The Stoichiometry Calculator is a free online application that generates a balanced equation for a chemical equation. The online stoichiometry calculator tool speeds up computations and displays the balanced equation in a fraction of a second.
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.
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
Calculate how much water (g) is created when 16 g of methane is burned?
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.