275790 $250 \mathrm{~mL}$ of a waste solution obtained from the workshop of a goldsmith contains $0.1 \mathrm{M} \mathrm{AgNO}_{3}$ and $0.1 \mathrm{M} A u C l$. The solution was electrolysed at $2 \mathrm{~V}$ by passing a current of 1 A for 15 minutes. The metal/metals electrodeposited will be
$\left(\mathrm{E}_{\mathrm{Ag}^{+} / \mathrm{Ag}}^{\mathbf{0}}=\mathbf{0 . 8 0} \mathrm{V}, \mathrm{E}_{\mathrm{Au}^{+} / \mathrm{Au}}^{0}=1.69\right)$

275791 Given $\mathrm{E}_{\mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}}^{0}=+0.76 \mathrm{~V}$ and $\mathrm{E}_{\mathrm{I}_{2} / \mathrm{I}^{-}}^{0}=+0.55 \mathrm{~V}$.
The equilibrium constant for the reaction taking place in galvanic cell consisting of above two electrodes is
$\left[\frac{2.303 \mathrm{RT}}{\mathrm{F}}=\mathbf{0 . 0 6}\right]$

275793 Which of the following statements is correct for the cell $\mathbf{Z n}\left \vert\mathbf{Z n}^{+2} \ \vert \mathbf{C u}^{+2}\right \vert \mathbf{C u}$ ?

275794 Which one of the following has a potential more than zero?

275796 For a cell involving one electron, $E_{\text {cell }}^{0}=0.59 \mathrm{~V}$ at $298 \mathrm{~K}$, the equilibrium constant for cell reaction is [Given that $\frac{2.303 R T}{F}=\mathbf{F} .059 \mathrm{~V}$ at $\mathbf{T}=\mathbf{2 9 8} \mathrm{K}]$

275790 $250 \mathrm{~mL}$ of a waste solution obtained from the workshop of a goldsmith contains $0.1 \mathrm{M} \mathrm{AgNO}_{3}$ and $0.1 \mathrm{M} A u C l$. The solution was electrolysed at $2 \mathrm{~V}$ by passing a current of 1 A for 15 minutes. The metal/metals electrodeposited will be
$\left(\mathrm{E}_{\mathrm{Ag}^{+} / \mathrm{Ag}}^{\mathbf{0}}=\mathbf{0 . 8 0} \mathrm{V}, \mathrm{E}_{\mathrm{Au}^{+} / \mathrm{Au}}^{0}=1.69\right)$

275791 Given $\mathrm{E}_{\mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}}^{0}=+0.76 \mathrm{~V}$ and $\mathrm{E}_{\mathrm{I}_{2} / \mathrm{I}^{-}}^{0}=+0.55 \mathrm{~V}$.
The equilibrium constant for the reaction taking place in galvanic cell consisting of above two electrodes is
$\left[\frac{2.303 \mathrm{RT}}{\mathrm{F}}=\mathbf{0 . 0 6}\right]$

275793 Which of the following statements is correct for the cell $\mathbf{Z n}\left \vert\mathbf{Z n}^{+2} \ \vert \mathbf{C u}^{+2}\right \vert \mathbf{C u}$ ?

275794 Which one of the following has a potential more than zero?

275796 For a cell involving one electron, $E_{\text {cell }}^{0}=0.59 \mathrm{~V}$ at $298 \mathrm{~K}$, the equilibrium constant for cell reaction is [Given that $\frac{2.303 R T}{F}=\mathbf{F} .059 \mathrm{~V}$ at $\mathbf{T}=\mathbf{2 9 8} \mathrm{K}]$

275790 $250 \mathrm{~mL}$ of a waste solution obtained from the workshop of a goldsmith contains $0.1 \mathrm{M} \mathrm{AgNO}_{3}$ and $0.1 \mathrm{M} A u C l$. The solution was electrolysed at $2 \mathrm{~V}$ by passing a current of 1 A for 15 minutes. The metal/metals electrodeposited will be
$\left(\mathrm{E}_{\mathrm{Ag}^{+} / \mathrm{Ag}}^{\mathbf{0}}=\mathbf{0 . 8 0} \mathrm{V}, \mathrm{E}_{\mathrm{Au}^{+} / \mathrm{Au}}^{0}=1.69\right)$

275791 Given $\mathrm{E}_{\mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}}^{0}=+0.76 \mathrm{~V}$ and $\mathrm{E}_{\mathrm{I}_{2} / \mathrm{I}^{-}}^{0}=+0.55 \mathrm{~V}$.
The equilibrium constant for the reaction taking place in galvanic cell consisting of above two electrodes is
$\left[\frac{2.303 \mathrm{RT}}{\mathrm{F}}=\mathbf{0 . 0 6}\right]$

275793 Which of the following statements is correct for the cell $\mathbf{Z n}\left \vert\mathbf{Z n}^{+2} \ \vert \mathbf{C u}^{+2}\right \vert \mathbf{C u}$ ?

275794 Which one of the following has a potential more than zero?

275796 For a cell involving one electron, $E_{\text {cell }}^{0}=0.59 \mathrm{~V}$ at $298 \mathrm{~K}$, the equilibrium constant for cell reaction is [Given that $\frac{2.303 R T}{F}=\mathbf{F} .059 \mathrm{~V}$ at $\mathbf{T}=\mathbf{2 9 8} \mathrm{K}]$

275790 $250 \mathrm{~mL}$ of a waste solution obtained from the workshop of a goldsmith contains $0.1 \mathrm{M} \mathrm{AgNO}_{3}$ and $0.1 \mathrm{M} A u C l$. The solution was electrolysed at $2 \mathrm{~V}$ by passing a current of 1 A for 15 minutes. The metal/metals electrodeposited will be
$\left(\mathrm{E}_{\mathrm{Ag}^{+} / \mathrm{Ag}}^{\mathbf{0}}=\mathbf{0 . 8 0} \mathrm{V}, \mathrm{E}_{\mathrm{Au}^{+} / \mathrm{Au}}^{0}=1.69\right)$

275791 Given $\mathrm{E}_{\mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}}^{0}=+0.76 \mathrm{~V}$ and $\mathrm{E}_{\mathrm{I}_{2} / \mathrm{I}^{-}}^{0}=+0.55 \mathrm{~V}$.
The equilibrium constant for the reaction taking place in galvanic cell consisting of above two electrodes is
$\left[\frac{2.303 \mathrm{RT}}{\mathrm{F}}=\mathbf{0 . 0 6}\right]$

275793 Which of the following statements is correct for the cell $\mathbf{Z n}\left \vert\mathbf{Z n}^{+2} \ \vert \mathbf{C u}^{+2}\right \vert \mathbf{C u}$ ?

275794 Which one of the following has a potential more than zero?

275796 For a cell involving one electron, $E_{\text {cell }}^{0}=0.59 \mathrm{~V}$ at $298 \mathrm{~K}$, the equilibrium constant for cell reaction is [Given that $\frac{2.303 R T}{F}=\mathbf{F} .059 \mathrm{~V}$ at $\mathbf{T}=\mathbf{2 9 8} \mathrm{K}]$

275790 $250 \mathrm{~mL}$ of a waste solution obtained from the workshop of a goldsmith contains $0.1 \mathrm{M} \mathrm{AgNO}_{3}$ and $0.1 \mathrm{M} A u C l$. The solution was electrolysed at $2 \mathrm{~V}$ by passing a current of 1 A for 15 minutes. The metal/metals electrodeposited will be
$\left(\mathrm{E}_{\mathrm{Ag}^{+} / \mathrm{Ag}}^{\mathbf{0}}=\mathbf{0 . 8 0} \mathrm{V}, \mathrm{E}_{\mathrm{Au}^{+} / \mathrm{Au}}^{0}=1.69\right)$

275791 Given $\mathrm{E}_{\mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}}^{0}=+0.76 \mathrm{~V}$ and $\mathrm{E}_{\mathrm{I}_{2} / \mathrm{I}^{-}}^{0}=+0.55 \mathrm{~V}$.
The equilibrium constant for the reaction taking place in galvanic cell consisting of above two electrodes is
$\left[\frac{2.303 \mathrm{RT}}{\mathrm{F}}=\mathbf{0 . 0 6}\right]$

275793 Which of the following statements is correct for the cell $\mathbf{Z n}\left \vert\mathbf{Z n}^{+2} \ \vert \mathbf{C u}^{+2}\right \vert \mathbf{C u}$ ?

275794 Which one of the following has a potential more than zero?

275796 For a cell involving one electron, $E_{\text {cell }}^{0}=0.59 \mathrm{~V}$ at $298 \mathrm{~K}$, the equilibrium constant for cell reaction is [Given that $\frac{2.303 R T}{F}=\mathbf{F} .059 \mathrm{~V}$ at $\mathbf{T}=\mathbf{2 9 8} \mathrm{K}]$