Question

If an aqueous solution of HNO3 is electrolyzed for 15.00 min at a steady current of 1.39 A, what volume of H2 (g) at 25.0°C and 1.05 atm will be collected at the cathode? vol H2 (L) = 18.8 The reaction is: 2 H+ (aq) + 2e → H2 (g) Submit Answer Incorrect. Tries 4/45 Previous Tries

Answer 1

2HNO3(aq) → H2 90 + 2NO, (99+0200 Ionic equation for oxidation of tons 247 +2e - M, C88) It takes a molds of at charge to create one mole of H₂. 1:39 A for 15 min means a total charge transfer if 1:39x 36X60212510; each election carries 1.6022x109c, so that amount of charge reprent 7.808x102 cleason which is 7808818²/6.021 X 1023 = 0.01296 molds of electors This will produce note 0.00648 moles & Hz from the gas formule prannt V=NRT/P = 0.00648700806 L-atm 1 malik x 290k - logatm. = 0.75L volume H₂ (L) = 0.15L