An unknown metal, X, has been deposited on the cathode of an electrolytic cell using an electric current of 3.30 Amps for a period of 25.0 mins:  2X2+ + 2 e– → X  The mass of X collected at the cathode was 1.51 g.  Identify the unknown metal, X.

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: MnO₂ (s) + 4H* (aq) + 2Cr²+ (aq) → Mn²+ (aq) + 2H₂O (1) + 2Cr³+ (aq) 2+ 2+ 3+ Suppose the cell is prepared with 3.73 MH* and 1.42 M Cr²+ in one half-cell and 4.21 M Mn²+ and 3.05 M Cr³+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 1 x10 X μ 00 Ś

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2VO₂ (aq) + 4H* (aq) + Fe (s) → 2VO²+ (aq) + 2H₂O (1)+Fe²+ (aq) Suppose the cell is prepared with 3.37 M VO and 3.31 MH* in one half-cell and 6.13 M VO²+ and 2.52 M Fe²+ in the other. 2+ 2+ Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.

The amount of lactic acid, HC3H5O3, produced in a sample of muscle tissue was analyzed by reaction with hydroxide ion. Hydroxide ion was produced in the sample mixture by electrolysis. The cathode reaction is given below. 2 H2O(l) + 2 e− → H2(g) + 2 OH− (aq) Hydroxide ion reacts with lactic acid as soon as it is produced. The endpoint of the reaction is detected with an acid-base indicator. It required 104 s for a current of 13.1 mA to reach the endpoint. How many grams of lactic acid (a monoprotic acid) were present in the sample?