Problem: 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?   

FREE Expert Solution
Problem Details

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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