$W = 4\, eV$
$KE_{max} = 6\, eV = KE_{initial}$
On applying accelerating potential of $7.6\,V$
$\Delta KE = charge × potential = 7.6\, eV$
$KE_f -KE_g = 7.6\, eV$
$KE_{final} = 7.6\, eV + 6\, eV = 13.6\, eV$
which is $KE$ of electron in $(n = 1)$ in hydrogen atom
$V = 2.188 \times 10^6\, m/s$
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$\begin{array}{*{20}{c}}
{\,\,\,\,\,\,\,\,\,\,\,C{H_3}}\\
{\,\,\,|\,\,}\\
{C{H_3} - C{H_2} - CH - C - N{H_2}}\\
{\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,||}\\
{\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,O\,\,\,}
\end{array}$ $\xrightarrow[\Delta ]{{B{r_2}/KOH}}\left( A \right)\xrightarrow{\begin{subarray}{l}
(1)\,\,C{H_3}I\,{\text{(excess)}} \\
(2)\,AgOH/\Delta \,
\end{subarray} }$ $(B)$
| List-I edox Reaction) | List-II(Type of RedoxReaction) | ||
| A | $\begin{array}{l} CH _{4(g)}+2 O _{2(g)} \xrightarrow{\Delta} CO _{2(g)}+ 2 H _2 O _{( l )}\end{array}$ | (I) | Disproportionation reaction |
| B | $\begin{array}{l}2 NaH _{( s )} \xrightarrow{\Delta} 2 Na _{( s )}+ H _{2(g)}\end{array}$ | (II) | Combination reaction |
| C | $\begin{array}{l} V _2 O _{5(s)}+5 Ca _{( s )} \xrightarrow{\Delta} 2 V_{( s )}+ 5 CaO _{( s )}\end{array}$ | (III) | Decomposition reaction |
| D | $\begin{array}{l}2 H _2 O _{2( aq )} \xrightarrow{\Delta} 2 H _2 O _{( l )} + O _{2(g)}\end{array}$ | (IV) | Displacement reaction |