The disproportionation of MnO2(s) toMn2+(aq) and MnO?4(aq) in acidsolution at 25 ?C [The reduction potential ofMnO?4(aq) to MnO2(s) is 1.68 V.]
Calculate ?G?rxn and K.
Please only full solutions with steps. I've tried this and keepgetting the wrong answer and I can't figure out why
The disproportionation of MnO2(s) toMn2+(aq) and MnO?4(aq) in acidsolution at 25 ?C [The reduction potential ofMnO?4(aq) to MnO2(s) is 1.68 V.]
Calculate ?G?rxn and K.
Please only full solutions with steps. I've tried this and keepgetting the wrong answer and I can't figure out why
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Pls Pls only answer if you are going to answer all of them and not just one or two thanks i got alot in my hands cuz of finals, and don't have time to do them, Appreciate it, trust that they'll be right , I posted this once but they only did one instead of all six so yeah thanks
1) The electrochemical cell described by the balanced chemical equation has a standard emf of 0.35 V. Calculate the value (J) for the Wmax that the cell can do under standard conditions. Round your answer to 3 significant figures.
2MnO42-(aq) + 2Hg2+(aq) â 2MnO4-(aq) + Hg22+(aq)
| St. Red. Pot. (V) | ||||
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| Faraday's Constant | ||||
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2) The voltaic cell described by the balanced chemical reaction has a standard emf of 4.05 V. Calculate the equilibrium constant (Kc) for the reaction at 25 oC. Round your answer to 3 significant figures. F2(g) + Mn(s) â 2F-(aq) + Mn2+(aq)
| St. Red. Pot. (V) | ||||
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| Constants | ||||
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| Faraday's Constant | ||||
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3) The voltaic cell described by the cell notation has an Eo of 0.68 V. Calculate the Wmax (kJ) the cell has done if 6.4700 mol of MnO4-(aq) (Molar Mass - 118.94 g/mol) reacts. Round your answer to 3 significant figures.
Pt(s) l VO2+(aq), VO2+(aq), H+(aq) ll H+(aq), MnO4-(aq) l MnO2(s) l Pt(s)
| St. Red. Pot. (V) | ||||
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| Faraday's Constant | ||||
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4) The galvanic cell described by the cell notation has an Eo of 1.23 V. Calculate the value (kJ) for the ÎGË of the cell. Round your answer to 3 significant figures.
Pt(s), H2(g) l H2O(l), OH-(aq) ll O2(g) l OH-(aq) l Pt(s)
| St. Red. Pot. (V) | ||||
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| Faraday's Constant | ||||
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5) The electrochemical cell described by the balanced chemical equation has a standard cell potential of -0.37 V. Calculate the value (kJ) for the standard free energy change of the cell. Round your answer to 3 significant figures.
Sn4+(aq) + 2Cu(s) â Sn2+(aq) + 2Cu+(aq)
| St. Red. Pot. (V) | ||||
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| Faraday's Constant | ||||
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6)The electrochemical cell described by the cell notation has an Eocell of 4.05 V. Calculate the maximum electrical work (kJ) the cell has done if 375.44 g of F2(g) (Molar Mass - 38.00 g/mol) reacts. Round your answer to 3 significant figures.
Mn(s) l Mn2+(aq) ll F2(g) l F-(aq) l Pt(s)
| St. Red. Pot. (V) | ||||
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| Faraday's Constant | ||||
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