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:
the mass of one mole of an element, or Avogadro's number (6.02 x 1023) of atoms, is equal to its atomic mass in grams. In other words, 1 amu = 1 gram/mole. So if the mass of one hydrogen atom is 1 amu, the mass of one mole of hydrogen is 1 gram.
Explanation:
Answer:
has 6 valence electrons as its in group 6
the atom will gain electrons
the charge will be 2- as it will gain 2 electrons to be a full configuration
Answer:
2 mol H
Explanation:
For every 2 mol of NaOH, we're reacting 2 mol of H2O. In order to figure out how many mol of H are needed, it needs to be set up stochiometrically. Starting off with the given value, 1 mol of NaOH, we can then make a mol to mol ratio. For 2 mol of NaOH, we have 2 mol of H2O. For every 2 mol of H2O, we have 4 mol of H (this is because we are multiplying the coefficient by the subscript: 2 × 2). Now, we can solve for our answer.
1 mol NaOH × (2 mol H₂O / 2 mol NaOH) × (4 mol H / 2 mol H₂O)
= 2 mol H
Thus, we get 2 mol of H are needed to completely react 1 mol of NaOH.
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Wikipedia › wiki › Aquifer
I hope this helps
