Calculate the equilibrium constant for the oxidation of bromine by ozone at 298 K. O 3 (g)+ 2 H + (aq)+ 2 e - $\to$ H 2 O( ) E° = +2.08 V BrO 3 - (g)+ 6 H + (aq)+ 5 e - $\to$ Br 2 (s)+ 3 H 2 O( ) E° = +1.52 V

The balanced chemical equation for the reaction is: 3 Br2(g) + 6 O3(g) → 6 BrO3-(aq) + 9 O2(g) Using the relationship ΔG° = -RT ln K, we can solve for the equilibrium constant: ΔG° = -nFE° ΔG° = -6 mol(-96.485 kJ/mol V)(2.08 V) ΔG° = 913.5 kJ/mol K = e^(-ΔG°/RT) K = e^(-913500 J/mol / (8.31 J/mol K)(298 K)) K = 3.93 x 10^10 Therefore, the answer is D, 3.93 x 10^10.

Calculate the equilibrium constant for the oxidation of bromine by ozone at 298 K. O 3 (g)+ 2 H + (aq)+ 2 e - $\to$ H 2 O( ) E° = +2.08 V BrO 3 - (g)+ 6 H + (aq)+ 5 e - $\to$ Br 2 (s)+ 3 H 2 O( ) E° = +1.52 V

The balanced chemical equation for the reaction is: 3 Br2(g) + 6 O3(g) → 6 BrO3-(aq) + 9 O2(g) Using the relationship ΔG° = -RT ln K, we can solve for the equilibrium constant: ΔG° = -nFE° ΔG° = -6 mol(-96.485 kJ/mol V)(2.08 V) ΔG° = 913.5 kJ/mol K = e^(-ΔG°/RT) K = e^(-913500 J/mol / (8.31 J/mol K)(298 K)) K = 3.93 x 10^10 Therefore, the answer is D, 3.93 x 10^10.

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Calculate the Equilibrium Constant for the Oxidation of Bromine by Ozone

Question 84

Multiple Choice

Calculate the equilibrium constant for the oxidation of bromine by ozone at 298 K. O₃(g) + 2 H⁺(aq) + 2 e^- $\to$ H₂O( $Calculate the equilibrium constant for the oxidation of bromine by ozone at 298 K. O3(g) + 2 H+(aq) + 2 e- \to H2O( ) E° = +2.08 V BrO3-(g) + 6 H+(aq) + 5 e- \to Br2(s) + 3 H2O( ) E° = +1.52 V A) 2.88 \times 109 B) 3.47 \times 10-10 C) 6.47 \times 1060 D) 3.93 \times 1094 E) 8.83$ )
E° = +2.08 V
BrO₃^-(g) + 6 H⁺(aq) + 5 e^- $\to$ $Calculate the equilibrium constant for the oxidation of bromine by ozone at 298 K. O3(g) + 2 H+(aq) + 2 e- \to H2O( ) E° = +2.08 V BrO3-(g) + 6 H+(aq) + 5 e- \to Br2(s) + 3 H2O( ) E° = +1.52 V A) 2.88 \times 109 B) 3.47 \times 10-10 C) 6.47 \times 1060 D) 3.93 \times 1094 E) 8.83$ Br₂(s) + 3 H₂O( $Calculate the equilibrium constant for the oxidation of bromine by ozone at 298 K. O3(g) + 2 H+(aq) + 2 e- \to H2O( ) E° = +2.08 V BrO3-(g) + 6 H+(aq) + 5 e- \to Br2(s) + 3 H2O( ) E° = +1.52 V A) 2.88 \times 109 B) 3.47 \times 10-10 C) 6.47 \times 1060 D) 3.93 \times 1094 E) 8.83$ )
E° = +1.52 V

A) 2.88 $\times$ 10⁹
B) 3.47 $\times$ 10^-10
C) 6.47 $\times$ 10⁶⁰
D) 3.93 $\times$ 10⁹⁴
E) 8.83

Correct Answer:

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