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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)

#### Video TutorialsVIEW ALL [3]

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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