Chemistry, 03.03.2020 00:06 cheyennebatz3609

Calculate the emf for the following reaction. Will the reaction occur spontaneously at 25°C, given that [Fe2+] = 0.600 M and [Cd2+] = 0.00550 M? Cd(s) + Fe2+(aq)→Cd2+(aq) + Fe(s) E o Cd2+/Cd = −0.40 V E o Fe2+/Fe = −0.44 V

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Answer from: tayjohnson0042

The EMF of the cell is -0.100 V and the reaction is non-spontaneous

Explanation:

The half reaction for the equation follows:

Oxidation half reaction: $Cd(s)\rightarrow Cd^{2+}(aq,0.00550M)+2e^-;E^o_{Cd^{2+}/Cd}=-0.40V$

Reduction half reaction: $Fe^{2+}(aq,0.600M)+2e^-\rightarrow Fe(s);E^o_{Fe^{2+}/Fe}=-0.44V$

Net cell reaction: $Cd(s)+Fe^{2+}(aq,0.600M)\rightarrow Cd^{2+}(aq,0.00550M)+Fe(s)$

Oxidation reaction occurs at anode and reduction reaction occurs at cathode.

To calculate the $E^o_{cell}$ of the reaction, we use the equation:

$E^o_{cell}=E^o_{cathode}-E^o_{anode}$

Putting values in above equation, we get:

$E^o_{cell}=-0.44-(-0.40)=-0.04V$

To calculate the EMF of the cell, we use the Nernst equation, which is:

$E_{cell}=E^o_{cell}-\frac{0.059}{n}\log \frac{[Cd^{2+}]}{[Fe^{2+}]}$

where,

$E_{cell}$ = electrode potential of the cell = ?

$E^o_{cell}$ = standard electrode potential of the cell = -0.04 V

n = number of electrons exchanged = 2

$[Cd^{2+}]=0.00550M$

$[Fe^{2+}]=0.600M$

Putting values in above equation, we get:

$E_{cell}=-0.04-\frac{0.059}{2}\times \log(\frac{0.00550}{0.600})$

$E_{cell}=-0.100V$

For the reaction to be spontaneous, the Gibbs free energy of the reaction must come out to be negative.

Relationship between standard Gibbs free energy and standard electrode potential follows:

$\Delta G^o=-nFE^o_{cell}$

For a reaction to be spontaneous, the standard electrode potential must be positive.

Hence, the EMF of the cell is -0.100 V and the reaction is non-spontaneous

Answer from: Quest

i just calculated it all out, and not including weekends, and all the different days off. as of this school year (2018-2019) students are spending 2198 hours in school this year

Answer from: Quest

definition

entropy is a measure of the randomness or the extent of disorder of a chemical process.

enthalpy is a measure of the heat change of a reaction occurring at a constant pressure.

measurement units:

entropy is measured in joule per kelvin (jk⁻¹) whereas enthalpy is measured in joule per mole (jmol⁻¹)

requirements:

entropy has no requirements or limits, and its change is measured by the division between the heat change of the chemical process and the temperature.

in contrast, enthalpy can only be related to the heat change of the reaction under standard conditions.

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Calculate the emf for the following reaction. Will the reaction occur spontaneously at 25°C, given t...