Consider the following balanced redox equation:
H2O + 2 MnO4 – + 3 SO32- → 2 MnO2 + 3 SO42- + 2 OH –
a) How many moles of SO32- (MW:80.07 g/mol) are required to completely react with 20.3 mL of a 0.500 M MnO4– (MW: 118.90 g/mol) solution?
a. 0.0152 moles SO32-
b. 0.0067 moles SO32-
c. 0.005075 moles SO32-
d. 0.3045 moles SO32-
b) How many mL of a 1.25 M Na 2SO3 (MW: 126 g/mol) are required to completely react with 2.55 mL of a 3.50 M KMnO4 (MW: 158 g/mol) solution?
c) How many grams of MnO 2 (MW: 86.94 g/mol) are produced when 32.0 mL of 0.615 M MnO 4- (MW: 118.90 g/mol) reacts with excess water and sulfite?
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