The following half reactions appear in the table of the information page Br_2(I)

Question

The following half reactions appear in the table of the information page Br_2(I) + 2e^- 2Hr (aQ) Ag^+ (aq) + e6- Ag(s) using these, write a balanced net ionic equation for the redox reaction in which Br_2(I) and Ag(s) are reaction. Using the table on the information page for any tarter infraction decide if reaction that you writes is the following halt reaction appear in table on the information Using the table. F_2(g) + 2e^- 2F^-(aq) Ce^3+(aq) + 2e^- Using these, write a balanced net ionic equation for the reaction in which F_2(g) and are reaction.

Explanation / Answer

Ag (s)<--->Ag+ (aq) +e-   (1), Eo= -0.80 V

Br2+2e<-->2Br- (2), Eo=1.066

Multiplying eq.1 with 2 and addition with Eq.2 gives

2Ag(s) +Br2(l) <---->2Ag+ (aq)+2Br-, Eo= 1.066-0.8= 0.266V

If delaG is -ve, the reaction is spontaneous.

deltaG=-nFE, n= no of electrons exchanged= 2, F= 96500 and E= 0.266V

deltaG=-2*96500*0.266=-51338 joules

2.

F2+2e- -------->2F- , Eo= 2.87V (1)

Co(s) ---------->Co+2+2e-, Eo= 0.288V (2)

addition of two reactions give F2+Co -------->2F- +CO+2, Eo= 2.87+0.288= 3.158 V

deltaG=-2*96500*3.158 =-609494 joules, spontaneous.

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.