4. Does the following reaction occur spontancously? Assume standard conditions,

Question

4. Does the following reaction occur spontancously? Assume standard conditions, and show an appropriate calculation of question Explain how your Ecel value is used to answer the 2 Ag(s) (s)-2 Ag (ag) 2 (aq) 5. The aluminum-manganese voltaic cell utilizes the following reaction with a measured cell potential of 0.48 V at 298 Mn(a)2 Als)-3 Mn(s) 2 Al (aq) What is AG for this reaction? 6. Calculate the value of Eel for the following reaction at 298 K given the non-standard concentrations listed. [Cu 0.010 M and [Na ]-0.50 M

Explanation / Answer

4)

2 Ag(s) + I2(s) ------> 2 Ag+(aq) + 2 I-(aq)

From stand reduction potential values,

E0 Ag/Ag+ = +0.8 V

E0 I2/I- = +0.54 V

so higher the reduction potential value then it under go reduction, so

E0 cell = E0 cathode - E0 anode

E0 cell = 0.8 - 0.54 = +0.26 V

5)

3 Mn+2(aq) + 2 Al(s) -------> 3 MN(s) + 2 Al+3(aq)

For the above reaction E cell = 0.48 V

we have the formula dG = - n * F * E0 cell

dG = - 6 * 96500 * 0.48

dG = -277920 J

dG = -277.92 kJ

6)

According to Nernst equation,

Ecell = E0 cell - 0.059/nlog[Na+]/[Cu+2]

E0 cell from the standard values is given by,

E0 cell = E cathode - E anode

E0 cell = 0.34 - (-2.71)

E0 cell = +3.05 V

E cell = 3.05 - 0.059/2*log(0.5/0.01)

E cell = +2.99 V

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