Determine the direction in which the following reaction is spontaneous at 25oc: mg2+(aq) + k(s) < > mg(s) + k+(aq) determine the equilibrium constant k and go using the cell potential for this reaction and which will be the anode and cathode?

The and of the reaction is and -108080 J respectively.

Explanation:

For the given cell reaction:

The half reaction follows:

Oxidation half reaction:

Reduction half reaction:

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

To calculate the of the reaction, we use the equation:

Putting values in above equation, we get:

where,

= Standard Gibbs free energy of the reaction = ?

n = number of electrons exchanged = 2

F = Faraday's constant = 96500

= standard electrode potential of the cell = 0.56 V

Putting values in above equation, we get:

R = Gas constant = 8.314 J/K.mol

T = temperature of the reaction =

= equilibrium constant of the reaction = ?

Putting values in above equation, we get:

Hence, the and of the reaction is and -108080 J respectively.

so what is the problem with your lab report and whats the subject of the lab report? i will you

a pan containing water is placed in a positio n where it is exposed to a 10 mile per hour wind. the pan contains a uniform depth of 1.27 cm of water, is quite wide, and has a length of 2.44 m in the wind direction. the water in the pan is at a constant temperature of 15.5 °c.