Question
Complete the following reaction equations:
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This reaction takes place in two step as given below:
Step-I $\text{H}_2\text{O}_2+\text{I}^-\rightarrow\text{H}_2\text{O}_2+\text{IO}^-\text{ (slow)}$
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This reaction takes place in two step as given below:
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$(a)$ The rate of a reaction is given by rate $= k [N_2O_5].$ In this equation what does $k$ stand for?
$(b)$ Is it possible to determine or predict the rate law theoretically by merely looking at the equation?
→$(a)$ The rate of a reaction is given by rate $= k [N_2O_5].$ In this equation what does $k$ stand for?
$(b)$ Is it possible to determine or predict the rate law theoretically by merely looking at the equation?