Question

Table 8.5 Oxidizing Strengths of Halogens Halogen tested Halide added Bromine saturated water 1 mL of 0.1 M NaCl Bromine saturated water 1 mL of 0.1 M Nal Chlorine saturated water 1 mL of 0.1 M NaBr Chlorine saturated water 1 mL of 0.1 M Nal Iodine saturated water 1 mL of 0.1 M NAD: Iodine saturated water 1 mL of 0.1 M NaCl ΤΟΤΗΤηοη η ηπατπτα, τα

Answer 1

Cl2 + 2e- --> 2Cl-           (E = 1.36V)

Br2 + 2e- --> 2Br-           (E = 1.09V)

I2 + 2e- --> 2I-                (E = 0.54V)

Oxidizing agent -- Cl2 > Br2 > I2

(i) Br2 (aq) + 2NaCl (aq) --> 2NaBr (aq) + 2Cl2 (l)

Net Ionic Equation is Br2 (aq) + 2Cl- (aq) --> 2Br- (aq) + 2Cl2 (l)

(Although this reaction is not feasible as Cl2 is better oxidising agent than Br2)

(ii) Br2 (aq) + 2NaI (aq) --> 2NaBr (aq) + 2I2 (l)

Net Ionic Equation is Br2 (aq) + 2I- (aq) --> 2Br- (aq) + 2 I2 (l)

(this reaction is feasible as Br2 is better oxidising agent than I2)

(iii) Cl2 (aq) + 2NaBr (aq) --> 2NaCl (aq) + 2Br2 (l)

Net Ionic Equation is Cl2 (aq) + 2Br- (aq) --> 2Cl- (aq) + 2Br2 (l)

(this reaction is feasible as Cl2 is better oxidising agent than Br2)

(iv) Cl2 (aq) + 2NaI (aq) --> 2NaCl (aq) + 2I2 (l)

Net Ionic Equation is Cl2 (aq) + 2I- (aq) --> 2Cl- (aq) + 2 I2 (l)

(this reaction is feasible as Cl2 is better oxidising agent than I2)

(v) I2 (aq) + 2NaBr (aq) --> 2NaI (aq) + 2 Br2 (l)

Net Ionic Equation is I2 (aq) + 2Br- (aq) --> 2I- (aq) + 2 Br2 (l)

(this reaction is Not feasible as Br2 is better oxidising agent than I2)

(vi) I2 (aq) + 2NaCl (aq) --> 2NaI (aq) + 2 Cl2 (l)

Net Ionic Equation is I2 (aq) + 2Cl- (aq) --> 2I- (aq) + 2 Cl2 (l)

(this reaction is Not feasible as Cl2 is better oxidising agent than I2)