8.1. Aldehydes and ketones — Chemistry STD 12 Science — Question

$2B\xrightarrow{k}{B_2}$        [Slow]

${B_2} + A \to D$          [Fast]

The rate law expression, order with respect to $A$, order with respect to $'B'$ and overall order are respectively

($A$) a high activation energy usually implies a fast reaction.

($B$) rate constant increases with increase in temperature. This is due to a greater number of collisions whose energy exceeds the activation energy.

($C$) higher the magnitude of activation energy, stronger is the temperature dependence of the rate constant.

($D$) the pre-exponential factor is a measure of the rate at which collisions occur, irrespective of their energy.

Reason : $\overset{\centerdot \,\,\centerdot }{\mathop{N}}\,{{H}_{2}}$ is more electron donating than $\overset{\centerdot \,\centerdot \,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,}{\mathop{O{{C}_{2}}{{H}_{5}}}}\,$

$[Image]$

is fastest, then $Z$ is

$\begin{array}{*{20}{c}}
  {OH\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,} \\ 
  {|\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,} \\ 
  {C{H_3}CHC{H_2}C{H_2}N{H_2}} 
\end{array}$ $\xrightarrow[{triethyla\min e}]{{ethyl\,formate\,\left( {1\,equiv} \right)}}$