Compare the rate of catalytic hydrogenation u | vedclass

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(A) The rate of catalytic hydrogenation depends on the accessibility of the double bond to the catalyst surface. In compound $(a)$,the bulky $-CH_3$ g

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$a > b$

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(A) The rate of catalytic hydrogenation depends on the accessibility of the double bond to the catalyst surface. In compound $(a)$,the bulky $-CH_3$ group is oriented away from the double bond,resulting in less steric hindrance for the approach of $H_2$ on the catalyst surface. In compound $(b)$,the $-CH_3$ group is oriented towards the double bond,creating significant steric hindrance. Therefore,the rate of reaction for $(a)$ is greater than that for $(b)$,i.e.,$a > b$.

Reaction	Nature of reaction
$A. RBr \xrightarrow{Na}$	$1. \text{Partial reduction}$
$B. RCOO^-Na^+ \xrightarrow{NaOH/CaO, \Delta}$	$2. \text{Electrophilic addition}$
$C. R-C \equiv C-R' \xrightarrow{\text{Lindlar's catalyst } (H_2)}$	$3. \text{Wurtz reaction}$
$D. H_2C=CH_2 \xrightarrow{Br_2/CCl_4}$	$4. \text{Decarboxylation}$
	$5. \text{Decarboxylative dimerisation}$

Compare the rate of catalytic hydrogenation using $H_2 / Pt$ for the following compounds $(a)$ and $(b)$:

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