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A voltaic cell consists of two H₂/H⁺ half-cells. Half-cell A has H₂ at 0.95 atm bubbling into 0.10 M HCl. Half-cell B has H₂ at 0.60 atm bubbling into 2.0 M HCl. Which half-cell houses the anode? What is the voltage of the cell?

Respuesta :

The voltage of the cell is 0.0385 V anode is present in half cell A

The reaction at half cell A is 2H^+ +2e→H2 (0.95atm 0.10 M HCl)

The reaction at half cell B is 2H^+ +2e→H2 (0.60 atm, 2.0 M HCl)

Oxidation takes place at the anode, it has a negative charge. Therefore, the electrode in A is negative and electrode B is positive.

In a concentration cell, the anode half-cell contains the more dilute solution, which is the solution in half-cell A.

Applying the Nernst equation, we get

Ecell= E0cell-0.0591/n logQ

Ecell=0-0.0591/2 log[H^+ (dil)/H^+ (conc)]

Ecell=0.0385V

What is a voltaic cell?

  • A Voltaic Cell is a galvanic cell which is an electrochemical cell that uses spontaneous redox reactions to generate electricity. It consists of two separate half-cells.
  • A half-cell is composed of an electrode containing a strip of metal M within a solution containing M^n+ ions in which M is any arbitrary metal.

To learn more about voltaic cells visit:

https://brainly.com/question/1370699

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