Stoichiometry Calculator

The quantitative link between reactants and products in a chemical process is expressed using stoichiometry. The stoichiometric coefficients in a balanced equation represent the molar ratios in the reaction. It enables for the prediction of particular quantities such as a gas's product or molar mass, percent yield, and so on.

• For the first letter, use uppercase, and for the second letter, use lowercase.
• Before and after the + and -> signs, there must be one space.

• When a chemical change happens, a chemical reaction occurs. Ex: Magnesium (Mg) + Oxygen (O) = Magnesium oxide, for example (MgO).
• The reactants are the components that change chemically during the reaction.
• The new substances generated during the reaction are referred to as products.
• Magnesium (Mg) + Oxygen (O) = Magnesium oxide, for example (MgO). Magnesium and oxygen are the reactants in this equation, while magnesium oxide is the result.

Mass cannot be generated or destroyed in a chemical reaction, according to the rule of conservation of mass. That is, the total mass of elements present in a chemical reaction's products must equal the total amount of elements present in the reactants.

Before and after a chemical reaction, the number of atoms on each element remains constant. For instance:- (i) 2Mg + O₂ à 2MgO (ii) Zn + H₂SO₄ à ZnSO₄ + H₂

Stoichiometry chemical equation of balance

• CH₄(g) + 2O₂ (g) à CO₂ (g) + 2H₂O (g).
• The information obtained from the aforesaid reaction is as follows
  • When one mole of CH₄ (g) interacts with two moles of O₂ (g), one mole of CO₂ (g) and two moles of H₂O are produced (g).
  • When one molecule of CH₄ (g) interacts with two molecules of O₂ (g), one molecule of CO₂ (g) and two molecules of H₂O are produced (g).
  • 16 g CH₄ (g) interacts with 232 g O₂ (g) to produce 44 g CO₂ (g) and 218 g H₂O. (g).

Calculate how much water (g) is created when 16 g of methane is burned?

Solution:

The balanced equation for methane combustion is CO₂ (g) + 2H₂O à CH₄ (g) + 2O₂ (g) (g)

1 One mole is equal to 16 g of CH₄.

Using the equation above, 1 mol of CH₄ (g) yields 2 mol of H₂O. (g)

2 mol water (H₂O) equals 2 (2+16) = 2 18 = 36 g

1 mol H₂O = 18 g H₂O ⇒ (18g H₂O)/ (1 mol H₂O) = 1

As a result, 2 mol H₂O (18g H₂O)/ (1 mol H₂O)

= 36 g H₂O = 2 18 g H₂O

1. What is meant by Stoichiometry?

Stoichiometry is used to express the quantitative relationship between reactants and products in the chemical equation.

2. 1. What is the stoichiometric calculation, and how does it work?

The majority of stoichiometric calculations are based on chemical formulas. The mass of a material is defined as the total of the atomic weights of all the atoms in the molecule. The mass of Na₂S, for example, is computed as 2(23) + 1(32) = 78.

3. What method do you use to calculate the mole ratio?

Divide the number of moles of each element by the least number of moles to find the ratio or moles of each element. Because there are fewer moles of oxygen than any other element, we'll use one mole to calculate the ratios.