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प्रश्न
Answer the following:
Predict whether the following reaction would occur spontaneously under standard state condition.
\[\ce{2Ag_{(s)} + Ni^{2+}_{ (aq)} -> 2Ag^{+}_{ (aq)} + Ni_{(s)}}\]
उत्तर
\[\ce{2Ag_{(s)} + Ni^{2+}_{ (aq)} -> 2Ag^{+}_{ (aq)} + Ni_{(s)}}\]
At anode: \[\ce{2Ag_{(s)} -> 2Ag^+_{ (aq)} + 2e^-}\]
At cathode: \[\ce{Ni^{2+}_{ (aq)} + 2e^- -> Ni_{(s)}}\]
From the electrochemical series we have,
`"E"_("Ag")^circ` = 0.799 V and `"E"_"Ni"^circ` = - 0.257 V
For cell having Ag as anode and Ni as cathode.
`"E"_"cell"^circ = "E"_"Ni"^circ - "E"_"Ag"^circ`
= - 0.257 V - 0.799 V
`"E"_"cell"^circ` = - 1.056 V
Emf of cell being negative, the given cell reaction is nonspontaneous.
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संबंधित प्रश्न
Write applications of electrochemical series.
Answer the following:
Identify oxidising agents and arrange them in order of increasing strength under standard state conditions. The standard potentials are given in parenthesis.
Al (–1.66V), Al3+(–1.66V), Cl2 (1.36V), Cd2+ (–0.4V), Fe (–0.44V), I2 (0.54V), Br- (1.09V).
Answer the following:
Which of the following species are reducing agents? Arrange them in order of increasing strength under standard state conditions. The standard potentials are given in parenthesis.
K (–2.93V), Br2(1.09V), Mg(–2.36V), Ce3+(1.61V), Ti2+(–0.37V), Ag+ (0.8 V), Ni (–0.23V).
Write two applications of electrochemical series.
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Which of the following metals does NOT displace zinc from it's solution?
Which element among the following is used as reducing agent for reduction of remaining three elements from their oxides?
Which metal from following has highest tendency to undergo oxidation?
The reduction potential is the tendency of an electrode to ______
Identify the weakest oxidising agent among the following.
Which of the following cannot be considered as an application of electrochemical series?
Calculate the value `"E"_"cell"^circ` at 298 K for the following cell.
\[\ce{Al | Al^{3+} (0.01 M) || Sn^{2+} (0.015 M) | Sn}\]
`"E"_("Al"^(3+)//"Al")^circ` = - 1.66 V and `"E"_("Sn"^(2+)//"Sn")^circ` = - 0.14 V
Define electrochemical series.
