Using english to calculate stoichiometry

 

Understanding Stoicymetry

        Stoichiometric Definition and Stoichiometric Type - Stoichiometry is a chemical branch associated with a quantitative relationship that exists between reactants and products in chemical reactions. The reactant is a substance that participates in a chemical reaction, and also the product is a substance obtained as a result of a chemical reaction.

Stoichiometry

     The stoichiometry depends on the fact that the elements behave in a predictable or predictable way, as well as material that can neither be created nor destroyed.
Therefore, when the elements are combined then produce a chemical reaction, something known and also specific that will occur and the reaction can be predicted by elements and also the number involved. Stoichiometry is the mathematics behind chemistry.
The stoichiometric calculations can find out how the elements and also the components diluted in a solution whose concentration is known react in the experimental conditions. The word "Stoichiometry" comes from the Greek word "stoicheion", meaning "element" and also "metron" means "size".

The laws governing Stoichiometry

The stoichiometry relies on law is like fixed comparative law, double comparative law and also the law of conservation of the masses.
• The law of mass conservation
Using the laws of physics is like the law of conservation of mass, which holds that the mass of the reactants is equal to the mass of the product, Stoichiometry is used to gather information about the amount of various elements used in a chemical reaction,
• Comparative law remains
This law states that the chemical compound (substance consisting of 2 (two) or more ages) which always contains the same proportion of an element (compound with one atom type) with mass.
• Law of multiple comparison
This law is one of the basic laws of stoichiometry, aside from the law of fixed comparison. Sometimes it is also called Dalton's law. It is said that, if 2 (two) elements form more than one compound between them, then the mass ratio of a second element which joins the fixed mass over the first element of both will have a ratio of a small sum of the whole.

Stoichiometric explanation

      Subject to the above laws, such chemical reactions may combine in a defined chemical ratio. The sum of each element must be the same throughout the reaction. In a balanced chemical reaction, the relationship between the amount of reactants and the product will usually form the ratio of integers. For example, in a reaction that forms ammonia (NH3), exactly 1 (one) nitrogen molecule (N2) reacts with 3 (three) hydrogen molecules (H2) to produce 2 molecules of NH3. It can be described as follows
N2 + 3H2 ---> 2NH3
Thus, the stoichiometry can be used to calculate the quantity as the amount of product that can be produced when the reactants are given and also the percentage of reactants made into a known product.

Stoichiometric Type
• Reaction stoichiometry
The stoichiometry is often used to balance the chemical equations found in reaction stoichiometry. It depicts that the quantitative relationship between substances is caused because they participate in chemical reactions.
• Composition Stoichiometry
The stoichiometry of this composition explains the quantitative (mass) relationship between an element in a compound. For example, the stoichiometry of the composition represents the (mass) nitrogen with the joined hydrogen and becomes a complex ammonia. Ie 1 mole of nitrogen and also 3 moles of hydrogen in each of 2 moles of ammonia. Mole is the unit used in chemistry for the amount of substance.
• Gas Stoichiometry
The type of stoichiometry is related to a reaction involving a gas, in which the gas is at a known temperature, pressure and volume and can also be considered an ideal gas. For gas, the ideal volume ratio is equal to the ideal gas law, but the ratio of the single reaction mass must be calculated from the molecular mass of the reactant as well as the product, in which the molecular mass is the mass of one (1) molecule of the substance.
The ideal gas is a theoretical gas consisting of 1 (one) set of randomly moving, non-interacting particles that adhere to an ideal gas law. The ideal gas law is an ideal gas state equation. The ideal gas law equation is as follows:
"PV = nRT, where P is pressure, V is volume and also T is absolute temperature, n is gas mol and also R is universal gas constant".

Understanding stoichiometric ratio

     A number of stoichiometry or also the ratio of reagents (substances added to a system in    order to create a chemical reaction) is either the amount or the ratio of which, assuming that the result of a reaction is completed on a basis,  Among others are as follows:
1. All reagents are consumed
2. There is no deficit reagent
3. There is no residual residue
4. Reactions will only occur or are created on stoichiometric ratios

Stoichiometry Formulas

The quantitative study of the relative amounts of reactants and products in chemical reactions is referred to as stoichiometry. Stoichiometric problems are solved in just four simple steps which are as following:

• First step is the balance the equation
• Convert units of a given reactants and products into moles.
• This is followed by calculating the moles of substance yielded by the reaction using the mole ratio,
• The final step is to convert moles of desired substance to desired units.

Let's suppose the following reaction of iron and oxygen that result in rust formation for stoichiometry calculation:

Fe+O2→Fe2O3

As mentioned, the first step in stoichiometric calculation is the balancing the equation. As we know that reactants of a chemical equation are never destroyed or lost and therefore, the products of a reaction exactly correspond to the original reactants. Now, let’s balance the given equation:

Fe+O2→Fe2O3

According to the equation, 1 iron (Fe) atom react with two oxygen (O) atoms to obtain 2 iron atoms and 3 oxygen atoms; the reaction is not balanced. 

4Fe+3O2→2Fe2O3

According to the above mentioned balanced equation, 4 atoms of iron and 6 atoms of oxygen (since 3 ×2 = 6 ) react to form 4 iron (since 2 × 2 = 4 ) and 6 oxygen (2 ×3 = 6). The atoms on both sides of the equation match. Now, convert the given units to moles using conversion factors and then calculate the moles of substance.

Stoichiometry Formulas List

Stoichiometry formulas used for stoichiometry calculations are as follows:

• One mole (1 mol) of an element = 6.022  × 1023

• entities (the Avogadro Number). 

Therefore, 1 mol of carbon-12 means there are 6.022 × 1023 carbon-12 atoms; 1 mol of H2O contains 6.022  × 1023 H2

O molecules. 

• Molar mass of an element = mass(g)/mole.

• Molar mass of an compound = Sum total of molar masses of atoms of elements in the formula

• Mole to mass stoichiometry formula:  Mass (g) = no. of moles×no. of grams1 mol

• Mass to mole stoichiometry formula: No. of moles = Mass(g)× 1 molno of grams

• Moles to substance entity (atoms, molecules etc) formula: No. of entities = no. of moles× 6.022×1023 entities1 mol

• Substance entity to mole stoichiometry formula: No. of moles = no. of entities×1 mol6.022×1023 entities

• Mass percent of an element in a compound is calculated using molecular mass and chemical formula. 

The formula is as follows:

Mass % of element X = atoms of X in formula×atomic mass of X (amu)molecular(orformula) mass of compound (amu) ×100

Since the chemical formula provides information about moles of each element in a compound, the mass percent of element X can be determined using the molar mass. The stoichiometry formula is as follows

Mass % of element X = moles of X in formula×molar mass of X (amu)mass of one mole of compound(amu)

×100.

Stoichiometry Formulas Mole to Mole

The mole to mole stoichiometry formulas determine the molar relationships of reactants and products in a chemical reaction using the balanced chemical equation which in turn is used to calculate the moles of a product produced from the given quantities of the reactants. It follows the law of conservation of mass which states that reactants of a chemical equation are never destroyed or lost and therefore, the products of a reaction exactly correspond to the original reactants. Using the law, the given equation is balanced and the stoichiometric ratios of the reactants and products; these ratios can be used as conversion factors for mole-to-mole conversions.

Now, let’s suppose, we want to calculate the number of mole produced by 2 moles of oxygen. For the purpose, the following equation will be used

H2+O2→H2O

.

Now, let’s first balance the equation. By balancing the equation, we get following one.

2H2+O2→H2O

.

Here, we can see one mole of oxygen produces two moles of water. The stoichiometric ratio is 1 mole of oxygen: 2 mole of water. Let’s assume that there is abundant hydrogen gas available for reaction. Under this condition,

2 mole of oxygen×2 mole of water1 mole of oxygen

= 4 moles of water

Mass to Mole Stoichiometry Formula

It uses molar mass as a conversion ration. Molar mass refers to the mass of a given substance divided by its amount (mol). As we know that mass of a substance is calculated by measuring the amount of the substance and then converting it into the moles. This is followed by calculating the substance's molar mass by multiplying its relative atomic mass to the molar mass constant (1 g/mol).The molar mass constant is then multiplied by the given mass to convert mass to moles.

Example: For example, convert 20 grams of water to moles of water. The molar mass of water is 20 g/mol. Therefore the molecular weight of water in g/mol can be used to convert gram to mole. Thus,

20 g water×1 mol20g water

= 1 mol water. 

Grams to Grams Stoichiometry Formula

The grams to grams stoichiometry formula converts mass of one substance into that of other which cannot be done directly. Instead, it is done by converting the mass of first substance into mole using mass to mole stoichiometry formula followed by mole to mole conversion factors and then convert the mole of second substance into mass. The first step is to use molar mass as conversion factor to convert the mass of substance A into mole. The second step is to use mole ratio as conversion factor to convert mole of substance A into that of substance B. Third step is to use molar ratio to convert the mole of substance B into mass of substance B.

Gas Stoichiometry Formula

According to the “ideal gas law”, at temperature (T) in Kelvin, the volume (V) occupied by n moles of any gas has a pressure (P).

The equation for gas law is given as following:

P V = n R T.

Here R is known as the gas constant and the equation is called the ideal gas law or equation of state. Under these conditions, 1 mole of gas occupies 22.4 litres of volume. The ideal gas law and balanced gas equations are used for stoichiometry calculations of gaseous reactions using gas stoichiometry formula