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5. The nickel-cadmium battery, despite issues with the toxicity of Cd, is still used in some...
A rechargeable nickel-cadmium (NiCd) battery contains the following half-reactions: NiO2 +2H2O(l)+2e– → Ni(OH)2 +2OH– E0 =0.49V...
A rechargeable nickel-cadmium (NiCd) battery contains the following half-reactions: NiO2 +2H2O(l)+2e– → Ni(OH)2 +2OH– E0 =0.49V Cd(OH)2 +2e– →Cd(s)+2OH– E0 =–0.81V a. What is the standard cell potential or voltage of this NiCd cell? b. Write the net chemical reaction in the direction of spontaneous reaction. Is cadmium oxidized or reduced? c. Write an expression for the reaction quotient Q. What is Q if the electrolyte concentrations are: [NiO2] = 1 M and [Cd(OH)2] = 0.01M and [Ni(OH)2] = 0.001...
Use the tabulated electrode potentials to calculate K for the oxidation of nickel by H+: Ni(s)+2H+(aq)→Ni2+(aq)+H2(g)...
Use the tabulated electrode potentials to calculate K for the oxidation of nickel by H+: Ni(s)+2H+(aq)→Ni2+(aq)+H2(g) Express your answer using two significant figures. Standard reduction half-cell potentials at 25∘C Half-reaction E∘ (V) Half-reaction E∘ (V) Au3+(aq)+3e−→Au(s) 1.50 Fe2+(aq)+2e−→Fe(s) −0.45 Ag+(aq)+e−→Ag(s) 0.80 Cr3+(aq)+e−→Cr2+(aq) −0.50 Fe3+(aq)+3e−→Fe2+(aq) 0.77 Cr3+(aq)+3e−→Cr(s) −0.73 Cu+(aq)+e−→Cu(s) 0.52 Zn2+(aq)+2e−→Zn(s) −0.76 Cu2+(aq)+2e−→Cu(s) 0.34 Mn2+(aq)+2e−→Mn(s) −1.18 2H+(aq)+2e−→H2(g) 0.00 Al3+(aq)+3e−→Al(s) −1.66 Fe3+(aq)+3e−→Fe(s) −0.036 Mg2+(aq)+2e−→Mg(s) −2.37 Pb2+(aq)+2e−→Pb(s) −0.13 Na+(aq)+e−→Na(s) −2.71 Sn2+(aq)+2e−→Sn(s) −0.14 Ca2+(aq)+2e−→Ca(s) −2.76 Ni2+(aq)+2e−→Ni(s) −0.23 Ba2+(aq)+2e−→Ba(s) −2.90 Co2+(aq)+2e−→Co(s) −0.28 K+(aq)+e−→K(s) −2.92 Cd2+(aq)+2e−→Cd(s)...
materials question electrochemistry table has associated voltages compute the voltage at 25c of an electrochemical cell...
materials question electrochemistry
table has associated voltages
compute the voltage at 25c of an electrochemical cell
consisting of pure copper immersed in 9x10^-2M solution of Cu^2+
ions and pure nickel in a 0.35 M solution of Ni^2+ ions.
half reactions are:
Cu-> Cu^2+ + 2e- @+0.345V electrode potential
Ni-> Ni^2+ + 2e- @ -2.250V
this is all the information I was given
We were unable to transcribe this imageWe were unable to transcribe this imageWe were unable to transcribe this...
- cellpotentials and standard reduction potential table. -Determining the Nernst equation and finding the Faraday constant....
- cellpotentials and standard reduction potential table.
-Determining the Nernst equation and finding the Faraday
constant.
If you can explain how to solve for each part please.
25°C Standard Reduction Potentials in Aqueous solution a 2.87 Reduction half-reaction 2F (a 1.77 2H2O 1.692 2e 2H (a Au (s 1.085 PbSO4 (s) 2H20. Au (ag) 2e 1.51 4H20 Mn 1.50 5e 8H (a Mno4 (a Au(S 1.36 3e 2Cl (aq 1.33 2e 2Cr3 (ag) 7H20 C12 6e- 1.229 14H 2H2O 1.08...
1. How do I read the half reaction table? 2. If im asked for the best...
1. How do I read the half reaction table?
2. If im asked for the best reducing agent from Cu+, Ag+, F2, and
Fe3+, where do I look first in the table? before the arrow or after
the arrow?
3. Sometimes a value that has originally a positive (V) from the
table it will have the negative sign in a homework problem, and
viceversa, so the question is, how do I use the positive and
negative signs in respect to...
HQ18.28 Homework • Unanswered Some electrode combinations that the Phoenix spacecraft designers may have considered for...
HQ18.28 Homework • Unanswered Some electrode combinations that the Phoenix spacecraft designers may have considered for use in their design are given in the table below. Assume the ambient Martian temperature is -67.5*C, 205.7 K. What electrode combination (assume 0.1 M solutions) would provide the 1.317 V required by the spacecraft electronics? Use Appendix 11 for your standard cell potentials. А Rh+ +e- Rh/Ni2+ + 2e + NI O B Rh+ + e + Rh/Cr3+ + 3e - Cr C...
5. How much faster would a reaction be if a catalyst is used that lowers the...
5. How much faster would a reaction be if a catalyst is used that lowers the activation energy from 20.0 kJ/mol to 10.0 kJ/mol? Do the calculation at two temperatures: first at 25.0°C and then at 0.0°C. (20 points) (V) Helpful Stuff Thermodynamics: AG° = AH-TAS Nernst Equation: 6 = 6 - (RT/nF)InQ AG=RTIK At 25°C: 8 = 6 - (0.0591/n)logQ AGRT Ke=e AGⓇ =-nF8° Units/Constants: Volt: 1 V = 1 J/C Faraday: 1 F = 96,485 C/mole Arrhenius Equation:...
use tabulated standard electrode potential to calculate the standard cell potential for the reaction occurring in an el...
use tabulated standard electrode potential to calculate the
standard cell potential for the reaction occurring in an
electrochemical cell at 25 C. (The equation is balanced.)
3Ni^2+(aq)+2Cr(s)--->3Ni(s)2Cr^3+(aq)
Express your answer to two significant figures and include the
appropriate units.
em 26 E (V) -0.45 -0.50 -0.73 -0.76 -1.18 Standard reduction half-cell potentials at 25°C Half-reaction E° (V) Half-reaction Aul+ (aq) + 3e +Au(s) 1.50 Fe2+ (aq) + 2eFe(s) Ag+ (aq) +e-Ag(s) 0.80 Cr3+ (aq) + Cr²+ (aq) Fe+(aq) + 3e...
Fe would corrode easily in a damp environment in which both water and oxygen are readily available. Identify the most l...
Fe would corrode easily in a damp environment in which both water and oxygen are readily available. Identify the most likely anodic and cathodic reactions, respectively, from the table below. What is the standard electrode potential difference? Standard Electrode Electrode Reaction Potential, V 3 + +1.420 Au 3eAu O2 + 4H + + 4e-_→ 2H2O Pt2ePt +1.229 +0.800 Increasingly inert (cathodic) +0.771 +0.401 O2 + 2H2O + 4e-_→ 4(OH-) Cu2eCu +0.340 2H+ + 2e 0.000 0.126 > H2 0.136 Ni2+...
A) Use tabulated electrode potentials to calculate ΔG∘ for the reaction. 2K(s)+2H2O(l)→H2(g)+2OH−(aq)+2K+(aq) B) (Refer to the...
A) Use tabulated electrode potentials to calculate ΔG∘ for the reaction. 2K(s)+2H2O(l)→H2(g)+2OH−(aq)+2K+(aq) B) (Refer to the following standard reduction half-cell potentials at 25∘C: VO2+(aq)+Ni2+(aq)2H+(aq)++2e−e−→ →Ni(s)VO2+(aq) +H2O(l)E∘=−0.23V E∘=0.99V) An electrochemical cell is based on these two half-reactions: Oxidation:Reduction:Ni(s)VO2+(aq,0.024M)+2H+(aq,1.4M)+e−→→Ni2+(aq,1.8M)+2e−VO2+(aq,1.8M)+H2O(l) Calculate the cell potential under these nonstandard concentrations. C) Standard reduction half-cell potentials at 25∘C Half-reaction E∘ (V ) Half-reaction E∘ (V ) Au3+(aq)+3e−→Au(s) 1.50 Fe2+(aq)+2e−→Fe(s) − 0.45 Ag+(aq)+e−→Ag(s) 0.80 Cr3+(aq)+e−→Cr2+(aq) − 0.50 Fe3+(aq)+3e−→Fe2+(aq) 0.77 Cr3+(aq)+3e−→Cr(s) − 0.73 Cu+(aq)+e−→Cu(s) 0.52 Zn2+(aq)+2e−→Zn(s) − 0.76...
materials question electrochemistry
table has associated voltages
compute the voltage at 25c of an electrochemical cell
consisting of pure copper immersed in 9x10^-2M solution of Cu^2+
ions and pure nickel in a 0.35 M solution of Ni^2+ ions.
half reactions are:
Cu-> Cu^2+ + 2e- @+0.345V electrode potential
Ni-> Ni^2+ + 2e- @ -2.250V
this is all the information I was given
We were unable to transcribe this imageWe were unable to transcribe this imageWe were unable to transcribe this...
- cellpotentials and standard reduction potential table.
-Determining the Nernst equation and finding the Faraday
constant.
If you can explain how to solve for each part please.
25°C Standard Reduction Potentials in Aqueous solution a 2.87 Reduction half-reaction 2F (a 1.77 2H2O 1.692 2e 2H (a Au (s 1.085 PbSO4 (s) 2H20. Au (ag) 2e 1.51 4H20 Mn 1.50 5e 8H (a Mno4 (a Au(S 1.36 3e 2Cl (aq 1.33 2e 2Cr3 (ag) 7H20 C12 6e- 1.229 14H 2H2O 1.08...
1. How do I read the half reaction table?
2. If im asked for the best reducing agent from Cu+, Ag+, F2, and
Fe3+, where do I look first in the table? before the arrow or after
the arrow?
3. Sometimes a value that has originally a positive (V) from the
table it will have the negative sign in a homework problem, and
viceversa, so the question is, how do I use the positive and
negative signs in respect to...
HQ18.28 Homework • Unanswered Some electrode combinations that the Phoenix spacecraft designers may have considered for use in their design are given in the table below. Assume the ambient Martian temperature is -67.5*C, 205.7 K. What electrode combination (assume 0.1 M solutions) would provide the 1.317 V required by the spacecraft electronics? Use Appendix 11 for your standard cell potentials. А Rh+ +e- Rh/Ni2+ + 2e + NI O B Rh+ + e + Rh/Cr3+ + 3e - Cr C...
5. How much faster would a reaction be if a catalyst is used that lowers the activation energy from 20.0 kJ/mol to 10.0 kJ/mol? Do the calculation at two temperatures: first at 25.0°C and then at 0.0°C. (20 points) (V) Helpful Stuff Thermodynamics: AG° = AH-TAS Nernst Equation: 6 = 6 - (RT/nF)InQ AG=RTIK At 25°C: 8 = 6 - (0.0591/n)logQ AGRT Ke=e AGⓇ =-nF8° Units/Constants: Volt: 1 V = 1 J/C Faraday: 1 F = 96,485 C/mole Arrhenius Equation:...
use tabulated standard electrode potential to calculate the
standard cell potential for the reaction occurring in an
electrochemical cell at 25 C. (The equation is balanced.)
3Ni^2+(aq)+2Cr(s)--->3Ni(s)2Cr^3+(aq)
Express your answer to two significant figures and include the
appropriate units.
em 26 E (V) -0.45 -0.50 -0.73 -0.76 -1.18 Standard reduction half-cell potentials at 25°C Half-reaction E° (V) Half-reaction Aul+ (aq) + 3e +Au(s) 1.50 Fe2+ (aq) + 2eFe(s) Ag+ (aq) +e-Ag(s) 0.80 Cr3+ (aq) + Cr²+ (aq) Fe+(aq) + 3e...
Fe would corrode easily in a damp environment in which both water and oxygen are readily available. Identify the most likely anodic and cathodic reactions, respectively, from the table below. What is the standard electrode potential difference? Standard Electrode Electrode Reaction Potential, V 3 + +1.420 Au 3eAu O2 + 4H + + 4e-_→ 2H2O Pt2ePt +1.229 +0.800 Increasingly inert (cathodic) +0.771 +0.401 O2 + 2H2O + 4e-_→ 4(OH-) Cu2eCu +0.340 2H+ + 2e 0.000 0.126 > H2 0.136 Ni2+...
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