work plz

2 H2O2 (aq) 2 H20 (1) + O2(g) 3. The mass of an aqueous solution of hydrogen peroxide is 6.159 g. The hydrogen peroxide in the solution decomposes completely according to the reaction represented above. The oxygen produced is collected in an inverted graduated tube over water at 23.7C and has a volume of 181.9 ml when the water level Inside and outside of the tube are the same. The atmospheric pressure in the lab is 762.8 torr, and the equilibrium vapor pressure of water at 23.7C is 22.0 torr. a. Calculate the partial pressure, in torr, of oxygen in the gas-collection tube. (1 point) b. Calculate the number of moles of oxygen produced in the reaction. (2 points) Calculate the mass, in grams, of hydrogen peroxide that decomposed. (2 points) d. Calculate the percent of hydrogen peroxide, by mass, in the original 6.159 g aqueous sample. (1 point) e. Identify the oxidation number of oxygen in hydrogen peroxide and the oxidation number of oxygen in oxygen gas. (2 point) f. Write the balance oxidation half-reaction for this reaction. (2 points) C