Electrochemistr...

Find the potential of a half-cell having reaction, $Ag_{2}S+2e\rightarrow2Ag+S^{2-}$ in a solution buffered
$pH=3$ and which is also saturated with $0.1\ M\ H_{2}S$. For $H_{2}S:\ K_{1}=10^{-8}$ and $K_{2}=2\times 10^{-13},\ K_{sp}(Ag_{2}S)=2\times 10^{-48},\ E_{Ag,ag}^{o}=0.8$

Which of the following represent first law of Faraday?

In $Zn|Zn^{+2}|| Ag^+|Ag$, how will cell potential be affected if KI is added to $Ag^{+}$ half cell?

A : Electrochemical cell is based on redox reaction.
R : Electrochemical cell converts electrical energy into chemical energy.

Which of the following substance has the lowest electric resistivity at room temperature?

The no. of electrons involved in the electro deposition of 63.5 g. of Cu from aq. $CuSO_4$ is :

In the electrolysis of aqueous $NaCl$, what volume of $Cl_2(g)$ is produced in the time that it takes to liberate $5.0$ liter of $H_2(g) ?$ Assume that both gases are measured at STP.

How many faradays of charge is transferred to produce 11.2 L of $H_2$ at STP in the reaction, in the reaction, $NaH +H_2O \rightarrow NaOH +H_ 2 \uparrow$ ?

2 ml ethanoic acid was taken in test tubes - A, B and C. 2 ml, 4 ml and 8 ml of water was added to the test tubes A, B and C respectively. Which test tube will show clear solution?

Deduce from the following ${E^ \circ }$ value of half cells, What combination of half cells would result in cell with the largest potential? 
i) ${A^{3 - }} \to {A^2} + {e^ - };{\rm{ }}{{\rm{E}}^ \circ } = 1.5V$
ii) ${B^{2 + }} + {e^ - } \to {B^ + };{\rm{ }}{{\rm{E}}^ \circ } =  - 2.1V$
iii) ${C^{2 + }} + {e^ - } \to  + {C^ + };{\rm{ }}{{\rm{E}}^ \circ } =  + 0.5V$
iv) $D \to {D^{2 + }} + 2{e^ - };{\rm{ }}{{\rm{E}}^ \circ } =  - 1.5V$