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Nernst Equation - Introduction

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Nernst equation [00:20:43]
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Series: Nernst Equation - Introduction
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Nernst equation
00:20:43  undefined
Electrochemistry part 11 (Nernst Equation)
00:11:30  undefined
Electrochemistry part 12 (Nernst Equation :- Derivation)
00:13:24  undefined

Related QuestionsVIEW ALL [17]

Write the Nernst equation and emf of the following cell at 298 K:

Mg(s) | Mg2+ (0.001 M) || Cu2+ (0.0001 M) | Cu(s)

Calculate emf of the following cell at 298 K:

\[\ce{Mg_{(s)} | Mg^{2+} (0.1 M) || Cu^{2+} (0.01) | Cu_{(s)}}\]

[Given \[\ce{E^{\circ}_{cell}}\] = +2.71 V, 1 F = 96500 C mol–1]

Write the Nernst equation and explain the terms involved.

For a general electrochemical reaction of the type:

\[\ce{{a}A + {b}B ⇔ {c}C + {d}D}\]

Nernst equation can be written as:

Write the Nernst equation and emf of the following cell at 298 K:

\[\ce{Sn_{(s)} | Sn^{2+} (0.050 M) || H^+ (0.020 M) | H2_{(g)} (1 bar) | Pt_{(s)}}\]

Calculate the e.m.f. of the following cell at 298 K:

Fe(s) | Fe2+ (0.001 M) | | H+ (0.01 M) | H2(g) (1 bar) | Pt(s)

Given that \[\ce{E^0_{cell}}\] = 0.44 V

[log 2 = 0.3010, log 3 = 0.4771, log 10 = 1]

Calculate ΔrG0 and log Kc for the following cell:

\[\ce{Ni(s) + 2Ag^+(aq) -> Ni^{2+}(aq) + 2Ag(s)}\]

Given that \[\ce{E^0_{cell}}\] = 1.05 V, 1F = 96,500 C mol–1.

Calculate the emf of the following cell at 298 K.

\[\ce{Cu/Cu^{2+}_{(0.025 M)}//Ag^+_{(0.005 M)}/Ag}\]

Given `"E"_("Cu"^(2+)//"Cu")^circ` = 0.34 V, `"E"_("Ag"^+//"Ag")^circ` = 0.80 V

1 Faraday = 96500 C mol -1

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