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)
VO2+/VO2+: +1.00
MnO4-/MnO2 :+1.68
Faraday's Constant
F = 96485 C
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)
H2O/H2: -0.83
O2/OH- : +0.40
Faraday's Constant
F = 96485 C
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)
Cu+/Cu: +0.52
Sn4+/Sn2+: +0.15
Faraday's Constant
F = 96485 C
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)
Mn2+/Mn: -1.18
F2/F- : +2.87
Faraday's Constant
F = 96485 C
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)
VO2+/VO2+: +1.00
MnO4-/MnO2 :+1.68
Faraday's Constant
F = 96485 C
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)
H2O/H2: -0.83
O2/OH- : +0.40
Faraday's Constant
F = 96485 C
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)
Cu+/Cu: +0.52
Sn4+/Sn2+: +0.15
Faraday's Constant
F = 96485 C
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)
Mn2+/Mn: -1.18
F2/F- : +2.87
Faraday's Constant
F = 96485 C
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Related questions
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) | ||||
| ||||
| 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) | ||||
| ||||
| Faraday's Constant | ||||
|
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) | ||||
| ||||
| Faraday's Constant | ||||
|
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) | ||||
| ||||
| Faraday's Constant | ||||
|
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) | ||||
| ||||
| Faraday's Constant | ||||
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