SHE

Q. 8 L of $H_2$ and 6 L $C{l}_2$ are allowed to react to their maximum possible extent. Find out the final volume of reaction mixture. Suppose P and T remains constant throughout the course of reaction.

1. 2 L
2. None of these
3. 14 L
4. 7 L

Q. Calculate the cell potential of the following cell at ${25}^{\circ }\text{C}$.
$Ag\left(s\right)|A{g}^{+}(aq,0.001\text{M})||A{g}^{+}(aq,0.5\text{M})|Ag\left(s\right)$

1. $0.03\text{V}$
2. $0.159\text{V}$
3. $1.09\text{V}$
4. $0.52\text{V}$

Q.

Which of the following can be used to measure pH?

1. a glass electrode

2. concentration cell

3. a hydrogen electrode

4. all of these

Q. In the reaction:
$2Al\left(s\right)+6HCl\left(aq\right)\to 2A{l}^{3+}\left(aq\right)+6C{l}^{-}\left(aq\right)+3H_2\left(g\right)$ Calculate the volume of $H_2$ gas (L) produced at $STP$(atm) for every 3 mol of $HCl$ consumed.

1. $33.6\text{L}$
2. $44.8\text{L}$
3. $67.2\text{L}$
4. $22.4\text{L}$

Q. The value of $E_{reduction}$ of a hydrogen electrode at $pH=0$ and $298K$, $1atm$ is:

1. $0.59V$
2. $0V$
3. $-0.59V$
4. $-0.059V$

Q. Specific conductance of $0.1MNaCl$ solution is $1.01\times {10}^{-2}oh{m}^{-1}c{m}^{-1}$. Its molar conductance in $oh{m}^{-1}c{m}^{2}mo{l}^{-1}$ is :

1. $1.01\times {10}^2$
2. $1.01\times {10}^4$
3. $1.01$
4. $1.01\times {10}^3$

Q. What is the reaction that takes place at the standard hydrogen electrode if it's coupled with metal-metal ion electrode of zinc (zinc in zinc sulphate solution).

1. $Pt\to P{t}^{+}+e^{-}$
2. $P{t}^{+}+e^{-}\to Pt$
3. $H_2\to 2H^{+}+2e^{-}$
4. $2H^{+}+2e^{-}\to H_2$

Q. For $I_2+2e^{-}\to 2I^{-},\text{standard reduction potential}=+0.54\text{Volt}.$
For $2B{r}^{-}\to B{r}_2+2e^{-},\text{standard oxidation potential}=-1.09\text{Volt}.$
For $Fe\to F{e}^{2+}+2e^{-},\text{standard oxidation potential}=+0.44\text{Volt}.$
Out of the below given reactions, how many reactions are spontaneous in nature (predict from the above data) ?
$B{r}_2+2I^{-}\to 2B{r}^{-}+I_2$
$Fe+B{r}_2\to F{e}^{2+}+2B{r}^{-}$
$Fe+I_2\to F{e}^{2+}+2I^{-}$
$I_2+2B{r}^{-}\to 2I^{-}+B{r}_2$

Q. The standard hydrogen electrode has zero electrode potential because

1. Hydrogen is easiest to oxidize
2. The electrode potential is assumed to be 0 for the SHE
3. Hydrogen has only one electron
4. Hydrogen is lightest element

Q. Calculate the reduction potential for the following half cell at $25{}^{o}C$.

$Cu\left(s\right)|C{u}^{2+}(aq,0.2M);E_{Cu/C{u}^{2+}}^0=-0.34V$

Take :
[$lo{g}_{10}5=0.7$]

Q. The value of $E_{reduction}$ of a hydrogen electrode at $pH=0$ and $298K$, $1atm$ is:

1. $0.59V$
2. $0V$
3. $-0.59V$
4. $-0.059V$