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Consider the change in oxidation state of Bromine corresponding to different emf values as shown in the diagram below:

Then the species undergoing disproportionation is:-

1. | \(\text{BrO}^-_3\) | 2. | \(\text{BrO}^-_4\) |

3. | \(\text{Br}_2\) | 4. | \(\text{HBrO}\) |

Subtopic: Electrode & Electrode Potential |

60%

From NCERT

NEET - 2018

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In the electrochemical cell:

Zn|ZnSO_{4}(0.01 M) || CuSO_{4}(1.0M),Cu, the emf of this Daniel cell is E_{1}. When the concentration of ZnSO_{4} is changed to 1.0 M and that of CuSO_{4} is changed to 0.01 M, the emf changes to E_{2}. The relationship between E_{1} and E_{2} is :

( Given, $\frac{RT}{F}$= 0.059)

1. E_{1} = E_{2}

2. E_{1} < E_{2}

3. E_{1} > E_{2}

4. E_{2} = 0 $\ne $E_{1}

Subtopic: Electrode & Electrode Potential | Nernst Equation |

68%

From NCERT

NEET - 2017

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The molar conductivity of a solution of AgNO_{3} (considering the given data for this solution) at 298 K is:

(a) Concentration: 0.5 mol/dm^{3}

(b) Electrolytic conductivity: 5.76×10^{–3 }S cm^{–1}

1. | 2.88 S cm^{2}/mol |
2. | 11.52 S cm^{2}/mol |

3. | 0.086 S cm^{2/}mol |
4. | 28.8 S cm^{2}/mol |

Subtopic: Conductance & Conductivity |

84%

From NCERT

NEET - 2016

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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

Subtopic: Faraday’s Law of Electrolysis |

54%

From NCERT

NEET - 2016

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If the E°_{cell} for a given reaction has a negative value, which of the following gives correct relationships for the values of $\u2206$G° and K_{eq} ?

(1) $\u2206$G° >0; K_{eq}< 1

(2) $\u2206$G° >0; K_{eq}>1

(3) $\u2206$G° < 0; K_{eq}> 1

(4) $\u2206$G° <0; K_{eq}< 1

Subtopic: Electrolytic & Electrochemical Cell | Relation between Emf, G, Kc & pH |

68%

From NCERT

NEET - 2016

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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)

1. 6 x 10^{23}

2. 6 x 10^{20}

3. 3.75 x 10^{20}

4. 7.48 x 10^{23}

Subtopic: Faraday’s Law of Electrolysis |

77%

From NCERT

NEET - 2016

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Zinc can be coated on iron to produce galvanised iron but the reverse is not possible. It is because

(1) zinc is lighter than iron

(2) zinc has lower melting point than iron

(3) zinc has lower negative electrode potential than iron

(4) zinc has higher negative electrode potential than iron

Subtopic: Nernst Equation |

62%

From NCERT

NEET - 2016

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The molar conductivity of a 0.5 mol/dm^{3} solution of AgNO_{3} with electrolytic conductivity of 5.76 × 10^{–3 }S cm^{–}^{1} at 298 K is:

1. 11.5 S cm^{2}/mol

2. 21.5 S cm^{2}/mol

3. 31.5 S cm^{2}/mol

4. 41.5 S cm^{2}/mol

Subtopic: Conductance & Conductivity |

86%

From NCERT

NEET - 2016

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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 × 10^{–19 }C)

1. $6\times {10}^{23}$

2. $6\times {10}^{20}$

3. $3.75\times {10}^{20}$

4. $7.48\times {10}^{20}$

Subtopic: Faraday’s Law of Electrolysis |

79%

From NCERT

NEET - 2016

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The pressure of H_{2} required to make the potential of H_{2 }- electrode zero in pure water at 298 K is:

1. | 10^{–12 }atm |
2. | 10^{–10 }atm |

3. | 10^{–4 }atm |
4. | 10^{–14 }atm |

Subtopic: Nernst Equation |

66%

From NCERT

NEET - 2016

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