Write the Nernst equation and emf of the following cell at 298 K: \\ce{Pt_{(s)} | Br^- (0.010 M) | Br2_{(l)} || H^+ (0.030 M) | H2_{(g)} (1 bar) | Pt_{(s)}}\ - Chemistry

प्रश्न

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

$Pt_{(s)} | Br^{-} (0.010 M) | Br_{2}_{(l)} | | H^{+} (0.030 M) | H_{2}_{(g)} (1 bar) | Pt_{(s)}$

संख्यात्मक

उत्तर

The cell reaction is as follows:

$2 Br^{-} (0.010 M) + 2 H^{+} (0.030 M) ⟶ Br_{2}_{(l)} + H_{2} (1 bar)$

Hence, n = 2,

According to the Nernst equation for the cell, the emf is given below:

`"E"_"cell" = ("E"_("H"^+//1/2"H"_2)^Θ - "E"_(1/2"Br"_2//"Br"^-)^Θ) - 0.059/2 log_10 ("pH"_2)/(["Br"^-]^2["H"^+]^2)`

= `[0 - (+ 1.08)] - 0.059/2 log_10 1/((0.010)^2 (0.030)^2)`

= `-1.08 - 0.059/2 log_10 (1.11 xx 10^7)`

= −1.08 − 0.208

= −1.288 V

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Nernst Equation - Introduction

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Nernst Equation - Introduction

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Write the Nernst equation and emf of the following cell at 298 K: \ce{Pt_{(s)} | Br^- (0.010 M) | Br2_{(l)} || H^+ (0.030 M) | H2_{(g)} (1 bar) | Pt_{(s)}}\ - Chemistry

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Write the Nernst equation and emf of the following cell at 298 K: \ce{Pt_{(s)} | Br^- (0.010 M) | Br2_{(l)} || H^+ (0.030 M) | H2_{(g)} (1 bar) | Pt_{(s)}}\ - Chemistry

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