Answer: To answer this question, we need to use the balanced chemical equation for the reaction between KMnO4 and MnSO4:
2 KMnO4 + 3 MnSO4 + 2 H2O → 5 MnO2 + K2SO4 + 2 H2SO4
From the equation, we can see that two moles of KMnO4 react to form five moles of MnO2. We can use this information, along with the molar mass of KMnO4, to calculate the number of moles of MnO2 that can be formed from 196.0 g of KMnO4:
1 mole of KMnO4 = 158.03 g
Number of moles of KMnO4 = 196.0 g / 158.03 g/mol = 1.24 mol
According to the stoichiometry of the balanced chemical equation, for every 2 moles of KMnO4, 5 moles of MnO2 are produced. Therefore, we can use a proportion to find the number of moles of MnO2 produced from 1.24 moles of KMnO4:
2 moles KMnO4 / 5 moles MnO2 = 1.24 moles KMnO4 / x moles MnO2
Solving for x, we get:
x = (5 moles MnO2 × 1.24 moles KMnO4) / 2 moles KMnO4 = 3.1 moles MnO2
Therefore, 3.1 moles of MnO2 can be formed from 196.0 g of KMnO4.
Step-by-step explanation: