Advertisements
Advertisements
प्रश्न
Calculate the emf of the following cell at 298 K:
Fe(s) | Fe2+ (0.01 M) | | H+ (1 M) | H2(g) (1 bar) Pt(s)
Given \[\ce{E^0_{cell}}\] = 0.44 V.
Advertisements
उत्तर
Fe(s) | Fe2+ (0.01 M) | | H+ (1 M) | H2(g) (1 bar) Pt(s)
\[\ce{E^0_{cell}}\] = 0.44 V
Reaction at anode: \[\ce{Fe -> Fe^{2+} + 2e^-}\]
Reaction at cathode: \[\ce{2H^+ + 2e^- -> H2}\]
Overall: \[\ce{Fe + 2H^+ -> Fe^{2+} + H2}\]
According to the Nernst equation,
E = `"E"_"cell"^0 - 0.0591/"n" log (["Fe"^(2+)])/(["H"^+]^2)`
As n = 2
E = `0.44 - 0.0591/2 log 0.01/1`
= `0.44 - 0.0591/2 (-2 log 10)`
= `0.44 + 2 xx 0.0591/2`
= 0.4991 V
APPEARS IN
संबंधित प्रश्न
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)
Write the Nernst equation and explain the terms involved.
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]
Complete the following statement by selecting the correct alternative from the choices given:
For a spontaneous reaction ΔG° and E° cell will be respectively:
For a general electrochemical reaction of the type:
\[\ce{{a}A + {b}B ⇔ {c}C + {d}D}\]
Nernst equation can be written as:
What is the pH of HCl solution when the hydrogen gas electrode shows a potential of −0.59 V at standard temperature and pressure?
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
Calculate the value of \[\ce{E^\circ}\]cell, E cell and ΔG that can be obtained from the following cell at 298 K.
\[\ce{Al/Al^3+ _{(0.01 M)} // Sn^{2+} _{(0.015 M)}/Sn}\]
Given: \[\ce{E^\circ Al^3+/Al = -1.66 V; E^\circ\phantom{.}Sn^2+/Sn = -0.14 V}\]
Write the Nernst equation and emf of the following cell at 298 K:
\[\ce{Sn_{(s)} | Sn^{2+} (0.050 M) || H^+ (0.020 M) | H2_{(g)} (1 bar) | Pt_{(s)}}\]
Write the Nernst equation and emf of the following cell at 298 K:
Pt(s) | Br− (0.010 M) | Br2(l) || H+ (0.030 M) | H2(g) (1 bar) | Pt(s)
