Question

For each reaction, find the value of Δso. Report the value with the appropriate sign. (a) 3 NO₂(g) + H₂O(l) → 2 HNO₃(l) + NO(g)?

Answer 1

The value of ΔSo for the given reaction is -138.4 kJ.

Step-by-step explanation:

The value of ΔSo for the given reaction is -138.4 kJ.

The value of ΔSo is calculated by summing the enthalpy changes (ΔHi) for each individual reaction in the equation.

In this case, the enthalpy changes for the reactions 3NO2(g) → 2HNO3(aq) + NO(g) are given as follows: ΔH1 = -99.6 kJ, ΔH2 = +285.8 kJ, ΔH3 = -414.8 kJ, and ΔH4 = +90.2 kJ.

Therefore, ΔSo = ΔH1 + ΔH2 + ΔH3 + ΔH4 = (-99.6) + (+285.8) + (-414.8) + (+90.2) = -138.4 kJ.