Calculate the cell EMF in mV for - Pt - H2 1atm - HCl 0-01 M - AgCls - Ags at 298 Kif - Gto values are at 25 oC - 109-56 kJmol for AgCls and - 130-79 kJmol for H - - Cl - aq

The correct option is A 456 mV (H_2 + 2 AgCl #160; #160; → 2Ag + 2 H^+ + 2Cl^ Δ G_cell #160;reaction^0 = 2 ( 130.79) 2 ( 109.56) = 4 ...

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Byju's Answer

Standard XII

Chemistry

Equilibrium Constant from Nernst Equation

Calculate the...

Question

Calculate the cell EMF in mV for :
$P t | H_{2} (1 a t m) | H C l (0.01 M) | A g C l (s) | A g (s) a t 298 K$
if $Δ G_{t}^{o}$ values are at 25 $^{o}$ C
$- 109.56 \frac{k J}{m o l}$ for AgCl(s) and
$- 130.79 \frac{k J}{m o l}$ for (H $^{+}$ + Cl $^{-}$ ) (aq)

456 m V

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654 m V

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546 m V

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None of these

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Solution

The correct option is A $456 m V$
$(H_{2} + 2 A g C l \to 2 A g + 2 H^{+} + 2 C l^{-}$
$Δ G_{c e l l r e a c t i o n}^{0} = 2 (- 130.79) - 2 (- 109.56) = - 42.46 k J / m o l e = - 2 f \times E_{c e l l}^{0}$
$∴ E_{c e l l}^{0} = \frac{- 42460}{- 2 \times 96500} = + 0.220 V$
Now, $E_{c e l l} = + 0.220 + \frac{0.059}{2} l o g \frac{1}{(0.01)^{4}} = 0.456 V = 456 m V$

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Similar questions

Q. For the reaction

A g^{+} (a q) + C l^{-} (a q) ⇌ A g C l (s)

; the

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and

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are + 77, -129 and -109 kJ mol

^{- 1}

. Write the cell representation of above reaction and calculate

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Q. Calculate the EMF of the cell at 298 K.

P t | H_{2} (1 a t m) | N a O H (x M) | | N a C l (x M) | A g C l (s) | A g

E_{C l^{-} / A g C l / A g}^{0} = 0.222 V

Δ G^{o}

of the cell reaction

A g C l (s) + 1 / 2 H_{2} (g) \to A g (s) + H^{+} (a q .) + {C l}^{-} (a q)

- 21.52 k J

Calculate the EMF for the cell reaction:

2 A g C l (c) + H_{2} (g) \to A g (s) + 2 H^{+} (a q .) + 2 {C l}^{-} (a q .)

Q. Consider the cell

A g (s) | A g B r (x) | B r^{-} (a q) | | C l^{-} (a q) | A g C l (s) | A g (s)

at 25

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Q. The EMF of the cell :

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is 0.27 and 0.26 V at

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Calculate the cell EMF in mV for :Pt|H2(1atm)|HCl(0.01M)|AgCl(s)|Ag(s)at298Kif ΔGot values are at 25oC−109.56kJmol for AgCl(s) and−130.79kJmol for (H+ + Cl−) (aq)

The correct option is A 456mV(H2+2AgCl→2Ag+2H++2Cl−ΔG0cell reaction=2(−130.79)−2(−109.56)=−42.46kJ/mole=−2f×E0cell∴E0cell=−42460−2×96500=+0.220VNow, Ecell=+0.220+0.0592log1(0.01)4=0.456V=456mV

Calculate the cell EMF in mV for :
$P t | H_{2} (1 a t m) | H C l (0.01 M) | A g C l (s) | A g (s) a t 298 K$
if $Δ G_{t}^{o}$ values are at 25 $^{o}$ C
$- 109.56 \frac{k J}{m o l}$ for AgCl(s) and
$- 130.79 \frac{k J}{m o l}$ for (H $^{+}$ + Cl $^{-}$ ) (aq)