During a lab class, a student connects a zinc bar with a silver bar through an e

Question

During a lab class, a student connects a zinc bar with a silver bar through an electrical wire, and puts both bars into a 1.0 M AgNO3 solution to assembly a voltaic cell. After 0.2 moles of electrons are transferred, how much mass was lost from the anode? During a lab class, a student connects a zinc bar with a silver bar through an electrical wire, and puts both bars into a 1.0 M AgNO3 solution to assembly a voltaic cell. After 0.2 moles of electrons are transferred, how much mass was lost from the anode? During a lab class, a student connects a zinc bar with a silver bar through an electrical wire, and puts both bars into a 1.0 M AgNO3 solution to assembly a voltaic cell. After 0.2 moles of electrons are transferred, how much mass was lost from the anode?

Explanation / Answer

anode reaction is

Zn ...............> Zn2+ + 2e

so as

0.2 moles of electrons are transferred.

Hence moles of Zn lost = 0.2 / 2 = 0.1 mole = 0.1 * 65.3 = 6.53 gm.

so 6.53 gm mass lost from anode.

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