Question

Explain why the following statements are incorrect: 1) Entropy increases in all spontaneous reactions. 2) Reactions...

Explain why the following statements are incorrect:

1) Entropy increases in all spontaneous reactions.

2) Reactions with a negative standard free energy change (deltaG<0) are product-favored and occur with rapid transformation of reactants to products.

3) All spontaneous processes are exothermic.

Science   Chemistry   
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Answer #1

Q1

this is false, there are some reactions which will be spontaneous and they decrease in entropy, this implies that the entropy of the usrroundings increases, so the process is possilbe (entropy of universe increases overall)

Q2

the dG data only states equilibrium values, will not relate vleocities, there are dG values larg eenough which favour a reaction, but will NOT favour rapid reactions, such as C-14 decay

Q3

there are known endothermic processes, such as boiling and evaporation

the spontanoeus reactions cna be both, endothermic and exothermic

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