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A photochemical reaction between H_(2(g)) and Cl_(2(g)) is a zero order reaction. Explain.

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Solution :Consider PHOTOCHEMICAL reaction between `H_(2)` and `Cl_(2)` gases.
`H_(2(g))+Cl_(2(g))("Diffused")/("Sunlight")2HCl_((g))`
In this the rate of the reaction remains constant throughout the progress of the reaction, even if the concentration of the reactants decreases with time, until the reactant has reacted entirely.
Hence, by the rate LAW,
`R=k[H_(2)]^(0)[Cl_(2)]^(0)=k"(constant)"`.
Hence the above reaction is a zero order reaction.


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