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(a) The e.m.f. of the following cell at...

(a) The e.m.f. of the following cell at 298 K is 0.1745 V
`Fe(s) //Fe^(2+) (0.1 M) ////H^(+)(x M)//H_(2)(g) ("1 bar")//Pt (s)`
Given : `E_(Fe^(2+)//Fe)^(0) = - 0.44 V`
Calculate the `H^(+)` ions concentration of the solution at the electrode where hydrogen is being produced.
(b) Aqueous solution of copper sulphate and silver nitrate are electrolysed by 1 ampere current for 10 minutes in separate electrolytic cells. Will the mass of copper and silver deposited on the cathode be same or different? Explain your answer.

Text Solution

AI Generated Solution

### Step-by-Step Solution #### Part (a) 1. **Identify the Cell Reaction**: The cell reaction can be written as: \[ \text{Fe}^{2+} + 2\text{H}^+ \rightarrow \text{H}_2 + \text{Fe} ...
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Knowledge Check

  • Calculate the e.m.f. of the following cell at 298K : Pt(s)|Br_(2)(l)|Br^(-)(0.010M)||H^(+)(0.030M)|H_(2)(g)(1"bar")|Pt(s) Given : E_((1)/(2)Br_(2)//Br^(-))^(@)=+1.08V .

    A
    `-1.288V`
    B
    `1.288V`
    C
    `0.128V`
    D
    `-128V`