According to the balanced chemical equation
5 H₂C₂O₄(aq) + 2 MnO₄^-(aq) + 6 H⁺(aq) → 10 CO₂(g) + 2 Mn²⁺(aq) + 8 H₂O(l)
0) 3500 grams of oxalic acid,H₂C₂O₄ will react with ________ moles of permanganate,MnO₄^-.

Question

Quizplus · Accepted Answer

3500 grams of oxalic acid, H2C2O4 will react with 0.001554 moles of permanganate, MnO4-.To determine the number of moles of permanganate required, we can use the stoichiometry of the balanced chemical equation:5 H2C2O4(aq) + 2 MnO4-(aq) + 6 H+(aq) → 10 CO2(g) + 2 Mn2+(aq) + 8 H2O(l)From the equation, we can see that 5 moles of oxalic acid react with 2 moles of permanganate. Therefore, the number of moles of permanganate required to react with 3500 grams of oxalic acid can be calculated as follows:Moles of oxalic acid = 3500 g / 90.03 g/mol = 38.87 molMoles of permanganate required = (38.87 mol oxalic acid) x (2 mol permanganate / 5 mol oxalic acid) = 0.001554 molTherefore, the correct answer is A) 0.001554.

According to the Balanced Chemical Equation