## Chapter 14

## Q. 14.2.1

## Q. 14.2.1

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:

What is the average rate of disappearance of H_{2}O_{2} over the period from 0 min to 434 min?

t (min) | [H_{2}O_{2}] (mol/L) |

0 | 0.0912 |

434 | 0.0566 |

868 | 0.0351 |

13.2 | 0.0218 |

## Step-by-Step

## Verified Solution

**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 = -\frac{\Delta \left[H_{2}O_{2}\right] }{\Delta t}=-\frac{\left(0.0566\text{ M}-0.0912 \text{ M}\right) }{\left(434\text{ min}-0\text{ min}\right) } =7.97\times 10^{-5} M/min