Chapter 5, Problem 5.106PAE

Interpretation Introduction

Interpretation:

The best way to generate small amounts of oxygen gas in a laboratory setting is by the decomposition of potassium permanganate.

${\text{2KMnO}}_{\text{4}}\text{(s) }\to {\text{K}}_{\text{2}}{\text{MnO}}_{\text{4}}{\text{(s) + MnO}}_{\text{2}}{\text{(s) + O}}_{\text{2}}\text{(g)}$

Suppose that you are carrying out an experiment for which you need exactly 2.00L of oxygen. Describe how you would determine the mass of potassium permanganate needed to obtain this amount. What would you have to measure in your experiment in addition to this mass?

Concept introduction:

From the reaction, we know that 2 moles of potassium permanganate produces 1 mole of oxygen

${\text{2KMnO}}_{\text{4}}\text{(s) }\to {\text{K}}_{\text{2}}{\text{MnO}}_{\text{4}}{\text{(s) + MnO}}_{\text{2}}{\text{(s) + O}}_{\text{2}}\text{(g)}$.