Advertisements
Advertisements
Question
A gas X at 1 atm is bubbled through a solution containing a mixture of 1 MY− and 1 MZ− at 25°C. If the reduction potential of Z > Y > X, then ______.
Options
Y will oxidise X and not Z
Y will oxidise Z and not X
Y will oxidise both X and Z
Y will reduce both X and Z
Advertisements
Solution
A gas X at 1 atm is bubbled through a solution containing a mixture of 1 MY− and 1 MZ− at 25°C. If the reduction potential of Z > Y > X, then Y will oxidise X and not Z.
Explanation:
A species can oxidise another if it has a higher reduction potential.
\[\ce{E^{\circ}_{Z} > E^{\circ}_{Y} > E^{\circ}_{X}}\]
So, Y− can oxidise X (since Y has a higher reduction potential than X), but cannot oxidise Z, because Z has an even higher reduction potential than Y. Hence, Y will oxidise X and not Z.
APPEARS IN
RELATED QUESTIONS
How many moles of electrons are required for reduction of 2 moles of Zn2+ to Zn?
If one mole electrons is passed through the solutions of CrCl3, AgNO3 and NiSO4, in what ratio Cr, Ag and Ni will be deposited at the electrodes?
Two metals M1 and M2 have reduction potential values of −xV and +yV respectively. Which will liberate H2 and H2SO4.
An electrochemical cell can behave like an electrolytic cell when ______.
For the given cell, \[\ce{Mg | Mg^{2+} || Cu^{2+} | Cu}\]
(i) \[\ce{Mg}\] is cathode
(ii) \[\ce{Cu}\] is cathode
(iii) The cell reaction is \[\ce{Mg^+ Cu^{2+} -> Mg^{2+} + Cu}\]
(iv) \[\ce{Cu}\] is the oxidising agent
Depict the galvanic cell in which the cell reaction is \[\ce{Cu + 2Ag^+ -> 2Ag + Cu^{2+}}\]
Consider a cell given below:
\[\ce{Cu | Cu^{2+} || Cl^{-} | Cl_{2},Pt}\]
Write the reactions that occur at anode and cathode
Match the terms given in Column I with the units given in Column II.
| Column I | Column II |
| (i) Λm | (a) S cm-¹ |
| (ii) ECell | (b) m-¹ |
| (iii) K | (c) S cm2 mol-¹ |
| (iv) G* | (d) V |
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.
What are electrochemical reactions?
