What is the definition of an equivalent?
a lab procedure requires 1.25 equivalents of zinc powder. How do I determine how much zinc that is?
Technically, we don't know eqivalents without a reaction but there are three definitions that are usually used.
The strict definition for chemistry is that amount of substance that will react with 1 g H2.
For your question, the equivalent weight of Zn is the atomic mass of Zn divided by the valence (Zn usually is 2+.)
I am performing debromination of 1,2-diphenylethane. the reaction is a 1:1 ratio of moles.
I have .41g of the dibromide compound and I need 1.25 equivalents of zinc. How many moles of zinc is that?
63.38/2 = 31.69g = 1 eq.
1.25 eq would be 1.25*31.69 = about 49.86g.
mols = grams/molar mass= about 0.625 mols.
An equivalent is a unit of measurement used in chemistry to compare the amounts of different substances involved in a reaction. It is based on the concept of equivalent weight, which is the mass of a substance that combines with or displaces one mole of hydrogen ions (H+) during a chemical reaction.
To determine how much zinc powder is needed for a lab procedure that requires 1.25 equivalents of zinc, you need to know the equivalent weight of zinc powder. The equivalent weight of zinc is calculated by dividing its atomic weight by the number of equivalents involved in the reaction.
The atomic weight of zinc is 65.38 g/mol, and in this case, we need 1.25 equivalents. So, we can calculate the amount of zinc powder required using the following formula:
Amount of zinc powder = equivalent weight of zinc × number of equivalents
Amount of zinc powder = (atomic weight of zinc / equivalents) × number of equivalents
Amount of zinc powder = (65.38 g/mol / 1 eq) × 1.25 eq
By plugging in the values, we find:
Amount of zinc powder = 65.38 g/mol × 1.25
Amount of zinc powder = 81.725 g
Therefore, you would need approximately 81.725 grams of zinc powder for the lab procedure that requires 1.25 equivalents of zinc.