure of a gas is proportional to the number of molecules in the gas. 

A common interpretation of this is that the overall pressure of a gas is made of the partial pressures of the various molecules that make up the gas, as follows:

 Ptotal =PA+PB+PC

Oxidation States are defined as follows: 

When it comes to electronegativity, oxidation state is related to electron configuration as well as electron configuration. 

As a result, when we go over these laws, we should have the periodic table in mind, and we should memorise them in terms of the table.

Balancing Redox Reactions

Because we now know the oxidation states of the products and reactants, we can divide the balanced process into its constituent oxidation and reduction reactions, as shown in the diagram.

In order to designate the oxidation state, you must write it on the element as if it were an electric charge on it.

Examples of several types of stoichiometry 

Stoichiometry difficulties are typically categorised based on the measurements that were utilised for the reactants involved — moles, mass, and volume — in order to simplify the problem.

Here are a few instances of the types of issues you will come across on your journey. Mole-mole conversions are at the heart of every stoichiometry calculation, yet they are also the most difficult.

CALCULATIONS BETWEEN MOLE-MOLE

Sulphur combines with oxygen to generate sulphur trioxide, which is represented by the equation

2S + 3O2= 2SO3 is a chemical equation.

CALCULATION OF THE MASS-MOLECULE

The breakdown of potassium chlorate results in the production of oxygen, as shown in the equation.

O2 + 2KClO3= 2KCl + 3O2

CONVERSIONS BETWEEN VOLUME AND MOLE

According to the equation, the reaction between hydrogen and nitrogen produces ammonia.

2NH3 is formed via the reaction of N2 with 3H2.

There are several different kinds of stoichiometric difficulties.

Stoichiometric difficulties can be classified into four categories:

• Mass to mass  conversion

• Mass to moles conversion

• Mole to mass steps conversion

• Mole to mole steps conversion

Using stoichiometry to solve problems

When addressing a stoichiometry problem, there are four steps to follow:

Fill in the blanks with the balanced chemical equation.

Convert the units of the given material (A) into moles of the same substance. 

Calculate the number of moles of the desired substance by dividing it by the mole ratio (B).

The requested substance’s moles must be converted to the relevant units of measurement.

Conclusion

A stoichiometric chemical reaction is one in which the quantities of the reactants and products are such that all of the reactants are consumed and none are left after the chemical reaction has been completed. 

Stoichiometry is important for measuring chemical reactions, such as those that occur in corrosion processes, because it allows for the simultaneous measurement of two variables.

Stoichiometry is a technique for calculating the needed quantities of chemical reactants and products from a balanced chemical equation, and it is employed in chemical engineering.  

In order for the chemical equation to stay balanced, the proportions of the reactants and products must remain constant when the quantities of the reactants and products are increased or decreased, respectively.

When it comes to chemical reactions, stoichiometry is founded on the law of conservation, which stipulates that for a chemical reaction equation to be balanced, the total mass of all of the reactants must be equal to the total mass of all of the products.