Consider the following reaction at constant P.Use the information here to determine the value of ΔS_surrat 355 K.Predict whether or not this reaction will be spontaneous at this temperature. 2 NO(g)+ O₂(g)→ 2 NO₂(g)ΔH = -114 kJ

Question

Quizplus · Accepted Answer

The change in entropy of the surroundings ($\Delta S_{surr}$) can be calculated using the formula $\Delta S_{surr} = -\Delta H/T$, where $\Delta H$ is the change in enthalpy (in joules) and $T$ is the temperature in Kelvin. Given $\Delta H = -114 kJ = -114,000 J$ and $T = 355 K$, $\Delta S_{surr} = -(-114,000 J) / 355 K = +321 J/K$. Since $\Delta S_{surr}$ is positive, the reaction is spontaneous at this temperature.

Consider the Following Reaction at Constant P