Hydrogen peroxide, H2O2, is common in many households and is used as a bleaching agent. It usually comes in a dark, opaque bottl
e. When exposed to heat or light, hydrogen peroxide will decompose according to the reaction: 2 H2O2→2 H2O + O2
Iron Nitrate has been shown to be an effective catalyst to accelerate the decomposition process, and sodium phosphate can inhibit the effects of this catalytic effect.
Naturally, the consumer does not want their hydrogen peroxide to decompose. Consider the factors affecting reaction rate that you learned about in this lesson. What should the consumer should do to prevent the decomposition of hydrogen peroxide?. For example, should the hydrogen peroxide be stored in a warm or cool location? Use scientific reasoning to support your response.
It has been confirmed that heat and light aids in the decomposition of hydrogen peroxide according to the equation; 2H2O2→2 H2O + O2.
This means that hydrogen peroxide must be stored in a cool place. This will reduce its rate of decomposition. Secondly, it should be stored in amber bottles away from light since light also aids in its decomposition.
Thirdly, drops of sodium phosphate may be added to prevent its catalytic decomposition during storage.
