Consider the following spontaneous reaction between what are the signs (+, -, or

Question

Consider the following spontaneous reaction between what are the signs (+, -, or 0) of delta H, delta S, and delta G, explain. Will this reaction become non spontaneous at higher or lower spontaneous at all temperatures? What is delta G degree at900k for the reaction: 2Co(s) + O_2 (g) rightarrow 2CaO(s) (delta H degree and delta G degree_m are respectively -1269.8 kJ and -1161.5 kJ at 298K) Ethylene oxide. C_2H_4O, is used to make antifreeze. It is produced Industrially by the catalyzed air oxidation of ethylene: At 298K delta G degree f equals 68.1 kJ/mol and -13.1 kJ/mol for C_2H_4 (g) and C_2H_4O (g) respectively. What is delta G degree_tax 298K. Is this reaction spontaneous at this temperature?

Explanation / Answer

Q1

A)

plenty of moles are becoming organized molecules, so this is getting ordered, i.e. chaos decreases, so entropy decreases

If spontanous:

dG = dH - T*dS

dG must be negative... since this is "spontanous" and dG < 0 always for forward reactions

dH must be negative... since dG is negative, and dS is possitive, so

dH >> T*dS

b)

the reaction will be nonspontanous at high T, since dH < T*dS if T*dS is large

For all further questions, please post multiple question in multiple set of Q&A. We are only allowed to answer to a single question per Q&A

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

---