Theories Of Reaction Rates

To find the rate of disappearance of , we need to relate the changes in concentration of to using the stoichiometry of the reaction:

The reaction is:

Given:

• The concentration of increases by mol L in 10 seconds.

Calculation:

1. Rate of formation of :
   
2. From the balanced equation, 4 moles of are produced for every 2 moles of consumed. Therefore, the rate of disappearance of is half the rate of formation of :
   

Conclusion:

The rate of disappearance of is \( 2.5 \times 10^{-4} \, \text{mol L}^{-1} \text{s}^{-1}