Zinc sulfide and oxygen gas react to form zinc oxide and sulfur dioxide. Determine the amount (g) of SO2 that should be produced in a reaction between 32.5 g of ZnS and 23.3 g of oxygen gas. What is the mass of the xs reactant?

7.30g O₂ are in excess and 21.3g of SO₂ should be produced.

Explanation:

The reaction of Zinc sulfide (ZnS) with oxygen (O₂) produce ZnO and SO₂ as follows:

2ZnS + 3O₂ → 2ZnO + 2SO₂

Using this reaction we can find the amount of SO₂ produced converting the ZnS and O₂ to moles and finding limiting and excess reactant as follows:

Moles ZnS -Molar mass: 97.47g/mol-:

32.5g * (1mol / 97.47g) = 0.333 moles ZnS

Moles O₂ -Molar mass: 32g/mol-:

23.3g O₂ * (1mol / 32g) = 0.728 moles O₂

For a complete reaction of the 0.333 moles of ZnS are required:

0.333 moles ZnS * (3mol O₂ / 2mol ZnS) = 0.500 moles O₂.

As there are 0.728 moles of O₂, limiting reactant is ZnS and excess reactant is O₂.

The moles and mass of O₂ in excess are:

0.728mol - 0.500mol = 0.228moles O₂ * (32g / mol) = 7.30g O₂ are in excess

The produced mass of SO₂ -Obtained from the moles of ZnS- is:

0.333 moles of ZnS * (2mol SO₂ / 2mol ZnS) = 0.333 moles SO₂

0.333 moles SO₂ * (64.066g / mol) =

"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."

3 1/4 %

explanation: