Considering the fact that the formation of a bond between two atoms is exothermi

Question

Considering the fact that the formation of a bond between two atoms is exothermic and is accompanied by an entropy decrease, explain why all chemical compounds decompose into individual atoms if heated to a high enough temperature. Select all that apply.       

1)Breaking a bond into atoms always has a positive ?S.                      

2)Breaking a bond into atoms always has a negative ?S.

3)This type of reaction becomes spontaneous at high temperature.

4)This type of reaction is spontaneous at low temperature.

5)Bond breaking always has a negative ?H.

6)Bond breaking always has a positive ?H.

Explanation / Answer

   Bond breaking always has a positive ?H.
Breaking a bond into atoms always has a positive ?S.
This type of reaction is spontaneous at low temperature.

Basics:
Bond formation is always exothermic(energy is released)
Bond breaking is always endothermic(energy is absorbed)

Compounds that have negative free energy changes are stable with respect to decomposition into their constituent elements. If decomposistion occur the condition is not stable, hence it has positive value of Gibbs free energy.

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