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Which of the following reactions canot b...

Which of the following reactions canot be a base for electrochemical cell?

A

`H_2+O_2 to H_2O`

B

`AgNO_3 + Zn to Zn(NO_3)_2 + Ag`

C

`AgNO_3 + NaCl to AgCl darr + NaNO_3`

D

`KMnO_4 + FeSO_4 + H_2SO_4 to K_2SO_4 + Fe_2(SO_4)_3 + MnSO_4 + H_2O`

Text Solution

AI Generated Solution

The correct Answer is:
To determine which of the given reactions cannot serve as a basis for an electrochemical cell, we need to identify whether each reaction is a redox reaction. A redox reaction involves the simultaneous oxidation and reduction of substances. Let's analyze each option step by step. ### Step 1: Analyze the First Reaction **Reaction:** H₂ + O₂ → H₂O - **Oxidation States:** - H₂: 0 (elemental form) - O₂: 0 (elemental form) - H₂O: H = +1, O = -2 - **Changes:** - H goes from 0 to +1 (oxidation) - O goes from 0 to -2 (reduction) **Conclusion:** This is a redox reaction. ### Step 2: Analyze the Second Reaction **Reaction:** AgNO₃ + Zn → Zn(NO₃)₂ + Ag - **Oxidation States:** - Ag in AgNO₃: +1 - Zn: 0 - Zn(NO₃)₂: Zn = +2, Ag = 0 - **Changes:** - Ag goes from +1 to 0 (reduction) - Zn goes from 0 to +2 (oxidation) **Conclusion:** This is also a redox reaction. ### Step 3: Analyze the Third Reaction **Reaction:** AgNO₃ + NaCl → AgCl + NaNO₃ - **Oxidation States:** - Ag in AgNO₃: +1 - Na in NaCl: +1 - AgCl: Ag = +1, NaNO₃: Na = +1 - **Changes:** - There is no change in the oxidation states of Ag and Na. **Conclusion:** This is NOT a redox reaction. ### Step 4: Analyze the Fourth Reaction **Reaction:** KMnO₄ + FeSO₄ + H₂SO₄ → K₂SO₄ + Fe₂(SO₄)₃ + MnSO₄ + H₂SO₄ - **Oxidation States:** - Mn in KMnO₄: +7 - Fe in FeSO₄: +2 - K₂SO₄: K = +1, Fe₂(SO₄)₃: Fe = +3, MnSO₄: Mn = +2 - **Changes:** - Mn goes from +7 to +2 (reduction) - Fe goes from +2 to +3 (oxidation) **Conclusion:** This is a redox reaction. ### Final Conclusion Among the reactions analyzed: - **First Reaction:** Redox reaction - **Second Reaction:** Redox reaction - **Third Reaction:** NOT a redox reaction (cannot be a basis for an electrochemical cell) - **Fourth Reaction:** Redox reaction Thus, the reaction that cannot serve as a basis for an electrochemical cell is the **third reaction (AgNO₃ + NaCl → AgCl + NaNO₃)**. ### Answer: **The reaction that cannot be a base for an electrochemical cell is the third reaction (AgNO₃ + NaCl → AgCl + NaNO₃).** ---

To determine which of the given reactions cannot serve as a basis for an electrochemical cell, we need to identify whether each reaction is a redox reaction. A redox reaction involves the simultaneous oxidation and reduction of substances. Let's analyze each option step by step. ### Step 1: Analyze the First Reaction **Reaction:** H₂ + O₂ → H₂O - **Oxidation States:** - H₂: 0 (elemental form) - O₂: 0 (elemental form) ...
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  • Which of the following is not an application of electrochemical series?

    A
    To compare the relative oxidising and reducing power of substances.
    B
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    C
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    D
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