Oxides of sulfur are important in atmospheric pollution, arising particularly from burning coal. Use the thermodynamic data at 25 C given in the appendix to answer the following questions. a. In air, the oxidation of SO2 can occur: 1 2O2(g) SO2(g) S SO3(g). Calculate rG 298

-70.87 kJ

Explanation:

Let's consider the following balanced equation.

1/2 O₂(g) + SO₂(g) ⇄ SO₃(g)

We can calculate the standard Gibbs free energy of reaction (ΔG°r) from the standard Gibbs free energies of formation (ΔG°f) using the following expression.

ΔG°r = 1 mol × ΔG°f(SO₃(g)) - 1/2 mol × ΔG°f(O₂(g) - 1 mol × ΔG°f(SO₂(g))

ΔG°r = 1 mol × (-371.06 kJ/mol) - 1/2 mol × 0 kJ/mol - 1 mol × (-300.194 kJ/mol)

ΔG°r = -70.87 kJ

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation:

your answer would be “dry”