Question

Hydrogen sulfide (H2S) burns in the air to produce sulfur dioxide and water according to the equation

2H2S + 3O2 --> 2SO2 + 2H2O
State the molecular, molar, and mass relationships indicated by equation

Answer 1

The balanced equation:

2H2S + 3O2 → 2SO2 + 2H2O

indicates the following relationships:

Molecular relationship: For every 2 molecules of hydrogen sulfide (H2S) that react, 3 molecules of oxygen (O2) are consumed, producing 2 molecules of sulfur dioxide (SO2) and 2 molecules of water (H2O).

Molar relationship: For every 2 moles of H2S that react, 3 moles of O2 are consumed, producing 2 moles of SO2 and 2 moles of H2O.

Mass relationship: The ratio of masses of the reactants and products in the balanced equation can be used to calculate the mass relationship. The equation indicates that 2 moles of H2S react with 3 moles of O2, producing 2 moles of SO2 and 2 moles of H2O. Therefore, the mass of H2S consumed is proportional to the mass of O2 consumed, and the masses of SO2 and H2O produced are proportional to each other.

Answer 2

The equation 2H2S + 3O2 --> 2SO2 + 2H2O represents molecular, molar, and mass relationships. Two molecules of H2S react with three molecules of O2 to yield two molecules of SO2 and two of H2O, which is also a molar ratio of 2:3:2:2, respectively. The mass of O2 needed to produce 4.60 mol SO2 would be 220.8 grams, considering the molar mass of O2 (32 g/mol).

When hydrogen sulfide (H2S) burns in the air, it reacts with oxygen (O2) to produce sulfur dioxide (SO2) and water (H2O). The balanced chemical equation for this reaction is 2H2S + 3O2 --> 2SO2 + 2H2O. This equation indicates several relationships:

Molecular relationship: 2 molecules of H2S react with 3 molecules of O2 to produce 2 molecules of SO2 and 2 molecules of H2O.

Molar relationship: 2 moles of H2S react with 3 moles of O2 to produce 2 moles of SO2 and 2 moles of H2O, as indicated by the coefficients in the balanced equation.

Mass relationship: To determine the mass of O2 consumed to produce a certain amount of SO2, we use the molar mass of the substances involved. For instance, to produce 4.60 mol of SO2, we require 6.90 mol of O2 (since the ratio of O2 to SO2 is 3:2), which is equivalent to 6.90 mol * 32 g/mol (molar mass of O2) = 220.8 grams of O2.