Question: Which of the following is an oxidation-reduction…

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Anu Bhardwaj · Accepted Answer

A redox reaction is one in which the oxidation states of atoms change. Let's analyze each option: A) C u ( s ) + 2 A g N O 3 ​ ( a q ) → 2 A g ( s ) + C u ( N O 3 ​ ) 2 ​ ( a q ) On the reactant side, Cu is in its elemental form, so its oxidation state is 0. Ag in A g N O 3 ​ is + 1 (since N O 3 ​ is - 1 ). On the product side, Ag is in its elemental form, so its oxidation state is 0. Cu in C u ( N O 3 ​ ) 2 ​ is + 2 (since two N O 3 ​ ions are − 2 total). The oxidation state of Cu changes from 0 to + 2 . This is oxidation. The oxidation state of Ag changes from + 1 to 0. This is a reduction. Since both oxidation and reduction occur, this is a redox reaction. B) H 2 ​ C O 3 ​ ( a q ) + C a ( N O 3 ​ ) 2 ​ ( a q ) → 2 H N O 3 ​ ( a q ) + C a C O 3 ​ ( s ) This is a double displacement reaction. Let's check the oxidation states: H is + 1 on both sides. C in H 2 ​ C O 3 ​ is + 4 (since 2 ( + 1 ) + C + 3 ( − 2 ) = 0 ⇒ C = + 4 ). C in C a C O 3 ​ is also + 4 (since + 2 + C + 3 ( − 2 ) = 0 ⇒ C = + 4 ). O is − 2 on both sides. Ca is + 2 on both sides. N in C a ( N O 3 ​ ) 2 ​ is + 5 (since + 2 + 2 ( N + 3 ( − 2 )) = 0 ⇒ 2 ( N − 6 ) = − 2 ⇒ N − 6 = − 1 ⇒ N = + 5 ). N in H N O 3 ​ is also + 5 (since + 1 + N + 3 ( − 2 ) = 0 ⇒ N = + 5 ). No element changes its oxidation state. This is not a redox reaction. C) A g N O 3 ​ ( a q ) + H Cl ( a q ) → A g Cl ( s ) + H N O 3 ​ ( a q ) This is a double displacement reaction (a precipitation reaction). Ag is + 1 on both sides. N is + 5 on both sides. H is + 1 on both sides. Cl is − 1 on both sides. O is − 2 on both sides. No element changes its oxidation state. This is not a redox reaction. D) B a ( C 2 ​ H 3 ​ O 2 ​ ) 2 ​ ( a q ) + N a 2 ​ S O 4 ​ ( a q ) → B a S O 4 ​ ( s ) + 2 N a C 2 ​ H 3 ​ O 2 ​ ( a q ) This is a double displacement reaction (a precipitation reaction). Ba is + 2 on both sides. The acetate ion ( C 2 ​ H 3 ​ O 2 ​ ) has a charge of − 1 and the carbon atoms' average oxidation state doesn't change. Na is + 1 on both sides. S is + 6 in both N a 2 ​ S O 4 ​ and B a S O 4 ​ . O is − 2 on both sides. No element changes its oxidation state. This is not a redox reaction. E) H Cl ( a q ) + N a O H ( a q ) → H 2 ​ O ( l ) + N a Cl ( a q ) This is an acid-base neutralization reaction. H is + 1 on both sides. Cl is − 1 on both sides. Na is + 1 on both sides. O is − 2 on both sides. No element changes its oxidation state. This is not a redox reaction. The only reaction where the oxidation states of elements change is reaction A. Copper is oxidized (oxidation state from 0 to +2), and silver is reduced (oxidation state from +1 to 0). =================================================================================================================================== Option A is correct. An oxidation-reduction (redox) reaction is a chemical reaction in which the oxidation states of atoms are changed. This involves the transfer of electrons between two species. Let's look at the oxidation states for reaction A: C u ( s ) + 2 A g N O 3 ​ ( a q ) → 2 A g ( s ) + C u ( N O 3 ​ ) 2 ​ ( a q ) Reactants: C u ( s ) : Copper is in its elemental form, so its oxidation state is 0. A g N O 3 ​ ( a q ) : The nitrate ion ( N O 3 − ​ ) has a charge of -1. To balance this, the silver ion ( A g + ) must have an oxidation state of +1. Products: A g ( s ) : Silver is in its elemental form, so its oxidation state is 0. C u ( N O 3 ​ ) 2 ​ ( a q ) : There are two nitrate ions, so the total negative charge is -2. To balance this, the copper ion ( C u 2 + ) must have an oxidation state of +2. Analysis of oxidation state changes: Copper (Cu): The oxidation state changes from 0 to +2. This is an increase in oxidation state, which is defined as oxidation . Copper loses electrons. Silver (Ag): The oxidation state changes from +1 to 0. This is a decrease in oxidation state, which is defined as reduction . Silver gains electrons. Since both oxidation and reduction occur in this reaction, it is a redox reaction. The other options (B, C, D, and E) are all double-displacement reactions (either precipitation or acid-base neutralization) where the oxidation states of all elements remain unchanged.

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Question: Which of the following is an oxidation-reduction reaction? Cu(s) + 2AgNO_3(aq) rightarrow 2Ag (s) + Cu(NO_3)_2(aq) H_2CO_3(aq) +

Anu Bhardwaj

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