Question

For the following example, identify the following. 2 Cl2O(g) + 2 C12(g) + O2(g) O at low temperature, the reaction is spontaneous and AG <0 and at high temperature, the reaction is spontaneous and AG < 0 at low temperature, the reaction is nonspontaneous and AG >0 and at high temperature, the reaction is spontaneous and AGO at low temperature, the reaction is spontaneous and AG <0 and at high temperature, the reaction is nonspontaneous and AG > O at low temperature, the reaction is nonspontaneous and AG >0 and at high temperature, the reaction is nonspontaneous and AG > 0 It is not possible to determine without more information.

Answer 1

The reaction described in the example is spontaneous at both low and high temperatures.

Step-by-step explanation:

In this example, 2 Cl2O(g) + 2 C12(g) + O2(g) react to form products. At low temperature, the reaction is spontaneous and AG < 0. This means that the reaction will proceed on its own without any external intervention. At high temperature, the reaction is also spontaneous and AG < 0. This indicates that the reaction will again occur without any external influence.

Answer 2

The question explores spontaneous and nonspontaneous chemical reactions in relation to Gibbs free energy (ΔG), enthalpy (ΔH°), and entropy (ΔS°). Depending on the signs and magnitudes of ΔH° and ΔS°, a reaction's spontaneity can change with temperature.

Step-by-step explanation:

The question is dealing with the concepts of spontaneity, free energy (ΔG), enthalpy (ΔH°), and entropy (ΔS°) changes in chemical reactions, which are fundamental topics in thermodynamics within Chemistry. The spontaneity of a reaction at a given temperature can be determined using the Gibbs free energy change (ΔG), which takes into account both enthalpy and entropy changes. If ΔG < 0, the reaction is spontaneous, while if ΔG > 0, the reaction is nonspontaneous.

By manipulating the Gibbs free energy equation ΔG = ΔH° - TΔS°, one can find at what temperatures a reaction becomes spontaneous or nonspontaneous. The reaction provided as an example seems to have undefined enthalpy and entropy values, so to provide a specific answer about its spontaneity, those values would be needed. Generally, if ΔH° is negative and ΔS° is positive, a reaction is likely to be spontaneous at lower temperatures. Conversely, at high temperatures, the TΔS° term may become prominent, potentially making a reaction with positive ΔH° spontaneous if ΔS° is sufficiently large.