The standard electrode potentials (reduction) of $P t / F e^{3 +}, F e^{2 +} a n d P t / S n^{4 +}, S n^{2 +} a r e + 0.77 V a n d + 0.15 V$ respectively at $25^{0} C .$ The standard EMF of the reaction $S n^{4 +} + 2 F e^{2 +} \to S n^{2 +} + 2 F e^{3 +} i s -$

(A) – 0.62 V

(B) – 0.92 V

(D) + 0.85 V

$25^{0} C पर$ $P t / F e^{2 +}, F e^{3 +} और P t / S n^{4 +}, S n^{2 +} के मानक इलेक्ट्रोड विभव (अपचयन) क्रमशः + 0.77 V और + 0.15 V हैं,$ अभिक्रिया $S n^{4 +} + 2 F e^{2 +} \to S n^{2 +} + 2 F e^{3 +}$ का मानक विद्युत वाहक बल है-

(1) – 0.62 V

(2) – 0.92 V

(3) + 0.31 V

(4) + 0.85 V

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Q93:

Acetic acid has K_a = 1.8 × 10^–5 while formic acid had K_a = 2.1 × 10^–4. What would be the magnitude of the emf of the cell

Pt(H₂) $|\begin{array}{l} 0 .1 M acetic acid + \\ 0 .1 M sodium acetate \end{array}| |\begin{array}{l} 0 .1 M formic acid + \\ 0 .1 M sodium formate \end{array}|$ Pt(H₂) at 25°C

(1) 0.0315 volt

(2) 0.0629 volt

(3) 0.0455 volt

(4) 0.0545 volt

एसीटिक अम्ल में K_a = 1.8 × 10^–5 होता हैजबकि फार्मिक अम्ल में K_a = 2.1 × 10^–4 होता है। सेल के विद्युत वाहक बल का परिमाण क्या होगा

Pt(H₂) $|\begin{array}{l} 0 .1 M एसीटिक अम्ल + \\ 0 .1 M सोडियम एसीटेट \end{array}| |\begin{array}{l} 0 .1 M फार्मिक अम्ल + \\ 0 .1 M सोडियम फार्मेट \end{array}|$ 25°C पर Pt(H₂)

(1) 0.0315 volt

(2) 0.0629 volt

(3) 0.0455 volt

(4) 0.0545 volt

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Q94:

Some half cell reaction & their standard potential are given which combination would result in a cell with the largest potential.

$(i) A + e^{-} \to A^{-} E ° = - 0.24$

$(i i) B^{-} + e^{-} \to B^{- 2} E ° = 1.25$

$(i i i) C^{-} + 2^{e -} \to C^{- 3} E^{-} = - 1.25$

$(i v) D + 2^{e -} \to D^{- 2} E ° = 0.06$

$(v) E + 4^{e -} \to E^{- 4} E ° = 0.38$

(A) i and ii

(B) ii and iii

(D) ii and v

कुछ अर्ध सेल अभिक्रिया और उनकी मानक विभव दी गयी है, जिसके संयोजन से सबसे ज्यादा विभव वाले सेल का परिणाम होगा।

$(i) A + e^{-} \to A^{-} E ° = - 0.24$

$(i i) B^{-} + e^{-} \to B^{- 2} E ° = 1.25$

$(i i i) C^{-} + 2^{e -} \to C^{- 3} E^{-} = - 1.25$

$(i v) D + 2^{e -} \to D^{- 2} E ° = 0.06$

$(v) E + 4^{e -} \to E^{- 4} E ° = 0.38$

(1) i और ii

(2) ii और iii

(3) iv और v

(4) ii और v

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Q95:

Calculate the maximum work that can be obtained from the Daniell cell given below -

$Z n (s) | Z n^{2 +} (a q) | | C u^{2 +} (a q) | C u (s) .$

Given that $E_{Z n^{2 +} / Z n}^{°} = - 0.76 V a n d E_{C u^{2 +} / C u}^{°} = + 0.34 V$

(1) – 212300 J

(2) – 202100 J

(3) – 513100 J

(4) – 232120 J

नीचे दिए गए डेनियल सेल से प्राप्त अधिकतम कार्य की गणना कीजिए-

$Z n (s) | Z n^{2 +} (a q) | | C u^{2 +} (a q) | C u (s) .$

दिया गया है कि $E_{Z n^{2 +} / Z n}^{°} = - 0.76 V और E_{C u^{2 +} / C u}^{°} = + 0.34 V$

(1) – 212300 J

(2) – 202100 J

(3) – 513100 J

(4) – 232120 J

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Q96:

Which of these ions Cu⁺, Co³⁺, Fe²⁺ is stable in aqueous medium.

Given :E°_Cu2+/Cu+ = 0.15 volt ; E°_Cu+/Cu = 0.53 V ;E°_Co3+/Co2+ = 1.82 V ;

E°_Fe3+/Fe2+ = 0.77 V ;E°_Fe2+Fe = –0.44 V ;E°_O2,H+/H2O = 1.23 V

(1) Cu⁺, Co³⁺

(2) Co³⁺

(3) Cu⁺

(4) Co³⁺, Cu⁺, Fe²⁺

इन आयनों Cu⁺, Co³⁺, Fe²⁺में से कौन जलीय माध्यम में स्थायी है।

दिया गया है: E°_Cu2+/Cu+ = 0.15 volt ; E°_Cu+/Cu = 0.53 V ;E°_{CO3 + / CO2 +}= 1.82 V;

E°_Fe3+/Fe2+ = 0.77 V ;E°_Fe2+Fe = –0.44 V ;E°_O2,H+/H2O = 1.23 V

(1) Cu⁺, Co³⁺

(2) Co³⁺

(3) Cu⁺

(4) Co³⁺, Cu⁺, Fe²⁺

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Q97:

The standard redox potentials $E^{\circ}$ of the following systems are-

System E° (volts)

$(i) M n O^{4 -} + 8 H^{+} + 5 e \to M n^{2 +} + 4 H_{2} O 1.51$

$(i i) S n^{4 +} + 2 e \to S n^{2 +} 0.15$

$(i i i) C r_{2} {O_{7}}^{2 -} + 14 H^{+} + 6 e \to 2 C r^{3 +} + 7 H_{2} O 1.33$

$(i v) C e^{4 +} + e \to C e^{3 +} 1.61$

The oxidising power of the various species decreases in the order-

1. $C e^{4 +} > C r_{2} {O_{7}}^{2 -} > S n^{4 +} > M n {O_{4}}^{-}$

2. $C e^{4 +} > M n {O_{4}}^{-} > C r_{2} {O_{7}}^{2 -} > S n^{4 +}$

3. $C r_{2} {O_{7}}^{2 -} > S n^{4 +} > C e^{4 +} + M n {O_{4}}^{-}$

4. $M n {O_{4}}^{-} > C e^{4 +} > S n^{4 +} > C r_{2} {O_{7}}^{2 -}$

निम्नलिखित निकायों में से मानक रेडॉक्स विभव $E^{\circ}$ हैं-

निकाय E° (volts)

$(i) M n O^{4 -} + 8 H^{+} + 5 e \to M n^{2 +} + 4 H_{2} O 1.51$

$(i i) S n^{4 +} + 2 e \to S n^{2 +} 0.15$

$(i i i) C r_{2} {O_{7}}^{2 -} + 14 H^{+} + 6 e \to 2 C r^{3 +} + 7 H_{2} O 1.33$

$(i v) C e^{4 +} + e \to C e^{3 +} 1.61$

विभिन्न स्पीशीज की ऑक्सीकारक क्षमता निम्न क्रम में घट जाती है-

$(1) C e^{4 +} > C r_{2} {O_{7}}^{2 -} > S n^{4 +} > M n {O_{4}}^{-}$

$(2) C e^{4 +} > M n {O_{4}}^{-} > C r_{2} {O_{7}}^{2 -} > S n^{4 +}$

$(3) C r_{2} {O_{7}}^{2 -} > S n^{4 +} > C e^{4 +} + M n {O_{4}}^{-}$

$(4) M n {O_{4}}^{-} > C e^{4 +} > S n^{4 +} > C r_{2} {O_{7}}^{2 -}$

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Q98:

The number of electrons delivered at the cathode during electrolysis by a current of 1 ampere in 60 seconds is (charge on electron = 1.60 x 10^-19 C)

(a) 6 x 10²³

(b) 6 x 10²⁰

(d) 7.48 x 10²³

60 सेकंड में 1 एम्पीयर की धारा द्वारा विद्युत अपघटन के दौरान कैथोड पर दिए गए इलेक्ट्रॉनों की संख्या होती है (इलेक्ट्रॉन पर आवेश = 1.60 x 10^-19 C)

(1) 6 x 10²³

(2) 6 x 10²⁰

(3) 3.75 x 10²⁰

(4) 7.48 x 10²³

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Q99:

The specific conductance has the unit :

(1) $o h m^{- 1} c m^{- 1}$

(2) ohm.cm

(3) $o h m c m^{- 1}$

(4) $o h m^{- 1} . c m$

विशिष्ट चालकता की इकाई होती है:

(1) $o h m^{- 1} c m^{- 1}$

(2) ohm.cm

(3) $o h m c m^{- 1}$

(4) $o h m^{- 1} . c m$

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Q100:

During the electrolysis of molten sodium chloride, the time required to produce 0.10 mol of chlorine gas using a current of 3 amperes is

(1) 55 minutes

(2) 110 minutes

(3) 220 minutes

(4) 330 minutes

गलित सोडियम क्लोराइड के विद्युतअपघटन के दौरान, 3 एम्पीयर की धारा का उपयोग करके क्लोरीन गैस का 0.10 मोल उत्पादित करने के लिए आवश्यक समय है

(1) 55 min (2) 110 min

(3) 220 min (4) 330 min

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