Hydrogen sulfide gas gives rotten eggs their terrible odor. hydrogen sulfide burns in air (o2) to produce sulfide dioxide gas and water vapor. in 1.38 moles of sulfide dioxide are produced when this reaction occurs, how many moles of oxygen were required?

2.07 mol O₂

Explanation:

First we need to write down the species present in the chemical equation, using the information given by the exercise:

However this equation is not balanced, so now we balance it:

Now we can use the stoichiometric ratio to calculate the moles of oxygen from the moles of sulfide dioxide:

  the   balanced   equation   for   reaction of   ca metal   with   o2 to   produce   cao   is as below

2 ca+ o2→ 2 cao2

  explanation

the reaction is   balanced     since the   number of atoms   in reactant side is   equal to   number of atoms   in   product side.   for   example   they   are 2   atom of   ca in   reactant   side   and   2   atoms of ca   in   the product side.

  the   process   is a   meet the   requirement   of   redox   reaction because :     calcium   is   oxidized   from   oxidation state 0   to 2+   while   oxygen   is reduced from   oxidation   state   0   to 2-