Advertisements
Advertisements
प्रश्न
A copper electrode is dipped in 0.1 M copper sulphate solution at 25°C. Calculate the electrode potential of copper.
[Given: \[\ce{E^0_{{Cu^{2+}|Cu}}}\] = 0.34 V]
Advertisements
उत्तर
Given that [Cu2+] = 0.1 M
\[\ce{E^0_{{Cu^{2+}|Cu}}}\] = 0.34 V
Ecell = ?
Cell reaction is
\[\ce{Cu^{2+}_{( aq)} + 2e^- -> Cu_{(s)}}\]
Ecell = `"E"^0 - 0.0591/"n" log (["Cu"])/(["Cu"^(2+)])`
= `0.34 - 0.0591/2 log 1/0.1`
= 0.34 – 0.0296
= 0.31 V
APPEARS IN
संबंधित प्रश्न
Derive a relation between ΔH and ΔU for a chemical reaction. Draw neat labelled diagram of calomel electrode. Resistance and conductivity of a cell containing 0.001 M KCI solution at 298K are 1500Ω and 1.46x10-4 S.cm-1 respectively.
What happens if external potential applied becomes greater than E°cell of electrochemical cell?
Define cathode
Reduction potential of two metals M1 and M2 are \[\ce{E^0_{{M_1^{2+}|M_1}}}\] = −2.3 V and \[\ce{E^0_{{M_2^{2+}|M_2}}}\] = 0.2 V. Predict which one is better for coating the surface of iron.
Given: \[\ce{E^0_{{Fe^{2+}|Fe}}}\] = −0.44 V
`E_(cell)^Θ` = 1.1V for Daniel cell. Which of the following expressions are correct description of state of equilibrium in this cell?
(i) 1.1 = `K_c`
(ii) `(2.303RT)/(2F) logK_c` = 1.1
(iii) `log K_c = 2.2/0.059`
(iv) `log K_c` = 1.1
Can absolute electrode potential of an electrode be measured?
Standard reduction electrode potentials of three metals A, B and C are respectively + 0.5 V, – 3.0 V. and – 1.2 V. The reducing powers of there metal is.
Which of the following is incorrect?
What should be the signs (positive/negative) for \[\ce{E^0_{cell}}\] and ΔG0 for a spontaneous redox reaction occurring under standard conditions?
Explain why the anode is of negative polarity in a galvanic cell.
