Balance the following chemical reaction in base, using the method for redox equa

Question

Balance the following chemical reaction in base, using the method for redox equations. Show your work. ClO^- + I^rightarrow Cl^- + I_2 Consider the galvanic cell based on the following two half-reactions: Au^3+ + 3e^- rightarrow Au epsilon^degree = 1.50V TI^+ + 1e^- rightarrow TI epsilon^degree = -0.34V a) Calculate and epsilon^degree _, delta G^degree, and K_eq for the galvanic cell at 25 degree C. b) Calculate epsilon_ at 25 degree C when [Au^3+] = 0.0010 M and [TI^+] = 10 times 10^-4 M. Describe rust and how to prevent it.

Explanation / Answer

(8)

ClO- + I- -----------> Cl- + I2

(i) seprate oxdiation and reduction half reactions

I- ------------> I2              oxidation half reaction

ClO- ------------> Cl-       reduction half reaction

(ii) Balance all atoms other than O and H

2 I- ------------> I2      

ClO- ------------> Cl-   

(iii) To balance oxygens in acidic medium add H2O molecules

2 I- ------------> I2      

ClO- ------------> Cl- + H2O

(iv) To balance hydrogens in acidic medium add H+ ions

2 I- ------------> I2      

ClO- + 2 H+ (aq.) ------------> Cl- + H2O

(v) To balance chages add electrons

2 I- ------------> I2 + 2 e

ClO- + 2 H+ (aq.) + 2 e ------------> Cl- + H2O

(vi) To equalise electrons in both half reactions multiply with suitable numbers.

2 I- ------------> I2 + 2 e

ClO- + 2 H+ (aq.) + 2 e ------------> Cl- + H2O

(vii) Add both half reactions to get final balanced equation.

ClO- + 2 H+ (aq.) + 2 I- ------------> I2 + Cl- + H2O

This is the balanced equation

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