Mark the incorrect statements.
Which of the following graphs is correct for a zero order reaction?
Which of the following graphs is correct for a first order reaction?
State a condition under which a bimolecular reaction is kinetically first order reaction.
Presence of one of the reactants in excess, as in such a condition, its concentration remains constant and rate of such reaction depends upon concentration of one reactant only and reaction is known as pseudo first order reaction e.g., acid catalysed hydrolysis of ethyl acetate.
$$\underset{\text { Ethyl acetate }}{\mathrm{CH}_3 \mathrm{COOC}_2 \mathrm{H}_5}+\mathrm{H}_2 \mathrm{O} \xrightarrow[\text { Acetic acid }]{\mathrm{H}^{+}} \mathrm{CH}_3 \mathrm{COOH}+\underset{\text { Ethyl alcohol }}{\mathrm{C}_2 \mathrm{H}_5 \mathrm{OH}}$$
This reaction is bimolecular but is found to be of first order as experimentally it is observed that rate of reaction depends upon the concentration of ethyl acetate not on water as it is present in excess.
Write the rate equation for the reaction $2 \mathrm{~A}+\mathrm{B} \longrightarrow \mathrm{C}$ if the order of the reaction is zero.
For reaction $2 A+B \longrightarrow C$ if the rate of reaction is zero then it can be represented as
$$\text { Rate }=k[A]^0[B]^0=k$$
i.e., rate of reaction is independent of concentration of $A$ and $B$.