Oxalic acid C2H2O4 is a metabolic product of many molds. Although oxalic acid is toxic to humans if ingested, many plants and vegetables contain significant amounts of oxalic acid or oxalate salts. In solution, oxalic acid can be oxidized by air via the following chemical equation: H2C2O4 (aq) + O2 (g) -> H2O2 (l) + 2 CO2 (g) If a plant metabolized enough oxalic acid to produce 3.2L of CO2​ on a day when the temperature was 29°C and the pressure was 752 mmHg,   a) how many grams of oxalic acid were converted to CO2​? b) Given that air is 2121% oxygen, what volume of air was needed for the oxidation?

Identify the oxidizing and reducing agent 4NaClO3 (aq) + 2 SO2 (aq) + 2H2SO4 -> 4NaHSO4 (aq) + 4ClO2 (g)

We want to determine the purity of copper in the wires used for electrical cables. This can be done using an electrolysis device with platinum electrodes and the following procedure: Weigh the electrodes and a piece of copper wire from a wire and record their mass. Dissolve the copper metal (Cu) with a solution of relatively dilute HNO3 (aq). Add hydrazine (N2H4) to the solution to give the solution a reducing agent better than H2O. Place the solution in the electrolysis apparatus, immerse the electrodes in it and start transmitting electricity. Copper metal (Cu) begins to deposit on one of the two electrodes. At the same time, we observe that gas bubbles are released from the solution. When the reaction is complete, stop the passage of electricity, disconnect the electrode, to which Cu has been deposited, and after drying, weigh it. From the difference in mass of the electrode and the known amount of Cu that we had dissolved, we calculate the purity of Cu. (a) At which electrode is Cu…

We want to determine the purity of copper in the wires used for electrical cables. This can be done using an electrolysis device with platinum electrodes and the following procedure: Weigh the electrodes and a piece of copper wire from a wire and record their mass. Dissolve the copper metal (Cu) with a solution of relatively dilute HNO3 (aq). Add hydrazine (N2H4) to the solution to give the solution a reducing agent better than H2O. Place the solution in the electrolysis apparatus, immerse the electrodes in it and start transmitting electricity. Copper metal (Cu) begins to deposit on one of the two electrodes. At the same time, we observe that gas bubbles are released from the solution. When the reaction is complete, stop the passage of electricity, disconnect the electrode, to which Cu has been deposited, and after drying, weigh it. From the difference in mass of the electrode and the known amount of Cu that we had dissolved, we calculate the purity of Cu. (a) How can we remove Cu…

A solution containing 0.40249 g of CoCl2. xH2O was exhaustively electrolyzed to deposit 0.09937 g of metallic cobalt on a platinum cathode. What is the number of moles of water per mole of cobalt in the reagent? FW CoCl2 = 129.84 g/mol H2O = 18.02 g/molAW Co = 58.93 g/mol

The hardness of water (hardness count) is usually expressed in parts per million (by mass) of CaCO_3,which is equivalent to milligrams of CaCO_3 per liter of water. What is the molar concentration of Ca2+ ions in a water sample with a hardness count of 175 mgCaCO_3L ?

Explain the difference in pH between diH2O and tap water

5. Sol CaC204 is obtained by mixing solutions of CaCl2 and Na2C2O4. Write the formula of the Sol micelle, if it is known that during electrophoresis, the pellet moves to the cathode.

The chief chemist of the Brite-Metal Electroplating Co. isrequired to certify that the rinse solutions that are discharged from the company’s tin-plating process into the municipal sewer system contain no more than 10 ppm (parts per million) by mass of Sn2+. The chemist devises the following analytical procedure to determine the concentration. At regular intervals, a 100-mL (100-g) sample is withdrawn from the waste stream and acidified to pH = 1.0. A starch solution and 10 mL of 0.10 M potassium iodide are added, and a 25.0-mA current is passed through the solution between platinum electrodes. Iodine appears as a product of electrolysis at the anode when the oxidation of Sn2+ to Sn4+ is practically complete and signals its presence with the deep blue color of a complex formed with starch. What is the maximum duration of electrolysis to the appearance of the blue color that ensures that the concentration of Sn2+does not exceed 10 ppm?