Data and Results Table Include proper units and significant

Data and Results Table (Include proper units and significant figures for all measurements.) Trial 1 Trial 2 Mass of the flask 02.20% 103.202 Mass of the flask+hydrogen peroxide solution Calculated mass of hydrogen peroxide solution Molarity of KMnOs solution (given on the bottle Initial buret reading Final buret reading Calculated volume of KMnOs added Calculated moles of KMnOs added Calculated moles of H0 reacted Calculate grams of H20z in flask Calculated % H202 in unknown solution 2 1 10,56 Results and Questions 1. Write the balanced equation for the reaction between hydrogen peroxide and potassium permanganate that occurs in acidic solution. 2. What is the molar ratio of reactants H202 to KMnO4 in this titration? 3. The moles of KMnOs reacted in each trial can be calculated using the volume (liters) of the KMnO, added and the molarity (ie. moles/liter) given for the permanganate solution. Calculate the moles of KMnO4 reacted in each trial and fill these values into the Data and Results Table 0.09o kui

Solution

1) 5H2O2(aq)+2KMnO4(aq) +6H⁺(aq) --->5O2(g) +2Mn²⁺ (aq) +8H2O(l)(balanced equation)

2)molar ratio of H2O2 to KMnO4=5:2

3)calculated mol of KMnO4 added=molarity(KMnO4)*Volume(KMnO4)

trial 1) calculated mol of KMnO4 added=(0.0908mol/L)*0.037L=0.00336mol

trial 2) calculated mol of KMnO4 added=(0.0908mol/L)*0.015L=0.00136 mol

4) mol of H2O2 reacted=5/2 mol KMnO4 added

trial 1) calculated mol of H2O2 reacted=5/2*0.00336mol=0.0084 mol

trial 2) calculated mol of H2O2 reacted=5/2*0.00136mol=0.0034 mol

5) grams of H2O2 in trial 1=mol*molar mass=0.0084mol*(34.015g/mol)=0.286 g(trial 1)

grams of H2O2 in trial 1=mol*molar mass=0.0034mol*(34.015g/mol)=0.116g(trial 2)