1.

2NO + H_(2) to N_(2)O + H_(2)O , The reaction , follows third orderkinetics. Write (a) ratelaw and (b) unitsof rateconstant. What happens to the rate if the volumeof vessel is reduceto one - halfat constnattemperature ?

Answer»

Solution :(a) Rate LAW is given as, rate `=[NO)^(2)[H_(2)]`
(b) Units of rate constant `=L^(2)" MOL"^(-2)s^(-1)`
It volume of the vessel is halved, concentration of each REACTANT is doubled.
The rate will be Rate `=k[2NO)^(2)[2H_(2)]=8k[NO)^(2)[H_(2)]`
Rate will be 8 times more than the ORIGINAL rate of the reaction.


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