When hydrogen sulfide reacts with oxygen, water and sulfur dioxide are produced. The balanced equation for this reaction is:

2H2S (g) + 3O2 (g) 2H2O (l) + 2SO2 (g)

If 6 moles of hydrogen sulfide react,

The reaction consumes how many moles of oxygen?

The reaction produces how many moles of water?

And how many moles of sulfur dioxide?

For 6.0 moles H2S we need 9.0 moles O2 to produce 6.0 moles H2O and 6.0 moles SO2

Explanation:

Step 1: Data given

Number of moles H2S = 6.0 moles

Molar mass of H2S = 34.1 g/mol

Step 2: The balanced equation

2H2S (g) + 3O2 (g) → 2H2O (l) + 2SO2 (g)

Step 3: Calculate moles O2

For 2 moles H2S we need 3 moles O2 to produce 2 moles H2O and 2 moles SO2

For 6.0 moles H2S we need 3/2 * 6.0 = 9.0 moles O2

Step 4: Calculate moles H2O and SO2

For 6.0 moles H2S we'll produce 6.0 moles H2O and 6.0 moles SO2

For 6.0 moles H2S we need 9.0 moles O2 to produce 6.0 moles H2O and 6.0 moles SO2