4. Reducing agent is a substance which itself gets oxidized (gains oxygen, loses hydrogen or loses electrons) in the reaction. We can observe that C4H10(g) gets oxidized to H6C4O4 (as it gains oxygen as well as loses H). So it is the reducing agent, so option (a) is correct.
Cr2O72- loses oxygen to form Cr3+ so it is not the reducing agent, rather it is the oxidizing agent i.e. the substance which itself gets reduced (loses oxygen or gains electrons)
To understand the case of H+going to form H2O we have to see it from the point of view of oxidation state. H has +1 oxidation state in H+ and in H2O, O has -2 oxidation state and to balance it each of the two H has +1 oxidation state. So it is H+ is neither oxidized nor reduced.
Consider the redox equation below, C4HI0(g)+CreO72-(ag) + H-(aq) H&C4O4(ag) +Cr3-(aq) + H2O() The reducing agent is...
QUESTION 9 In the following redox reaction, what is the reducing agent? H20(1) + 3CH3OH(aq) + Cr2O72-(aq) — 3CH20(aq) + 2Cr3+(aq) + 8OH"(aq) O H₂O (1) CH3OH (aq) Cr2072- (aq) o cr2 O Cr3+(aq)
Consider a voltaic cell that operates from the following redox reaction: Cr2+ (aq) + Ag+ (aq) → Cr3+ (aq) + Ag (s) What is the value of Eocell if Eored(Ag1+/Ag) = 0.80 V and Eored(Cr3+/ Cr2+) = -0.41 V? Question options: A) Eocell = 0.39 V C) Eocell = -1.21 V D) Eocell = -0.39 V E) Eocell = 1.21 V
[References] Sc(s) + 3Ag+ (aq) + 3 Ag(s) + Sc3+ (aq) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced CE SC HBr(9) + NH3(g) + NH4Br(s) Redox? Oxidizing Agent in Reducing Agent Substance Oxidized Substance Reduced GeCl4 (1) + 2H2O(l) + 4HCl(aq) + GeO2 (s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced d. Si C14 (1) + 2Ba(s) + 2BaCl2(8) + Si(s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced Yes 2 SiBr, Ba SiBa Al(OH).-...
What substance is the reducing agent in the following redox reaction? H+(aq) + Mn(s) + NO3-(aq) → Mn2+(aq) + NO(aq) + H2O(l) Mn NO3- Mn2+ none of the above NO
5. Consider the following redox molecular reaction: Na(s) + H2O(l) ? NaOH(aq) + H2(g) If water is written as HOH(), then the equation is Na(s) + HOH(l) ? NaOH(aq) + H2(g) Write the following reactions: Oxidation reaction: Reduction reaction: Balanced net ionic reaction: Reducing agent: Oxidizing agent:
Rank the following in order of strength as a reducing agent. EM Ag (aq) +e-Ag(s) +0.80 Alaq) + 3e-4Alls) 1.66 Aul(aq) + 3e- 4 Au(s) +1.50 Co2(aq) + 2e- 4 Co(s) -0.28 Cr2(aq) + 2e-4Cr(s) -0.91 Ni2(aq) + 2e-4Nils) -0.25 P2*(aq) + 2e- A Pt(s) +1.19 Sn2(aq) + 2e-4Sn(s) -0.14 Ag [Choose) ΑΙ (Choose) Со [Choose)
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4. Consider the following unbalanced net redox equation: HCI + KMnO, (aq) + H,02 (aq) -. MnC12 (aq) + O2 (g) + KCI in an acid solution a. Determine the oxidation state of each atom or ion in the above reaction: b. Which atom is being oxidized? Which atom is being reduced? C. Which species is the reducing agent? Which is the oxidizing agent? d. Write the net...
Consider the following half-reactions.Which of these is the strongest reducing agent listed here? Au (aq) +eAu(s) E 1.69 V N20(g) +2H+(aa) +2e N2/g)+H200 EO - 1.77 V Cr3t(ag) +3 e Cris) Eo0.74 V Selected Answer: 5. Cr3(aa) Correct Answer: 6. Cr(s)
a Cu(s) + 2Ag+ (aq) → 2 Ag(s) + Cu2+ (aq) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced b HCl(g) + NH3 (g) → NH4Cl(s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced c SiCl4 (l) + 2H2O(l) → 4HCl(aq) + SiO2 (s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced d C14 (1) + 2Mg(s) + 2MgCl2(8) + Si(s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced e Al(OH)4-(aq) → AIO2- (aq) + 2H2O(l) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced
QUESTION 1 In the redox reaction: Zn(s) + H2SO4(aq) → Zn2SO4(aq) + H2(g), the reducing agent is O H2S04 O Zn2804 O H2 Ozn OH+