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which of the following affects the rate of constant of a reaction?

The temperature of the system


What would happen to the rate of a reaction with rate law rate k NO H2 if the concentrations 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 concentration of NO were double?

The rate would quadruple (increase by a factor of 4). This is because the rate depends on the SQUARE of the concentration of NO.


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 th rate of a reaction with rate law rate k NO2H2 of concentration of NO were halved?

If the concentration of NO is halved in a reaction with the rate law ( \text{rate} = k[\text{NO}]^2[\text{H}_2] ), the rate of the reaction would decrease. Specifically, since the concentration of NO is squared in the rate law, halving it would result in a decrease in the rate by a factor of ( (0.5)^2 = 0.25 ). Therefore, the new rate would be one-quarter of the original rate.

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