Stoichiometry and Stoichiometric Calculations Based on Chemical Formulas
You may wonder why is it necessary to quantify elements involved in chemical reactions. If by chance your cook puts extra salt in your favourite food, will you prefer eating it? Possibly not. Likewise, without a correct examination of stoichiometry, it is not possible to rule out what amount of elements is appropriate for any specific reaction. So, what is stoichiometry?
Here, in this content, you will get to know what does stoichiometry mean and what are stoichiometric calculations.
Let us start.
What is Stoichiometry?
Stoichiometry refers to the evaluation of products and reactants taking part in any chemical reaction. The term “stoichiometry” is obtained from two Greek words, namely “stoichion” which determines element and “metry” which means measuring.
Moreover, stoichiometry is established on the law of conservation of mass where entire mass of reactants is equivalent to the whole mass of products, which illustrates that relations among products and reactants’ quantities usually make a ratio of +ve integers. This shows that if you know the number of individual products, you can easily calculate the product amount.
Again, if the quantity of one reactant is known, and product quantity can be determined using an experiment, then calculation of other reactants is also possible. This is represented in the following example of a balanced chemical reaction.
CH4 + 2O2 -> CO2 + 2H2O
In this reaction, one mole of methane undergoes a reaction with two oxygen gas molecules to produce one carbon dioxide molecule and two water molecules. This chemical reaction is a perfect example of full combustion (burning).
Now that you have understood what is stoichiometry, you must also know about reaction, composition and gas stoichiometry.
The description of quantitative relationships among the elements while they participate in reactions is called reaction stoichiometry. For the above reaction example, reaction stoichiometry evaluates the relationship of amounts of methane and oxygen that reacts to give out water and carbon dioxide.
As atomic weight and moles have a relation between them, the ratios which are calculated by stoichiometry are used to measure quantities in terms of weight in a balanced equation. This process is known as composition stoichiometry.
Next, gas stoichiometry is concerned with the reactions that involve gases. In these reactions, gases have a known volume, pressure and temperature and hence assumed as ideal gases. The volume ratio of gases is the same according to Ideal Gas Law, but ratio of mass of one reaction has to be determined from reactants and products’ molecular masses. In real life, since isotopes exist, calculations of mass ratio are done using molar masses.
Now, as the discussion of what is meant by stoichiometry is completed, let us move further with stoichiometric calculations based on chemical formulas.
The conversion factors in chemistry can be used to solve stoichiometric problems. Generally, solution of all stoichiometry issues can be found in just a few steps:
Balancing the equation
Converting substance units to moles
Using mole ratio to calculate moles of yielded substances in the reaction
Converting moles of needed elements to the required units.
Take a look at the following example of how rusting of iron takes place.
Fe + O2 -> Fe2O3
A chemical equation’s elemental parts never get lost or destroyed. The product of a reaction must correspond to the actual reagents. This fact is true not only for element types in the production but for the numbers as well. The unbalanced equation is:
Fe + O2 -> Fe2O3
This chemical equation shows that two atoms of oxygen react with one atom of iron to form 2 atoms of iron and three atoms of oxygen. (The subscript value like 2 in O2 shows how many oxygen atoms are there in a molecule.) However, since the equation is unbalanced, the reaction is not real, because it demonstrates a reaction where one iron atom yields two atoms of iron.
Hence, balancing the equation is a must by putting coefficients before the substances to make sure that total number of atoms on the reactants’ side is similar to total number of substances on the product side. The balanced equation is:
4Fe + 3O2 -> 2Fe2O3
On counting the atoms in this new balanced equation, you will see that on the arrow’s left side, there are four iron atoms and six oxygen atoms (3 x 2 = 6). On arrow’s right side, there are 4 iron atoms (2 x 2 = 4) and 6 oxygen atoms (2 x 3 = 6). Therefore, atoms on both left and right side match.
The procedure of transforming units to moles demands for conversion factors. Below you will be able to see the most used and essential conversion factors that are used between moles and volumes of gases, moles and grams, moles and molecules and moles and solutions. You must remember that although these factors mainly convert other units to moles, they also can convert from moles to other units.
Conversion of Grams to Moles
Gram formula mass of an element refers to one mole of an element’s mass. According to the definition, it is estimated in grams/mole and is evaluated by adding all the atomic weights of atoms of a compound. In the periodic table, atomic weights are provided in atomic mass units, but they depict gram formula mass. For example, one mole of carbon of 12 a.m.u has a weight of 12 grams.
As a conversion factor, GFM (gram formula mass) is used in stoichiometric evaluations by the following expression:
Moles = grams / gram formula mass
Conversion of Volumes of Gas to Moles
With regards to the Ideal Gas Law PV = nRT, where n is number of moles, the equation can be rearranged to find a solution for n. So the equation can be written as:
n = PV / RT, where P = pressure in atm
V = volume in litres
T = temperature in Kelvin
R = gas constant which is equivalent to 0.0821 L - atm / mol – K
Hence, if P, T and V are given, moles of a compound in a gas can be found out. Furthermore, if a problem mentions that calculations should be done using Standard Temperature and Pressure (STP) where P = 1 atm and T = 273 K, the problems become easier. So, one mole of gas will occupy a volume of 22.4 litres at STP.
Conversion of Individual Particle to Moles
The Avogadro number gives the conversion factor for converting particle number to moles. In general 6.02 x 1023 particle formula units are there in one mole of a substance, where the formula unit determines whether that substance is a molecule, compound, atom or ion. Take a look at some formula unit examples below:
Compounds = Cu2S, NaCl
Molecules = N2, H2
Atoms = Fe, Na
Ions = Na+ (aq) Cl- (aq)
As 1 mole is equal to 6.02 x 1023 formula units, the conversion can be done using the following equation:
Moles = formula units / 6.02 x 1023
Conversion of Solutions to Moles
It is comparatively simple to convert solution measures (molality and molarity) to moles.
The division of mole number of solute by litres of solvent is known as molarity. So after rearranging the equation, the following is obtained:
Moles = molarity x litres of solution
The division of mole number of solute by the number of solvent in kilograms is known as molality. Here also, after rearranging the equation, it is found:
Moles = Molality x kilograms of solution
Considering the example of rusting of iron 4Fe + 3O2 -> 2Fe2 O3, the frontal coefficients of oxygen, iron and iron(III) oxide ratios govern the reaction. However, these numbers do not say that this reaction can only happen provided that there are exactly 3 oxygen moles and 4 iron moles that will yield 2 iron (III) oxide moles. Rather, it suggests that the reaction of oxygen and iron will stick to a ratio of 4 : 3. For instance, 2 iron moles undergo reaction with 1.5 oxygen moles to form 1 iron (III) oxide mole.
Now, with the help of a balanced equation, units converted to moles and understanding mole ratio, calculation of the yields in a reaction in moles is possible.
The last step calls for the conversion of moles to original units asked in a particular problem. So, it involves turning back of the required conversion factors said above.
Problem: The equation N2 (g) + H2 (g) -> NH3 (g) is at STP. Calculate the volume of H2 (g) required to produce 22 litres of NH3 (g).
Answer: After balancing the equation: N2 (g) + 3H2 (g) -> 2NH3 (g)
Conversion to moles: (224 L of NH3 (g) x 1 mole) / 22.4 L = 10 moles of NH3 (g)
Mole ratio: (10 NH3 moles (g) x 3H2 moles (g)) / 2NH3 moles (g) = 15 moles of H2 (g)
Conversion to required unit: 15H2 moles (g) x 22.4 L / 1 mole = 336 L of H2 (g)
We hope that the above discussion on what is stoichiometry and its calculations will clear your concept of the same. For more stoichiometric calculations based on chemical formulas download Vedantu app today.
1. What is the Definition of Stoichiometry?
Ans. In simple words, stoichiometry is the evaluation of reactants and products in all chemical reactions.
2. What is Mole Ratio?
Ans. Mole ratio refers to the ratio of mole amounts of any two substances taking part in a chemical reaction.
3. How is Stoichiometry Used in Real Life?
Ans. In real life, stoichiometry has vast applications in the production of soaps, gasoline, tyres, deodorants, fertilisers, etc.
4. What are Stoichiometric Calculations?
Ans. Stoichiometric calculations involve various processes that include balancing equation, evaluation of moles of substances produced in a reaction, conversion of units to moles and vice versa with the help of various conversion factors.