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What would happen to the rate of a reaction with rate law rate kNO2H2 if the concentration of NO were halved?
In the given rate law, the rate of the reaction is dependent on the concentration of NO and possibly other reactants. If the concentration of NO is halved, the rate of the reaction would decrease proportionally, assuming that NO is a reactant in the rate law. Specifically, if the rate law is of the form rate = k[NO]^n[other species], the rate would be affected by the new concentration of NO, resulting in a reduced reaction rate. The exact impact on the rate would depend on the order of the reaction with respect to NO.
What would happen to the rate of a reaction with rate law kNO2H2 if the concentration of NO were doubled?
The rate would be four times larger
What would happen to the rate of a reaction with rate law rate kno2h2 if the no were doubled?
the rate would be four times larger. apex
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