During a laboratory experiment, 36.12 grams of Aboz was formed when O2 reacted with aluminum metal at 280.0 K and 1.4 atm. What was the volume of O2 used during the experiment?
30 2+ 4A1 -- 2AI2O3
8.70 liters
9.22 liters
10.13 liters
12.81 liters

8.70 liters

Explanation:

First we convert 36.12 g of AI₂O₃ into moles, using its molar mass:

Then we convert AI₂O₃ moles into O₂ moles, using the stoichiometric coefficients of the reaction:

We can now use the PV=nRT equation to calculate the volume, V:

"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."

2b2t

explanation:

2b2t