Decomposition of Hydrogen peroxide occurs as follows:
2 H2O2 (aq) ---> 2 H2O (l) + O2(g) enthalpy: -196.1 kJ/mol
The decomposition of hydrogen peroxide is possible when there are suitable conditions for the reaction to occur like activation energy of the reaction is about 75 kJ/mol. If this energy is available then there is no need of any catalyst. On the other hand, use of Platinum metal catalysts can decrease the demand of energy up to 49 kJ/mol.
This shows that decomposition, of hydrogen peroxide results in the formation of water and oxygen.
2 H2O2 (aq) ---> 2 H2O (l) + O2(g) enthalpy: -196.1 kJ/mol
The decomposition of hydrogen peroxide is possible when there are suitable conditions for the reaction to occur like activation energy of the reaction is about 75 kJ/mol. If this energy is available then there is no need of any catalyst. On the other hand, use of Platinum metal catalysts can decrease the demand of energy up to 49 kJ/mol.
This shows that decomposition, of hydrogen peroxide results in the formation of water and oxygen.