Calculate E°cell for the reaction of nickel(II) ions with cadmium metal at 25°C. K = 1.17 x105 Ni2+(aq) + Cd(aq) ----- Cd2+(aq) + Ni(s)
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Calculate E°cell for the reaction of nickel(II) ions with cadmium metal at 25°C. K = 1.17...
17. Write the overall cell reaction for the following voltaic cell. Cd(s)|Cd2+(aq)||Ni2+ (aq)|Ni(s) 18. Calculate the standard cell potential of the following cell at 25°C. Cd(s) Cd2+ (aq)||Ni2+ (aq) Ni(s)
Calculate E°cell for the following reaction:2Fe2+(aq) + Cd2+(aq) ? 2Fe3+(aq) + Cd(s)A. -0.37 VB. 0.37 VC. -1.17 VD. 1.17 VE. none of these
What is the standard cell potential of a cell created using a cadmium electrode in 0.45 M Cd(NO3)2(aq) and a graphite electrode in an aqueous solution that is 0.45 M in both Fe2+ and Fe3+? 0.38 V 1.95 V 1.94 V 1.17 V 1.18 V What is the standard cell potential of a cell which utilizes the following reaction: Zn (s) + Ni2+ (aq) → Ni (s) + Zn2+ (aq) All solutions are 1.0 M and the reaction occurs at...
Anode E A Cathode B 7 С D Ni2+ + 2e -0.40 V Cd2+ + 2e -0.26 V Ni (s) Cd (s) Reduction Ni (8) Ereduction Cd (8) Ereduction Ni2+ (aq) Cd2+ (aq) Oxidation Salt Bridge Look at the voltaic cell diagram above and finish the following sentences using options given on the table above: i) Ais ii) B is metal on the left metal on the right solution on the left iii) Cis iv) Dis solution on the right...
Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25°C, given that [Ni2+] = 0.00100 M and [Au?+] = 0.781 M. Standard reduction potentials can be found in this table. 3 Ni(s) + 2 Au?+ (aq) =3 Ni2+ (aq) + 2 Au(s) E = V
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)...
(a) Compute the voltage at 25˚C of an electrochemical cell consisting of pure cadmium immersed in a 2 × 10-3 M solution of Cd2+ ions and pure iron in a 0.2 M solution of Fe2+ ions. (b)Determine the spontaneous electrochemical reaction for iron (reduced/oxidized) and cadmium (reduced/oxidized).
Nickel-cadmium (nicad) alkaline batteries are currently very popular because they maintain a constant potential and are rechargeable. The relevant half-cell reactions for such batteries are given in this table. Half-Reaction, Cd(OH)2(s) + 2e- -> Cd(s) + 2 OH- (aq) E(volts) = -0.809 NiOOH(s)+ H2O(l) + e- -> Ni(OH)2(s)+OH-(aq) E(volts) = +0.490 A) Write a balanced equation for the process that produces electricity in a nicad battery and specify the half- reaction that occurs at the anode. B) Calculate the potential expected...
For a voltaic cell based on the reaction below, what reaction happens at the anode? 2Ni3+(aq)+Cd(s)→2Ni2+(s)+Cd2+(aq) Ni3+(aq)+e-→Ni2+(aq) Ni2+(aq)→ Ni3+(aq)+e- Cd2+(aq)+2e-→Cd(s) Cd(s)→Cd2+(aq)+2e- A student measures the voltage across different metal electrodes placed in a voltaic cell. Using a copper cathode, the voltages when using a first a tin, then gold anode are positive and negative, respectively. The order of chemical reactivity of the solid metals must be Au>Cu>Sn Au=Sn Sn>Cu>Au Au=Sn>Cu
1) Given the reaction Cd(s)+Ni2+(aq)------>Cd2+(aq)+Ni(s) Calculate the equilibrium constant (K). Ecell of +0.350 V and at 25.0 celsius 2)If 75.0mL of 0.195 M Hbr is combined with 75.0mL of 195M Ca(OH)2 at 25.0 celsius calculate the pH of this solution