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Byju's Answer

Standard XII

Chemistry

Electrochemical Series

The electrode...

Question

The electrode oxidation potential of electrode $M (s) \to M^{n +} (a q .) (2 M) + n e^{-}$ at 298K is $E_{1}$ . When temperature (in $C^{\circ}$ ) is doubled and concentration is made half, then the electrode potential becomes $E_{2}$ . Which of the following represent the correct relationship between $E_{1}$ and $E_{2}$ ?

E_{1} > E_{2}

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E_{1} < E_{2}

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E_{1} = E_{2}

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Can’t be predicted

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Solution

The correct option is B $E_{1} < E_{2}$
Use Nernst equation,

$E_{c e l l} = E_{c e l l}^{0} - \frac{2.303 R T}{n F} l o g [M^{n +}]$

$E_{1} = E^{0} - \frac{2.303. R T}{n F} l o g [2]$

$E_{2} = E^{0} - \frac{2.303. R (2 T)}{n F} l o g [1]$

$E_{2} = E^{0}$

$S i n c e l o g (1) = 0$

$E_{1} - E_{2} = - \frac{2.303. R T}{n F} l o g [2]$

$E_{1} = E_{2} - \frac{2.303. R T}{n F} l o g [2]$

Therefore $E_{2} > E_{1}$

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Similar questions

Q. The electrode oxidation potential of electrode

M (s) \to M^{n +} (a q .) (2 M) + n e^{-}

at 298K is

E_{1}

. When temperature (in

C^{\circ}

) is doubled and concentration is made half, then the electrode potential becomes

E_{2}

. Which of the following represent the correct relationship between

E_{1}

and

E_{2}

Q. The electrode potential of electrode at 298 kelvin is even when the temperature is doubled and concentration is made half then the electrode potential becomes E2 which of the following represent the correct correct relationship between E1 and E2

Q. A hydrogen electrode placed in a solution containing sodium acetate and acetic acid in the concentration ratios of

x : y

and

y : x

has electrode potential values

E_{1}

and

E_{2}

volts, respectively, at

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. The

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value of acetic acid is:

Q. A hydrogen electrode is placed in a buffer solution of acetic acid and sodium acetate in the ratio

y : x

and

x : y

has electrode potential values

E_{1}

and

E_{2}

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p K_{a}

value for acetic acid is__________.
(

E_{1}

and

E_{2}

are oxidation potentials).

A hydrogen electrode placed in a buffer solution of $C H_{3} C O O N a$ and $C H_{3} C O O H$ in the ratios $x : y$ and $y : x$ has electrode potential values $E_{1}$ volts and $E_{2}$ volts respectively at 25 $^{0}$ C . The $p K_{a}$ value of acetic acid is :

[ $E_{1}$ and $E_{2}$ are oxidation potentials]

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The electrode oxidation potential of electrode M(s)→Mn+(aq.)(2M)+ne− at 298K is E1. When temperature (in C∘) is doubled and concentration is made half, then the electrode potential becomes E2. Which of the following represent the correct relationship between E1 and E2?

The correct option is B E1<E2Use Nernst equation, Ecell=E0cell−2.303RTnFlog[Mn+] E1 = E0 −2.303.RTnFlog[2] E2 = E0 −2.303.R(2T)nFlog[1] E2 = E0 Since log(1)= 0 E1 −E2 = −2.303.RTnFlog[2] E1 = E2 −2.303.RTnFlog[2] Therefore E2 >E1