How many grams of copper(II) fluoride are needed to make 6.7 L of a 1.2 M solution?

816.40572 grams CuF2 OR 820 grams CuF2 (with sigfigs)

Explanation: To find the amount in grams, you first have to find it in moles and use the molar mass as a conversion factor to convert it into grams. To find the amount in moles you must switch around the formula for molarity. Molarity = number of moles / volume or M = n/V. As you can see, the unit for molarity is M or moles/liter and the units for volume is liters. All you have to do is switch the equation around so you are solving for number of moles, or n. The switched equation looks like n = MV. So, you just have to multiply the amount of liters and the molarity and then convert to grams. 6.7 liters*1.2 moles/liter = 8.04 moles CuF2 (the liters cancel out). Then you have to convert to moles: 8.04 moles CuF2*101.543 grams/mol CuF2 = 816.40572 grams CuF2. If you want the answer with significant figures, it would be 820 grams CuF2.

"among the transition metal elements, manganese and zinc have a slight lowering of electronegativities. the reason behind this is that the nuclear charges of these elements are slightly weaker than the other transition metal elements due to the way their valence electrons are filled up. both manganese and zinc have their valence electrons filled up to the 4th shell with 1 pair of electrons (4s2) completely occupying it. although the electrons in the 3rd shell (3d) are yet to be paired since the outer most shell is filled up, the ability of the nucleus to attract electrons is lessened. hence,   the electronegativity (or the ability to attract electrons) is lessened."

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.