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The standard potential of the following ...

The standard potential of the following cell is `0.23V` at `15^(@)C` and `0.21V` at `35^(@)C:`
`Pt|H_(2(g)|HCl(aq)|AgCl(s)|Ag(s)`
`a.` Write the cell reaction.
`b.` Calculate `DeltaH^(c-)` and `DeltaS^(c-)` for the cell reaction by assuming that these quantities remain unchanged in the range `15^(@)C` to `35^(@)C`
`c.` Calculate the solubility of `AgCl` in water at `25^(@)C`.
Given `:` The standard reduction potential of `Ag^(o+)(aq)|Ag(s)` is `0.80V` at `25^(@)C`.

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The standard potential of the following cell is 0.23 V at 15^(@)C and 0.21V at 35^(@)C . Pt|H_(2) |HCl(aq) |Agcl (s)|g(s) (i) write the cell reaction . (ii) Calculate DeltaH^(@) and DeltaS^(@) for the cell reaction by assuming that these quantities remain unchanged in the range 15^(@)C to 35^(@)C . (iii) calculate the solubility of AgCl in water at 25^(@)C . Give , the standard reduction potential of the (Ag^(+)(aq) //Ag(s) is 0.80 V at 25^(@) C .

The EMF of the following cellis 1.05V at 25^(@)C: Pt,H_(2)(g)(1.0 atm)|NaOH(0.1m),NaCl(0.1M)|AgCl(s),Ag(s) a. Write the cell reaction, b. Calculate pK_(w) of water.

For the cell Zn|ZnCl_(2)(m)|AgCl,E is 1.24V at 25^(@)C and 1.260V at 35^(@)C of m=10^(-3) . Write down the cell reaction and calculate DeltaG, DeltaH, and DeltaS at 25^(@)C .

The E^(@) at 25^(@) C for the following reaction is 0.22 V. Calculate the equilibrium constant at 25^(@) C : H_(2)(g)+2AgCl(s)to2Ag(s)+2HCl(aq)

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