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

Question

Quizplus · Accepted Answer

The molar mass of oxalic acid (H2C2O4) is approximately 90.03 g/mol. Given 0.875 grams of oxalic acid, the number of moles is calculated as 0.875 g / 90.03 g/mol = 0.009717 moles. According to the balanced chemical equation, 5 moles of oxalic acid react with 2 moles of permanganate. Therefore, the moles of permanganate that will react with 0.009717 moles of oxalic acid are (0.009717 moles of oxalic acid) * (2 moles of permanganate / 5 moles of oxalic acid) = 0.003885 moles of permanganate.

According to the Balanced Chemical Equation 5 H2C2O4(aq)+ 2 MnO4-(aq)

According to the Balanced Chemical Equation 5 H₂C₂O₄(aq)+ 2 MnO₄^-(aq)