What is the -G- for the following reaction-Cuaq2- 2Ags - Cus - 2Agaq-Given-ECu2-Cu0- 0-34V-EAg-Ag-0 - -0-8 V

Point to remember: ⇒Δ ^0G= nFE^0_cell Given informations in question : ⇒ Reduction half cell Cu^2+(aq)+2e^ → Cu(s) ⇒ Oxidation half cell Ag(s)→ Ag^+(aq)+e^ S ...

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Standard XIII

Chemistry

Gibb's Free Energy

What is the ∆...

Question

What is the $Δ G^{\circ}$ for the following reaction?
$C u_{(a q)}^{2 +} + 2 A g_{(s)} \to C u_{(s)} + 2 A g_{(a q)}^{+}$
Given: $E_{C u^{2 +} / C u}^{0} = 0.34 V, E_{A g / A g^{+}}^{0} = - 0.8 V$

-44.5 kJ

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44.5 kJ

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-89 kJ

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89 kJ

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Solution

The correct option is D 89 kJ
Point to remember:
$\Rightarrow Δ^{0} G = - n F E_{c e l l}^{0}$
Given informations in question :
$\Rightarrow R e d u c t i o n h a l f c e l l$
$C u^{2 +} (a q) + 2 e^{-} \to C u (s)$
$\Rightarrow O x i d a t i o n h a l f c e l l$
$A g (s) \to A g^{+} (a q) + e^{-}$
So from these half reactions we find that $n = 2$
To calculate $Δ G$ we need to find $E_{c e l l}^{o}$
$E_{c e l l}^{o}$ = $E_{c a t h o d e}^{o} - E_{a n o d e}^{o}$
$E_{c e l l}^{o}$ = $E_{C u^{2 +} / C u}^{o} - E_{A g^{+} / A g}^{o}$
$E_{c e l l}^{o} = 0.34 - 0.8 = - 0.46$
On substituting
$Δ^{0} G = - 2 \times 96500 \times (- 0.46) = 88780 \approx 89 k J$

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Similar questions

Q. What is the

Δ G^{\circ}

for the following reaction?

C u_{(a q)}^{2 +} + 2 A g_{(s)} \to C u_{(s)} + 2 A g_{(a q)}^{+}

Given:

E_{C u^{2 +} / C u}^{0} = 0.34 V, E_{A g / A g^{+}}^{0} = - 0.8 V

Q. Calculate the equailibrium constant for the reaction:

{C u}_{(s)} + {2 A g}_{(a q)}^{+} ⟶ {C u}_{(a q)}^{2 +} + {2 A g}_{(s)}

Given that :

E_{A g^{+} / A g}^{0} = 0.80 V, E_{C u^{2 +} / C u}^{0} = 0.34 V .

Q. E.M.F. of the cell reaction,

2 A g^{+} + C u ⟶ 2 A g + C u^{2 +}

is 0.46 V. If

E_{{C u}^{2 +} / C u}

is 0.34 V,

E_{{A g}^{+} / A g}

is:

Q. What is the

Δ G^{\circ}

for the following reaction?

C u_{(a q)}^{2 +} + 2 A g_{(s)} \to C u_{(s)} + 2 A g_{(a q)}^{+}

Given:

E_{C u^{2 +} / C u}^{0} = 0.34 V, E_{A g / A g^{+}}^{0} = - 0.8 V

Consider the reaction

Cu (s) + 2Ag⁺ (aq) → Cu²⁺ (aq) + 2Ag (s)

Which of the following statement is true for this cell reaction?

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What is the ΔG∘ for the following reaction? Cu2+(aq)+2Ag(s)→Cu(s)+2Ag+(aq) Given:E0Cu2+/Cu=0.34V,E0Ag/Ag+=−0.8V

What is the $Δ G^{\circ}$ for the following reaction?
$C u_{(a q)}^{2 +} + 2 A g_{(s)} \to C u_{(s)} + 2 A g_{(a q)}^{+}$
Given: $E_{C u^{2 +} / C u}^{0} = 0.34 V, E_{A g / A g^{+}}^{0} = - 0.8 V$