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| The study of quantitative relationships between the amounts of reactants used and products formed by chemical reaction; is based on the law of conservation of mass. | ||
| Ratio between the numbers of moles of any two of the substances in a balanced chemical equation. | ||
| a variable whose values are solutions of an equation | ||
| a whole number that appears in front of a formula in a chemical equation | ||
| a chemical equation in which mass is conserved; each side of the equation has the same number of atoms of each element. | ||
| a ratio of equivalent values used to express the same quantity in different units; is always equal to 1 and changes the units of a quantity without changing its value | ||
| the mass in grams of 1 mol of a substance | ||
| the amount of product actually produced when the chemical reaction is carried out in an experiment | ||
| the amount of product that could form during a reaction calculated from a balanced chemical equation; it represents the maximum amount of product that could be formed from a given amount of reactant | ||
| actual yield/theoretical yield x 100% | ||
| a reactant that is totally consumed during a chemical reaction, limits the extent of the reaction, and determines the amount of product | ||
| # of particles in 1 mole of a pure substance (rounded to 6.022 x 10 to 23rd power); number of atoms in exactly 12 grams of a Carbon-12 isotope. | ||
| states that mass is neither created nor destroyed during ordinary chemical reactions or physical changes. |
