JEE Main 2019 (Online) 12th January Morning Slot | Electrochemistry Question 86 | Chemistry

JEE Main 2019 (Online) 12th January Morning Slot

MCQ (Single Correct Answer)

-1

The standard electrode potential $${E^o }$$ and its temperature coefficient $$\left( {{{d{E^o }} \over {dT}}} \right)$$ for a cell are 2V and $$-$$ 5 $$ \times $$ 10^$$-$$4 VK^$$-$$1 at 300 K respectively.
The cell reaction is
Zn(s) + Cu²⁺ (aq) $$\buildrel \, \over \longrightarrow $$ Zn²⁺ (aq) + Cu(s)

The standard reaction enthalpy ($$\Delta $$_rH$${^o }$$) at 300 K in kJ mol^–1 is, [Use R = 8 JK^–1 mol^–1 and F = 96,000C mol^–1]

$$-$$ 412.8

$$-$$ 384.0

192.0

206.4

JEE Main 2019 (Online) 11th January Morning Slot

MCQ (Single Correct Answer)

-1

For the cell Zn(s) |Zn²⁺ (aq)| |M^x+ (aq)| M(s), different half cells and their standard electrode potentials are given below :

M^x+ (aq)/M(s)	Au³⁺(aq)/Au(s)	Ag⁺(aq)/Ag(s)	Fe³⁺(aq)/Fe²⁺ (aq)	Fe²⁺(aq)/Fe(s)
E⁰_M^x+_/M/(V)	1.40	0.80	0.77	$$-$$0.44

If $$E_{z{n^{2 + }}/zn}^0$$ = $$-$$ 0.76 V, which cathode will give maximum value of E^o_cell per electron transferred?

Ag⁺/Ag

Fe³⁺/Fe²⁺

Au³⁺/Au

Fe²⁺/Fe

JEE Main 2019 (Online) 10th January Evening Slot

MCQ (Single Correct Answer)

-1

In the cell

Pt$$\left| {\left( s \right)} \right|$$H₂(g, 1 bar)$$\left| {HCl\left( {aq} \right)} \right|$$AgCl$$\left| {\left( s \right)} \right|$$Ag(s)|Pt(s)

the cell potential is 0.92 V when a 10^–6 molal HCl solution is used. The standard electrode potential of (AgCl/ AgCl^– ) electrode is :
$$\left\{ {} \right.$$Given, $${{2.303RT} \over F} = 0.06V$$ at $$\left. {298} \right\}$$

0.94 V

0.40 V

0.76 V

0.20 V

JEE Main 2019 (Online) 10th January Morning Slot

MCQ (Single Correct Answer)

-1

Consider the following reduction processes :
Zn²⁺ + 2e^– $$ \to $$ Zn(s) ; E^o = – 0.76 V
Ca²⁺ + 2e^– $$ \to $$ Ca(s); E^o = –2.87 V
Mg²⁺ + 2e^– $$ \to $$ Mg(s) ; E^o = – 2.36 V
Ni² + 2e^– $$ \to $$ Ni(s) ; E^o = – 0.25
The reducing power of the metals increases in the order :

Ca < Mg < Zn < Ni

Ni < Zn < Mg < Ca

Zn < Mg < Ni < Ca

Ca < Zn < Mg < Ni

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