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(a)
Interpretation:
The given redox chemical equation in acidic medium should be balanced.
Concept Introduction:
A redox reaction is a
Oxidation state or oxidation number of an atom is defined as the positive or the negative charge that an atom would possess if it is present as ions in the given compound. In such type of reaction, the oxidation state of the atom undergoing oxidation will increase which depends upon the number of electrons lost by a particular atom. Reduction of a chemical species refers to the gain of electrons by the chemical species which results in decrease in oxidation state of that atom.
(b)
Interpretation:
The given redox chemical equation in acidic medium should be balanced.
Concept Introduction:
A redox reaction is a chemical reaction in which oxidation and reduction reactions takes place simultaneously. In such type of reaction one of the chemical species is getting oxidized while the other species gets reduced at the same time.
Oxidation state or oxidation number of an atom is defined as the positive or the negative charge that an atom would possess if it is present as ions in the given compound. In such type of reaction, the oxidation state of the atom undergoing oxidation will increase which depends upon the number of electrons lost by a particular atom. Reduction of a chemical species refers to the gain of electrons by the chemical species which results in decrease in oxidation state of that atom.
(c)
Interpretation:
The given redox chemical equation in acidic medium should be balanced.
Concept Introduction:
A redox reaction is a chemical reaction in which oxidation and reduction reactions takes place simultaneously. In such type of reaction one of the chemical species is getting oxidized while the other species gets reduced at the same time.
Oxidation state or oxidation number of an atom is defined as the positive or the negative charge that an atom would possess if it is present as ions in the given compound. In such type of reaction, the oxidation state of the atom undergoing oxidation will increase which depends upon the number of electrons lost by a particular atom. Reduction of a chemical species refers to the gain of electrons by the chemical species which results in decrease in oxidation state of that atom.
(c)
Interpretation:
The given redox chemical equation in acidic medium should be balanced.
Concept Introduction:
A redox reaction is a chemical reaction in which oxidation and reduction reactions takes place simultaneously. In such type of reaction one of the chemical species is getting oxidized while the other species gets reduced at the same time.
Oxidation state or oxidation number of an atom is defined as the positive or the negative charge that an atom would possess if it is present as ions in the given compound. In such type of reaction, the oxidation state of the atom undergoing oxidation will increase which depends upon the number of electrons lost by a particular atom. Reduction of a chemical species refers to the gain of electrons by the chemical species which results in decrease in oxidation state of that atom.
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Chapter 15 Solutions
Basic Chemistry
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- Question 10 of 25 Complete and balance the following redox reaction in acidic solution NO2(g) → NO3 (aq) + NO(g) 04- O+ 2+ 3+ O4+ 1 4 6. 7 9. O2 3 4 O5 O6 07 O8 O9 (s) (1) (g) (aq) H e N H* OH H2O H30* Reset x H2O Delete MacBook Pro 80 000 DII DD F2 F3 F4 F5 F6 F7 F8 F9 F10 %23 %24 3 5 3. 2.arrow_forwardComplete and balance the following redox reaction in basic solution Zn(s) + 4 OH (aq) Zn(OH), +2 e 04- 02 04+ 1 4. 6. 8 9. 02 (s) (1) (g) (aq) H* H30* e Zn H H20 OH Reset • z H20 Delete 7. LO 3. question 9arrow_forward(5.9: Similar to For Practice 5.15) Identify the oxidizing agent in the reaction below. Mg(s) + 2HCl(aq) --> MgCl2(aq) + H2(g) O Mg O H₂ OHCI This is not a redox reaction. < Previousarrow_forward
- 9. 8. m Balance the following redox reaction in basic solution. Mn0,(s)+Br,(1) MnO,(aq)+Br (aq) Mno, (s) + Br, (1) - Mno, (aq) + Br (aq) 00arrow_forward(7.1a) Complete and balance the following by ion-electron method. Reactions are taking place in acidic solution. a) Cu(s) + NO3 (aq) - Cu*taq) + NO2(g Analysis: Oxidation-Half reation: Balancing atoms & charges: Cu(s) Cu(aq) * e Reduction-Half reation: Balancing 0 & H and charges: H* + NO3 (aq) + e - NO2(g) H20 Balancing electrons lost & gained and balancing the equation: Cus) NO3 (aq) * H* - Cu(aq) NO2(g) H20arrow_forwardConsider the unbalanced reaction below occurring in acidic solution: PbO₂ (s) + (aq) Pb2+ (aq) + 1₂(5) Which of the following reactions is the properly balanced net redox reaction? O PbO₂(s) + 21-(aq) + 4H*(aq) O PbO₂(s) +41-(aq) + 4H*(aq) O PbO₂(s) +1-(aq) + 2H*(aq) - O PbO₂(s) + 21-(aq) - 1 Pb2+ (aq) + 12(s) + 2H₂O() Pb2+ (aq) +212(s) + 2H₂O() Pb2+ (aq) + 1₂(s) + H₂O() Pb2+ (aq) + 1₂(s) + O₂(g)arrow_forward
- Complete and balance the following redox reaction in acidic solution Mn2 (aq) + BiO3 (aq) → MnO4 (aq) + Bi³" (aq) 14- 3- 2- D2+ 03+ 04+ 2 3 1 6. 7 8 9. 4 Os 15 6. 7 8. (s) (1) (g) (aq) Bi H3O Mn e H2O OH 1L 2.arrow_forward(4: 5 pts) Balance the following redox reaction in basic conditions. Show your work clearly and circle the two balanced half reactions and indicate which is a reduction and which is an oxidation. Fe2+(aq) + MnO4-(aq) = Fe3+ (aq) + Mn2+(aq)arrow_forwardComplete and balance the following redox reaction in acidic solution Mn2* (aq) + BiO3 (aq) MnO, (aq) + Bia* (aq) 3. 2. 3+ O4+ 04- 6. 8 9. 1 O2 03 O5 O6 17 O8 O9 (s) (1) (g) (aq) 1) Mn OH Bi e H3O* H20 H* Delete 5 4.arrow_forward
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