Formula masses

Molarity (M) A concentration unit defined to be the number of moles of solute per liter of solution, 95q, 259 concentration unit conversion, 261-262 potassium chromate, 263 Mole A collection of6.0122 X 1023 items. The mass in grams of one mole of a substance is numerically equal to its formula mass, 55. See also Amount Mole fraction (X) A concentration unit defined as the number of moles of a component divided by the total number of moles, 116-117,261 Mole-gram conversions, 55-56,68-68q... [Pg.692]

For molecular and ionic substances, one mole of any substance is its relative molecular mass or relative formula mass expressed in grams. This is called the molar mass, i.e. the mass in grams of one mole of a substance. [Pg.16]

The empirical formula is C3H2N02, with a formula mass of 84.0 g/mol. This is one-half the experimentally determined molar mass. Thus, the molecular formula is C6H4N204. [Pg.306]

A given charge liberates different species in the ratio of their relative formula masses, divided by the number of electrons in the electrode reaction... [Pg.284]

An experiment is to be performed to determine the formula mass of a solute (KN03) through boiling-point elevation. [Pg.143]

KN03 formula mass (from data) = 95 g/mole... [Pg.144]

In the problem above, we determined the percentage data from the chemical formula. We can determine the empirical formula if we know the percent compositions of the various elements. The empirical formula tells us what elements are present in the compound and the simplest whole-number ratio of elements. The data may be in terms of percentage, or mass or even moles. However, the procedure is still the same—convert each element to moles, divide each by the smallest, and then use an appropriate multiplier if necessary. We can then determine the empirical formula mass. If we know the actual molecular mass, dividing the molecular formula mass by the empirical formula mass, gives an integer (rounded if needed) that we can multiply each of the subscripts in the empirical formula. This gives the molecular (actual) formula, which tells what elements are in the compound and the actual number of each. [Pg.39]

The empirical formula mass is 46.00 g/mol. Dividing the actual molar mass by the empirical molar mass gives ... [Pg.39]

Determine the mass percent of each of the elements in C6H12Og Formula mass (FM) = 180.158 amu... [Pg.90]

Measurements include initial and final masses, and initial and final volumes. Calculations may include the difference between the initial and final values. Using the formula mass and the mass in grams, moles may be calculated. Moles may also be calculated from the volume of a solution and its molarity. [Pg.95]

C—The general formula, C H2b, means that 1 mol of H20 will form per mole of empirical formula unit, regardless of the value of n. The moles of water formed is the mass of the alkene divided by the empirical formula mass. [Pg.275]

Thus, 24.6 years must be two half-lives of the empirical formula mass. [Pg.318]

Silver oxide, Ag20, can be decomposed to silver metal, Ag, plus oxygen gas, 02. How many moles of oxygen gas will form when 4.64 g of solid silver oxide is decomposed The formula mass of silver oxide is 232. [Pg.329]

Antibiotic Formula Mass Centers Moieties Croups Year>>... [Pg.111]

The mass spectrum shown is that for ethanol (CHjCHjOH). The 100-peak with the highest m/z ratio provides the gram formula mass of the organic compound. In the example, this appears at m/z = 46 and confirms the gram formula mass of ethanol as 46 g. [Pg.74]

Reaction Product Molar Formula Mass Percent... [Pg.275]

Chemists may distinguish between the molar masses of pure elements, molecular compounds, and ionic compounds by referring to them as the gram atomic mass, gram molecular mass, and gram formula mass, respectively. Don t be fooled The basic concept behind each term is the same molar mass. [Pg.103]

To determine a moleculcir formula, you must know the gram formula mass of the compound as well as the empirical formula (or enough information to calculate it yourself from the percent composition see the preceding section for details). With these tools in hand, calculating the molecular formula involves three steps ... [Pg.109]

What is the molecular formula of a compound that has a gram formula mass of 78 g/mol and the empirical formula NaO ... [Pg.110]

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