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Hydrogen peroxide decomposes spontaneously to yield water and oxygen gas according to the reaction equation:2H2O2 (aq) -> 2H2O (l) O2 (g)The activation energy for this reaction is 75 kJ/mol. In the presence of a metal catalyst, the activation energy is lowered to 49 kJ/mol. What temperature would the non-catalyzed reaction need to be run at to have an equal rate to that of the metal-catalyzed reaction at 25°C?

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SOLVED: The hydrogen peroxide solution that you are using in this experiment is labeled as a 3.00% solution. This is a mass/volume percent, which can also be expressed as 3.00 g H2O2/100.0 mL of solution. In order to complete the calculations to determine activation energy, we need to express that concentration in units of molarity. Calculate the initial concentration of H2O2 in units of M.(Your answer should have 3 sig figs)