For the concentration cell, M|M+ (aq, 0.01 mol/dm3)| |M+ (aq), 0.1 mol/dm3|M the EMF (E) of the cell at a temperature (T) equals
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Engineering Chemistry · all questionsElectrochemistry
Electrochemistry
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The activity of water at 11 bar and 298 K is
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Given that E°(Fe3+, Fe) = -0.4 V and E°(Fe2+, Fe) = -0.44 V, the value of E°(Fe3+, Fe2+) is
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According to the Debye-Huckel limiting law, if the concentration of a dilute aqueous solution of KCl is increased 4-fold, the value of In γz (γz is the molar mean ionic activity coefficient) will
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Given the standard potential for the following half-cell reaction at 298 K,
Cu+(aq) + e- → Cu(s); E° = 0.52 V
Cu2+(aq) + e- → Cu+(aq); E° = 0.16 V
Calculate the ΔG° (kJ) for the reaction, [2Cu+(aq) → Cu(s) + Cu2+]
Cu+(aq) + e- → Cu(s); E° = 0.52 V
Cu2+(aq) + e- → Cu+(aq); E° = 0.16 V
Calculate the ΔG° (kJ) for the reaction, [2Cu+(aq) → Cu(s) + Cu2+]
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A student recorded a polarogram of 2.0 mM Cd2+ solution and forget to add KCl solution. What type of error do you expect in his results?
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For a 2 molal aqueous NaCl solution, the mean ionic activity coefficient and the Debye-Huckel Limiting Law constant (A) are related as
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The standard reduction potentials at 298 K for single electrodes are given below.
From this we can infer that
| Electrode | Electrode potential (volt) |
| Mg2+ /Mg | -2.34 |
| Zn2+ /Zn | -0.76 |
| Fe2+ /Fe | -0.44 |
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For the reaction, Hg2Cl2(s) + H2(g) → 2Hg(liq) + 2HCl(aq), the correct representation of the cell and the thermodynamic properties ΔG, ΔH and ΔS at 298 K respectively, are (Given: E298 = 0.2684 V and temperature coefficient = 3 × 10-4 VK-1)
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The Nernst equation for the reaction, A2+ + 2e- → B, in terms of the free energy change is
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