Search results
Results from the WOW.Com Content Network
The ideal gas law is used for these calculations. Often, but not always, the standard temperature and pressure (STP) are taken as 0 °C and 1 bar and used as the conditions for gas stoichiometric calculations. Gas stoichiometry calculations solve for the unknown volume or mass of a gaseous product or reactant.
The formula unit is used as an independent entity for stoichiometric calculations. [4] [5] Examples of formula units, include ionic compounds such as NaCl and K 2 O and covalent networks such as SiO 2 and C (as diamond or graphite). [6]
Stoichiometry is used to run calculations about chemical reactions, for example, the stoichiometric mole ratio between reactants and products. The stoichiometry of a chemical reaction is based on chemical formulas and equations that provide the quantitative relation between the number of moles of various products and reactants, including yields ...
For example, a calculation of the mass of natural gas as fuel — which often contains carbon dioxide (CO 2), nitrogen (N 2), and various alkanes — includes the mass of the carbon dioxide, nitrogen and all alkanes in determining the value of m fuel. [2] For pure octane the stoichiometric mixture is approximately 15.1:1, or λ of 1.00 exactly.
The type of equilibrium defects in non-stoichiometric compounds can vary with attendant variation in bulk properties of the material. [1] Non-stoichiometric compounds also exhibit special electrical or chemical properties because of the defects; for example, when atoms are missing, electrons can move through the solid more rapidly.
The equivalence point, or stoichiometric point, of a chemical reaction is the point at which chemically equivalent quantities of reactants have been mixed. For an acid-base reaction the equivalence point is where the moles of acid and the moles of base would neutralize each other according to the chemical reaction.
Constant level of this surface is identified from the equation (,) =, where is called as the stoichiometric mixture fraction which is obtained by setting = = (since if they were react to consume fuel and oxygen, only on the stoichiometric locations both fuel and oxygen will be consumed completely) in the definition of to obtain
For example, oxygen makes up about 8 / 9 of the mass of any sample of pure water, while hydrogen makes up the remaining 1 / 9 of the mass: the mass of two elements in a compound are always in the same ratio. Along with the law of multiple proportions, the law of definite proportions forms the basis of stoichiometry. [1]