Look at the following reaction.

Suppose that you are given the following information for this reaction at room temperature:
for SO₂(g) = -300.19 kJ/mol
for O₂ = 0.0 kJ/mol
for SO₃ = -371.1 kJmol
Find the value for ΔG° for this reaction and state whether the forward reaction is spontaneous, non-spontaneous, or at equilibrium.
a. ΔG° = 141.8 kJ / mol. The forward reaction is spontaneous.
b. ΔG° = 70.91 kJ / mol. The forward reaction is non-spontaneous.
c. ΔG° = 141.8 kJ / mol. The forward reaction is non-spontaneous.
d. ΔG° = 141.8 kJ / mol. The reaction is at equilibrium.

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answer: option (a) is the correct answer.

explanation:

the measurement of hydrogen ions in a solution is known as ph.

if ph of a solution is less than 7 then the solution is acidic. if ph of a solution is greater than 7 then the solution is basic.

when the ph of a solution equals 7, then the solution is considered as neutral.

the ph of pure water is 7, therefore, it means that concentration of hydronium ions equals that of hydroxide ions.