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Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 °C Cu(s) Cu2 (0...
Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at...
Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 °C Cu(s) Cu2+ (0.15 M) Fe2+ (0.0039 M) Fe(s) E =-0.440 V E+Cu = 0.339 V Fe2+/Fe Is the electrochemical cell spontaneous or not spontaneous -0.779 Ecell = as written at 25 C? not spontaneous spontaneous о Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 'C Pt(s) Sn2 (0.0024 M), Sn4+ (0.12 M) |...
Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at...
Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 °C. Cu(s) Cu2+(0.14 M) | Fe2+(0.0044 M) Fe(s) Ecu?+Icu = 0.339 V Efez lfe = -0.440 V Ecell = v Is the electrochemical cell spontaneous or not spontaneous as written at 25 °C? O not spontaneous O spontaneous Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 °C. Pt(s) Sn2+(0.0048 M), Snº+(0.11 M) || Fe3+(0.12...
Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at...
Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 ∘ C . Cu ( s ) ∣ ∣ Cu 2 + ( 0.13 M ) ∥ ∥ Fe 2 + ( 0.0011 M ) ∣ ∣ Fe ( s ) E ∘ Cu 2 + / Cu = 0.339 V E ∘ Fe 2 + / Fe = − 0.440 V E cell = V
Answers and detailed explanations For the following electrochemical cell, calculate the potential and determine if the...
Answers and detailed explanations
For the following electrochemical cell, calculate the potential and determine if the cell reaction is spontaneous as written at 25 °C. Cu(s)|Cu2+(0.15 M)||Fe2+(0.0020 M)|Fe(s) Ecuaticu = 0.339 V Efez-ffe = -0.440 V Ecell = Determine if the cell reaction is spontaneous as written. O spontaneous O not spontaneous
For the spontaneous as written at 25°C. A) Cu(s) I Cu (0.10 M)IFe (0.0053 M) I...
For the spontaneous as written at 25°C. A) Cu(s) I Cu (0.10 M)IFe (0.0053 M) I Fe(s) O Spontaneous O Not B) Pt(s) ISn2(0.0021 M), Sn (0.15 M) II Fe2 (0.0012 M), Fe (0.12 M) I Pt(s) O Not Spontaneous
4. Use the table below to provide a redox reaction involving the spontaneous oxidation of Cr...
4. Use the table below to provide a redox reaction involving the spontaneous oxidation of Cr (balance your final reaction and provide the Ecell). Half-reaction E (V) Cr3+ (aq) + 3e Cr(s) -0.74 Fe(s) -0.440 Fe3+ (aq) + → Fe2+ (s) +0.771 Sn4+ (aq) + 2e Sn2+ (aq) +0.154 Fe2+ (aq) + 2e-
Half-reaction Cr3+ (aq) + 3e- → Cr(s) Fe2+ (aq) + 2e- → Fe (s) Fe3+ (aq) + e- + Fe2+ (s) Sn4+ (aq) + 2e- + Sn2+ (aq...
Half-reaction Cr3+ (aq) + 3e- → Cr(s) Fe2+ (aq) + 2e- → Fe (s) Fe3+ (aq) + e- + Fe2+ (s) Sn4+ (aq) + 2e- + Sn2+ (aq) E° (V) -0.74 -0.440 +0.771 +0.154 3Sn** (aq) +2Cr(s) → 2Cr** (aq) +3Sn²+ (aq) 3. What is the cell potential, Ecell, for the reaction above if [Sn] = 1.00 M, [Cr3+1 = 0.0200 M and [Sn2+] = 0.0100 M?
2. Using the information provided, calculate the standard cell potential, Eºcell, for the reaction below: Half-reaction...
2. Using the information provided, calculate the standard cell potential, Eºcell, for the reaction below: Half-reaction Cr3+ (aq) + 3e- → Cr(s) Fe2+ (aq) + 2e- → Fe(s) Fe3+ (aq) + e- + Fe2+ (s) Sn4+ (aq) + 2e- + Sn2+ (aq) E° (V) -0.74 -0.440 +0.771 +0.154 3Sn(aq) +2Cr(s) →2Cr" (aq) +35n²+ (aq)
What would be the standard cell potential for a spontaneous electrochemical cell constructed with the two...
What would be the standard cell potential for a spontaneous electrochemical cell constructed with the two metals below? Cu2+(aq) + 2e– → Cu(s) E° = 0.34 V Sn4+(aq) + 2e– → Sn2+(aq) E° = 0.13 V
What would be the standard cell potential for a spontaneous electrochemical cell constructed with the two...
What would be the standard cell potential for a spontaneous electrochemical cell constructed with the two metals below? Cu2+(aq) + 2e– → Cu(s) E° = 0.34 V Sn4+(aq) + 2e– → Sn2+(aq) E° = 0.13 V
Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 °C Cu(s) Cu2+ (0.15 M) Fe2+ (0.0039 M) Fe(s) E =-0.440 V E+Cu = 0.339 V Fe2+/Fe Is the electrochemical cell spontaneous or not spontaneous -0.779 Ecell = as written at 25 C? not spontaneous spontaneous о Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 'C Pt(s) Sn2 (0.0024 M), Sn4+ (0.12 M) |...
Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 °C. Cu(s) Cu2+(0.14 M) | Fe2+(0.0044 M) Fe(s) Ecu?+Icu = 0.339 V Efez lfe = -0.440 V Ecell = v Is the electrochemical cell spontaneous or not spontaneous as written at 25 °C? O not spontaneous O spontaneous Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 °C. Pt(s) Sn2+(0.0048 M), Snº+(0.11 M) || Fe3+(0.12...
Answers and detailed explanations
For the following electrochemical cell, calculate the potential and determine if the cell reaction is spontaneous as written at 25 °C. Cu(s)|Cu2+(0.15 M)||Fe2+(0.0020 M)|Fe(s) Ecuaticu = 0.339 V Efez-ffe = -0.440 V Ecell = Determine if the cell reaction is spontaneous as written. O spontaneous O not spontaneous
For the spontaneous as written at 25°C. A) Cu(s) I Cu (0.10 M)IFe (0.0053 M) I Fe(s) O Spontaneous O Not B) Pt(s) ISn2(0.0021 M), Sn (0.15 M) II Fe2 (0.0012 M), Fe (0.12 M) I Pt(s) O Not Spontaneous
4. Use the table below to provide a redox reaction involving the spontaneous oxidation of Cr (balance your final reaction and provide the Ecell). Half-reaction E (V) Cr3+ (aq) + 3e Cr(s) -0.74 Fe(s) -0.440 Fe3+ (aq) + → Fe2+ (s) +0.771 Sn4+ (aq) + 2e Sn2+ (aq) +0.154 Fe2+ (aq) + 2e-
Half-reaction Cr3+ (aq) + 3e- → Cr(s) Fe2+ (aq) + 2e- → Fe (s) Fe3+ (aq) + e- + Fe2+ (s) Sn4+ (aq) + 2e- + Sn2+ (aq) E° (V) -0.74 -0.440 +0.771 +0.154 3Sn** (aq) +2Cr(s) → 2Cr** (aq) +3Sn²+ (aq) 3. What is the cell potential, Ecell, for the reaction above if [Sn] = 1.00 M, [Cr3+1 = 0.0200 M and [Sn2+] = 0.0100 M?
2. Using the information provided, calculate the standard cell potential, Eºcell, for the reaction below: Half-reaction Cr3+ (aq) + 3e- → Cr(s) Fe2+ (aq) + 2e- → Fe(s) Fe3+ (aq) + e- + Fe2+ (s) Sn4+ (aq) + 2e- + Sn2+ (aq) E° (V) -0.74 -0.440 +0.771 +0.154 3Sn(aq) +2Cr(s) →2Cr" (aq) +35n²+ (aq)
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> Your way of calculating spontaneous, non spontaneous is correct. however you are using the wrong equation. You want to use the Nernst equation in this case.
Quinten Maas Mon, Jan 17, 2022 4:54 AM