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Consider the decomposition of hydrogen peroxide reaction. If the rate of decomposition of hydrogen peroxide at a particular temperature is determined to be 0.098 mol/(L·s), what are the rates of reaction with respect to the products of the decomposition reaction?

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Answer:

0.049 mol/L.s

Explanation:

The decomposition of hydrogen peroxide is:

[tex]H_2O_2 \to H_2O + \dfrac{1}{2}O_2[/tex]

[tex]Rate = -\dfrac{\Delta [H_2O_2]}{\Delta t}= \dfrac{\Delta [H_2O_2]}{\Delta t}= \dfrac{ 2 \Delta [H_2O_2]}{\Delta t}[/tex]

The rate of decomposition reaction = the rate of formation of [tex]H_2O[/tex] = 0.098 mol/L.s

∴

Rate of formation of [tex]O_2[/tex] [tex]= \dfrac{ rate \ of \ reaction }{2}[/tex]

[tex]= \dfrac{ 0.098 }{2}[/tex]

= 0.049 mol/L.s

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