Determine the non-standard potential of the following redox reaction if [Fe2+]0 = 0.500 M, [Fe3+]0 = 0.125 M, [MnO4-]0 = 0.050 M, and [Mn2+]0 = 0.045 M at pH = 7.0. 5 Fe2+(aq) + MnO4-(aq) + 8 H+(aq) ? 5 Fe3+(aq) + Mn2+(aq) + 4 H2O(l)
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First, we need to write the balanced redox reaction: 5 FeĀ²āŗ(aq) + MnOāā»(aq) + 8 Hāŗ(aq) ā 5 FeĀ³āŗ(aq) + MnĀ²āŗ(aq) + 4 HāO(l) Show moreā¦
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Determine the non-standard potential of the following redox reaction if [Fe2+] = 0.500 M; [Fe3+] = 0.125 M, [MnO4-] = 0.050 M, and [Mn2+] = 0.045 M at pH = 7.0. 5 Fe2+(aq) + MnO4-(aq) + 8 H+(aq) ā 5 Fe3+(aq) + Mn2+(aq) + 4 H2O(l)
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Given the following standard reduction potentials: MnO4-(aq) + 8H+(aq) + 5e- ā Mn2+(aq) + 4H2O(l) EĀ° = 1.51 V Fe3+(aq) + e- ā Fe2+(aq) EĀ° = 0.77 V What is the cell potential E for the following reaction under the non-standard condition with 0.18 M of MnO4-, 0.87 M of Mn2+, 0.92 M of Fe3+, and 0.451 M of Fe2+ in a buffered solution with 1.0 M of H+? Please keep your answer to two decimal places. 5Fe2+(aq) + MnO4-(aq) + 8H+(aq) ā 5Fe3+(aq) + Mn2+(aq) + 4H2O(l)
For the following reaction at 25Ā°C, 5Fe2+(aq) + MnO4^-(aq) + 8H+(aq) ā 5Fe3+(aq) + Mn2+(aq) + 4H2O(l), calculate (a) the standard potential, (b) the equilibrium constant, and (c) the potential under these conditions: [Fe2+] = 0.50 M, [Fe3+] = 0.10 M, [MnO4^-] = 0.025 M, [Mn2+] = 0.015 M, and a pH of 7.00.
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