Calculate the number of grams of metal M produced in 1.055 hour by the electrolysis if the electrical current is 16.273 A. The molar mass of metal M is 58.148 g/mol. M2+ + 2 e– → M Recall that, C = A*s, and Faraday’s constant, F, is 96,485 C/mole of electrons.

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?

Suppose 830. mmol of electrons must be transported from one side of an electrochemical cell to another in 231. seconds. Calculate the size of electric current that must flow. Be sure your answer has the correct unit symbol and the correct number of significant digits.

Calculate the voltage of the redox reaction of element X (group 2) if the Gibb’s free energy evolved during the redox reaction is + 150 kJ/mol. (Faraday constant, 9.649 x 104C)

a) Balance the following redox reaction occurring under basic conditions using the Oxidation  Number method: IO31-(aq) + C2O42-(aq) → I1-(aq) + CO2(g)  b) Identify the oxidizing agent and the reducing agent. Give reasons for your choices.

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Suppose 190. mmol of electrons must be transported from one side of an electrochemical cell to another in 21.0 minutes. Calculate the size electric current that must flow. Be sure your answer has the correct unit symbol and the correct number of significant digits. 0 x10 • X μ Ś