Rate of reaction (2018 VCE) 1) Hydrogen peroxide, H2O2, in aqueous solution at room temperature decomposes slowly and irreversibly to form water, H2O, and oxygen, O2, according to the following equation. 2H2O2(aq) → 2H2O(l) + O2(g) ∆H < 0 a) What effect will increasing the temperature have on the rate of O2 production? Use collision theory to explain your answer Solution b) When a small lump of manganese(IV) dioxide, MnO2, is added to the H2O2 solution, the rate of O2 production increases, but when powdered MnO2 is added instead, the rate of O2 production is greatly increased. The MnO2 is recovered at the end of the reaction. State the function of MnO2 in this reaction. Solution c) A solution of H2O2 is labelled ‘10 volume’ because 1.00 L of this solution produces 10.0 L of O2 measured at standard laboratory conditions (SLC) when the H2O2 in the solution is fully decomposed. Calculate the concentration of H2O2 in the ‘10 volume’solution, in grams per litre, when this solution is first prepared. Solution 