COMBINING WEIGHT Meaning and
Definition
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Combining weight, also known as equivalent weight or equivalent mass, is a term commonly used in chemistry. It refers to the relative mass of an element or compound that combines with or replaces one mole of hydrogen in a chemical reaction.
In chemical reactions, elements and compounds combine to form new substances. The combining weight indicates the specific quantity of an element or compound required to react with a fixed amount of another substance. It is expressed in atomic mass units (amu) and is determined by the valence or oxidation state of the element or compound.
To calculate the combining weight of an element, its atomic weight is divided by the valence number. For example, the atomic weight of sulfur is 32.07 amu, and its valence is 2. Therefore, the combining weight of sulfur is 32.07 amu divided by 2, which equals 16.035 amu.
The concept of combining weight is crucial in stoichiometry, which helps determine the relative amounts of reactants and products in a chemical reaction. It assists in balancing chemical equations and predicting how much of each substance is required for a complete reaction.
Overall, combining weight plays an essential role in understanding the quantitative aspects of chemical reactions and is fundamental to the study of chemistry.
Common Misspellings for COMBINING WEIGHT
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Etymology of COMBINING WEIGHT
The term "combining weight" is not derived from a specific etymology. Rather, it is a technical term used in chemistry to describe the mass of an element or compound that can combine with or replace a fixed amount of another element. It is defined based on the concept of atomic or molecular weight. The term "combining weight" is a combination of the words "combining", which refers to the act of two or more substances uniting chemically, and "weight", which in this context represents the mass or amount of a substance.
Similar spelling word for COMBINING WEIGHT
