According to the following reaction, how many grams of sulfur are formed when 37.4 g of water are formed? 2 H2S(g) + SO2(g) → 3 S(s) + 2H2O(l)

Mass = 100.8 g

Explanation:

Given data:

Mass of sulfur form = ?

Mass of water formed = 37.4 g

Solution:

Chemical equation:

2H₂S + SO₂      →      3S + 2H₂O

Number of moles of water:

Number of moles = mass/molar mass

Number of moles = 37.4 g/ 18 g/mol

Number of moles = 2.1 mol

Now we will compare the moles of water with sulfur.

                   H₂O        :         S

                      2          :         3

                  2.1           :     3/2×2.1 = 3.15 mol

Mass of sulfur:

Mass = number of moles × molar mass

Mass = 3.15 mol ×  32 g/mol

Mass = 100.8 g

  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-