Why can’t molecularity of any reaction be equal to zero ?
Why can’t molecularity of any reaction be equal to zero ?
Molecularity is the number of molecules taking part in an elementary step. For this we require at least a single molecule leading to the value of minimum molecularity of one.
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For a reaction $A+ B\to $ Products, the rate law is - Rate $=$ $k\,[A]\, [B]^{\frac {3}{2}}$ . Can the reaction be an elementary reaction ? Explain.
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For the non-stoichiometric reaction $2A + B \to C + D,$ the following kinetic data were obtained in three separate experiments, all at $298\,K$.
Initial Conc.
$(A)$
Initial Conc.
$(B)$
Initial rate of
formation of $C\,(mol\, L^-S^-)$
$0.1\,M$
$0.1\,M$
$1.2 \times 10^{-3}$
$0.1\,M$
$0.2\,M$
$1.2 \times 10^{-3}$
$0.2\,M$
$0.1\,M$
$2.4 \times 10^{-3}$
For the reaction the rate of formation of $C$ will be
For the non-stoichiometric reaction $2A + B \to C + D,$ the following kinetic data were obtained in three separate experiments, all at $298\,K$.
| Initial Conc. $(A)$ |
Initial Conc. $(B)$ |
Initial rate of |
| $0.1\,M$ | $0.1\,M$ | $1.2 \times 10^{-3}$ |
| $0.1\,M$ | $0.2\,M$ | $1.2 \times 10^{-3}$ |
| $0.2\,M$ | $0.1\,M$ | $2.4 \times 10^{-3}$ |
For the reaction the rate of formation of $C$ will be
Select the incorrect option :
Select the incorrect option :