If the cell is initially at standard state conditions, which of the following st

Question

If the cell is initially at standard state conditions, which of the following statement is true? Zn^2+ (aq) + 2e^- Zn(s): E degree = -0.76 V Cu^2+(aq) + 2e^- Cu(s); E degree = 0.34 V a. Initially Delta G = 212kJ, and it will become more positive with time. b Initially Delta G = -212kJ, and it will not change with time. c. Initially Delta G = -2l2kJ, and it will become more negative with time. d. Initially Delta G = 212 kJ, and it will become more negative with time. e. Initially Delta G = -212 kJ, and it will become more positive with time.

Explanation / Answer

The cell reaction is Zn +Cu+2 ------> Zn+2 + Cu

The Eo cell initially = 0.34 v -(-0.76V) = 1.1V

The realtion between Delta G and E cell is

delta Go = -nFEcell

= -2 x 96500C x 1.1 V= 212300 J

= -212.3 kJ

As the reaction progresses the voltage drops, so the value of delta g becomes less negative (or more positive)with time.

OPtion E

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