Answer: The net ionic equation for the cobalt-silver voltaic cell is 
Explanation: In cobalt-silver voltaic cell, one half of the cell consists of cobalt electrode immersed in
solution ( which means that
are present in the solution) and other half of the cell consists of the Ag electrode immersed in
solution ( which means that
is present in the solution)
The two electrodes are joined by the copper wire. The cobalt electrode acts as an anode and the silver electrode acts a cathode.
At anode, oxidation reaction takes place and at cathode, reduction reaction takes place.
At Anode : 
At Cathode: ![[Ag^+(aq.)+e^-\rightarrow Ag(s)]\times 3](https://tex.z-dn.net/?f=%5BAg%5E%2B%28aq.%29%2Be%5E-%5Crightarrow%20Ag%28s%29%5D%5Ctimes%203)
Net ionic equation: 
Answer:
455 Kcal
Explanation:
2Cl2(g) + 7O2(g) + 130kcal → 2Cl2O7(g)
Rearranging we get,
2Cl2(g) + 7O2(g) → 2Cl2O7(g) Δ H = 130 kcal . mol⁻¹
So for per mol reaction will be as above.
In case of 7 mols of product, we need 7/2 mole ratio x 130 = 455 Kcal
Robert A. Millikan and Harvey Fletcher performed the oil drop experiment.