Question

Part IV. Decomposition Into a test tube, place about 2 mL of 3% hydrogen peroxide along with a pea size amount of Mnog Manganese dioxide, the common name, is used as a catalyst. Remember, that a catalyst is used to lower the activation energy of a reaction, thereby speeding up the reaction. It does not get con- sumed in the reaction and therefore is not part of your balanced chemical equation. It is written above the reaction arrow in a chemical equation. Note any evidence of the reaction. Has a gas been evolved? Light a wood splint and blow out the flame. Put the glowing splint into the test tube. What happens? Remember, when writing your balanced equation, H, gas was not produced. TABLE 9.15 Observations decomposition of hydrogen peroxide Condensation it turned off the flame. not hot firy when the splorasin' eubbles in the fiery liquid a. If a gas was evolved, what was the identity of the gas? Explain how you came to this conclusion using experimental evidence. Den of the test tube. nce. Oxygen Reactants Products Balanced Chemical Equation

Answer 1

We are using 3% hydrogen peroxide so peroxide in aqueous state. The gas evolved is Oxygen, and can be confirmed by using flame test - it will becomes brightly burns. The observation is dense white color fumes evolved even though oxygen is colorless

Reactants: H₂O₂ (aq)

Products: H₂O (l) and O₂ (g)

The balanced chemical reaction equation is : 2H₂O₂ (aq) --> 2H₂O (l) + O₂ (g)

The reaction can be seen as

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