Problem: Predict the sign of ΔS° for each of the following reactions. In addition, given the ΔH° values provided, predict at what temperatures (if any) the reactions would be spontaneous in the forward direction: low temperatures, high temperatures, or all temperatures. Circle your final answers.2 CO (g) + O2 (g) → 2 CO2 (g),   ΔH° = -566.0 kJ/mol(Circle One) Sign of ΔS°: +       -Spontaneous at (Circle One):i) Low temperaturesii) High temperaturesiii) All temperaturesiv) Not spontaneous at any temperatures

FREE Expert Solution

We’re being asked to determine predict the sign of ΔS where the reaction is spontaneous and ΔH is negative

Recall that when ΔH and ΔS are given, we can determine the spontaneity of the reaction based on their signs

We can use the Punnett square shown below:

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Problem Details

Predict the sign of ΔS° for each of the following reactions. In addition, given the ΔH° values provided, predict at what temperatures (if any) the reactions would be spontaneous in the forward direction: low temperatures, high temperatures, or all temperatures. Circle your final answers.

2 CO (g) + O2 (g) → 2 CO2 (g),   ΔH° = -566.0 kJ/mol

(Circle One) Sign of ΔS°: +       -

Spontaneous at (Circle One):

i) Low temperatures

ii) High temperatures

iii) All temperatures

iv) Not spontaneous at any temperatures