For the decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C,
2 H $_{2}$ O $_{2}$ (aq) → 2 H $_{2}$ O(ℓ) + O $_{2}$ (g)
the following data have been obtained:

Question

For the decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C,
2 H[latex]_{2}[/latex]O[latex]_{2}[/latex](aq) → 2 H[latex]_{2}[/latex]O(ℓ) + O[latex]_{2}[/latex](g)
the following data have been obtained:

What is the average rate of disappearance of H[latex]_{2}[/latex]O[latex]_{2}[/latex] over the period from 0 min to 434 min?

Accepted Answer

You are asked to determine the average rate of disappearance of a reactant over a given period of time.
You are given the balanced chemical equation and data showing the reactant concentration as a function of time.
Average reaction rate is equal to the change in concentration over the change in time.

rate = [latex]-\frac{\Delta \left[H_{2}O_{2} ight] }{\Delta t}=-\frac{\left(0.0566 ext{ M}-0.0912 ext{ M} ight) }{\left(434 ext{ min}-0 ext{ min} ight) } =7.97 imes 10^{-5}[/latex] M/min

t (min)	[H $_{2}$ O $_{2}$ ] (mol/L)
0	0.0912
434	0.0566
868	0.0351
13.2	0.0218

Chapter 14

Q. 14.2.1

Q. 14.2.1

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