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Solution - Calculate E and Ag for the Following at 28°C - Galvanic Cells - Introduction

Question

Calculate E and AG for the following at 28°C:

Mg(s) + Sn2+(0.04M) → Mg2+(0.06M) + Sn(s)

Ecell = 2.23V

Is the reaction spontaneous?

Solution

`E=E_`

`[Mg^(+2)]=0.06`

`E=2.23-0.059/2`

`E=2.23-0.059/2log((3xx10^-2)/(2xx10^-2))`

     `=2.23-0.059/2log1.5`

     `=2.23-(0.059/2xx(0.1760))`

       = 2.23 - 0.0052

        =2.225

Ecell = 2.225

Now ΔG = -nFE

n = 2mol, F = 96500C, E = 2.225

ΔG = -2 x 96500 x 2.225

      = -429425CV

ΔG = -429.425kJ

The reaction is spontaneous.

Is there an error in this question or solution?

APPEARS IN

2014-2015 (March)
Question 4.2 | 7 marks (combined)
Solution for question: Calculate E and Ag for the Following at 28°C concept: Galvanic Cells - Introduction. For the courses HSC Science (Computer Science), HSC Science (Electronics), HSC Science (General)
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