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Concept explainers
(a)
Interpretation:
The gain of electrons needs to be classified as oxidation or reduction.
Concept Introduction :
In a redox
(b)
Interpretation:
The reaction of a reducing agent needs to be classified as oxidation or reduction.
Concept Introduction :
In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, one of the reactants get oxidized and 1 gets reduced, this is known as a redox reaction. The species that reduces others and itself gets oxidized is known as a reducing agent.
(c)
Interpretation:
The given reaction needs to be classified as oxidation or reduction:
Concept Introduction :
In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. When in a reaction, 1 of the reactants get oxidized and 1 gets reduced, this is known as a redox reaction.
(d)
Interpretation:
The given reaction needs to be classified as oxidation or reduction:
Concept Introduction :
In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, one of the reactants get oxidized and 1 gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.
(e)
Interpretation:
The given reaction needs to be classified as oxidation or reduction:
Concept Introduction :
In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, one of the reactants get oxidized and one gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.
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Chapter 15 Solutions
EBK BASIC CHEMISTRY
- (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_forwardComplete and balance the following redox reaction in basic solution Zn(s) → Zn(OH),*(aq) + H,(g) 4 4- 2- D2+ 3+ 4+ + 1 2 3 4 6. 7 8 9. O3 O6 O7 (s) (1) (g) (aq) + e Zn H* OH Reset • x H,0 Delete 9. 4. 3. 2.arrow_forwardGiven the following redox pair, identify the reducing agent: NAD+/ NADH (-0.32) 2e- 202H2O (0.82) 2e- A. NADH B. NAD+ C. O₂ D. H₂Oarrow_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*2(aq) + NO2(g) + NO29) Analysis: Oxidation-Half reation: Balancing atoms & charges: Cu(s) Cu*2, (aq) e Reduction-Half reation: Balancing O & H and charges: H* + NO3 (aq) e NO2(g) + 1 H20 Balancing electrons lost & gained and balancing the equation: Cu(s) NO3 (aq) + H* - Cu*(aq) NO2(g) H20arrow_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_forwardFor each of the reaction below, identify: (0.5 marks each) substance being oxidized substance being reduced oxidizing agent reducing agent number of electrons transferred. 1. K2Cr207 + 14HCI -> 2KCI + 2CrCl + 3Cl + 7H20 2. 10 OH +4C12 + S2032 > 5H20 + 2502 + 8 CIarrow_forward
- (7: 4 pts) Balance the following redox reaction in basic conditions. Show your work for partial credit.arrow_forwardQuestion 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_forward(27) What is the value of the equilibrium constant (Keq) when the following redox reaction takes place at 727°C? Mn (s) + Sn¹+ (aq) → Mn²+ (aq) + Sn²+ (aq) (A) 2.55 x 10¹3 (B) 2.76 x 10¹8 (C) 7.62 x 1036 (D) 5.23 x 10-15 (E) 3.62 x 10-1⁹ The most convenient form of the equation for this one might not be on your note sheet. I suggest using: RT ECELL -In K nF (28) An archaeologist claims that a bone in her collection is from a saber-toothed tiger that is believed to have the carbon-1arrow_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_forwardFor cach of the following compounds, give the oxidation state of each element in the compound. 1. CoO b. HCIO NACIO C. Fe(10.) d. H,SO For the balanced chemical equation shown below, calculate the oxidation states of all the reactants and products. Identify the elements that are oxidized and reduced, and identify the oxidizers and reducers. How many electrons were transferred during the course of the reaction? CO:(g) 2F:(g) → CF(g) Ox(g)arrow_forward10) The average electrical current (I in ampere) delivered if 1.0 g of zinc were oxidized to zinc(11) in 60 second is: a) 24.6 A b) 49.2 A c) c) 11.9 Aarrow_forward
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