The SI unit representing the number of particles in a measured amount of substance is the . Molecular mass is the total of the masses of all atoms in one molecule
of a compound and is measured in . Molar mass for the same compound is the
same number, measured in grams per mole, and represents the mass of substance containing
one . One mole of a substance has atoms or
molecules. This number is known as number. To determine the
number of moles in a sample of an element, compound, or molecule, the mass of the
substance measured in is divided by the molar mass of the substance.
How many moles are contained in 24 grams of carbon? To determine the number of moles, first
find the molar mass of carbon. The molar mass is g/mol. Divide
grams by the molar mass. There are moles of
carbon in the sample.

Calculate the expected ph values of the buffer systems from the experiments (a,b,c,d), using the henderson- hasselbalch equation, ph-pka+log[a-]/[ha]. use for pka values carbonic acid= 6.37, and acetic acid= 4.75.

Oxidation-reduction reactions (often called "redox" for short) are reactions that involve the transfer of electrons from one species to another. oxidation states, or oxidation numbers, allow chemists to keep track of these electron transfers. in general, one element will lose electrons (oxidation), with the result that it will increase in oxidation number, and another element will gain electrons (reduction), thereby decreasing in oxidation number. the species that is oxidized is called the reducing agent or reductant. the species that is reduced is called the oxidizing agent or oxidant. to sum up: oxidation = increase in oxidation state = loss of electrons = reducing agent reduction = decrease in oxidation state = gain of electrons = oxidizing agent part a which element is oxidized in this reaction? fe2o3+3co→2fe+3co2 enter the elemental symbol. view available hint(s) is oxidized part b which element is reduced in this reaction? 2hcl+2kmno4+3h2c2o4→6co2+2mno2+2kcl+4h2o enter the elemental symbol. view available hint(s) is reduced

The atom fluorine generally will become stable through the formation of an ionic chemical compound by accepting electron(s) from another atom. this process will fill its outer energy level of electrons.