PLS only answer if you know what you're doing and if you are going to answer all of them, i got alot to do cuz of finals so i'd appreciate it if you answer them all correctly, thank you
1) Calculate the standard emf (electromotive force) for a voltaic cell whose cell reaction is represented by the balanced equation.
2H2O(l) â H2(g) + H2O2(aq)
2) Calculate the standard cell potential for a galvanic cell whose cell reaction is represented by the balanced equation.
2Fe(s) + 3I2(s) â 2Fe3+(aq) + 6I-(aq)
St. Red. Pot. (V)
Fe3+/Fe -0.04 I2/I- 0.54
3) For the voltaic cell shown, calculate the standard cell potential.
Pt(s) l H2O(l), H2O2(aq), H+(aq) ll H+(aq) l H2(g), Pt(s)
St. Red. Pot. (V) H2O2/H2O 1.78 H+/H2 0
4)For the voltaic cell shown, calculate the standard cell potential.
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
5)For the galvanic cell shown, calculate the Eo.
Fe(s) l Fe2+(aq) ll Cd2+(aq) l Cd(s)
St. Red. Pot. (V)
Fe2+/Fe -0.44 Cd2+/Cd -0.40
6) The value for the standard emf of a voltaic cell described by the cell notation is 1.88 V. Determine the value (V) of the standard half cell potential for the F2/F- couple.
Au(s) l AuCl4-(aq), Cl-(aq) ll F2(g) l F-(aq) l Pt(s)
St. Red. Pot. (V)
AuCl4-/Au 0.99
St. Red. Pot. (V) H2O2/H2O 1.78 H+/H2 0
PLS only answer if you know what you're doing and if you are going to answer all of them, i got alot to do cuz of finals so i'd appreciate it if you answer them all correctly, thank you
| 1) Calculate the standard emf (electromotive force) for a voltaic cell whose cell reaction is represented by the balanced equation. 2) Calculate the standard cell potential for a galvanic cell whose cell reaction is represented by the balanced equation. St. Red. Pot. (V)
3) For the voltaic cell shown, calculate the standard cell potential.
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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) | ||||
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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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Please answer all.
1)Enter the balanced chemical equation including states that describes the electrochemical cell that is represented by the cell notation as shown.
Pt(s) l Fe2+(aq), Fe3+(aq) ll Hg2+(aq) l Hg(l)
St. Red. Pot. (V)
| Fe3+/Fe2+ | +0.77 |
| Hg2+/Hg | +0.85 |
2)Enter the balanced chemical equation including states that describes the electrochemical cell that is represented by the cell notation as shown.
Pt(s) l Fe2+(aq), Fe3+(aq) ll Hg2+(aq) l Hg(l)
| St. Red. Pot. (V) | ||||
|
3)Enter the balanced chemical equation including states that describes the electrochemical cell that is represented by the cell notation as shown.
Pt(s) l SO42-(aq), S2O82-(aq) ll Br2(l) l Br-(aq) l Pt(s)
St. Red. Pot. (V)
| S2O82-/SO42- | +2.01 |
| Br2/Br- | +1.07 |
4)Enter the balanced chemical equation including states that describes the electrochemical cell that is represented by the cell notation as shown.
Pt(s) l Pb2+(aq) l PbO2(s) l H+(aq) ll H+(aq) l MnO2(s) l Mn2+(aq) l Pt(s)
St. Red. Pot. (V)
| PbO2/Pb2+ | +1.46 |
| MnO2/Mn2+ | +1.21 |
