2. Half Re...2reqUse standard reduction potentials to calculate the standard free3. Combini...energy change in kJ for the reaction:2req4. Full Re...2reqCu2*(aq) + Fe(s)→ Cu(s) +Fe2+(aq)5. Reducti...2reqAnswer:kJ6. Calculat...2reqK for this reaction would bethan one.QuestionQuestionSubmit AnswerRetry Entire GroupQuestion2req9 more group attempts remaining7. Relation...8. Calculat...2req9. Calculat..2req

By using standard reduction potential E° cell calculated ,than standard free energy change…

lalf Re... 2req Use standard reduction potentials to calculate the standard free Combini... 2req energy change in kJ for the reaction: ull Re... 2req Cu2*(aq) + Fe(s)→ Cu(s) + Fe²+(aq) Reducti... 2req Answer: kJ Calculat... 2req K for this reaction would be than one. uestion uestion uestion Submit Answer Retry Entire Group Eelation... 2req 9 more group attempts remaining Calculat... 2req Calculat 2reg

lalf Re... 2req Use standard reduction potentials to calculate the standard free Combini... 2req energy change in kJ for the reaction: ull Re... 2req Cu2*(aq) + Fe(s)→ Cu(s) + Fe²+(aq) Reducti... 2req Answer: kJ Calculat... 2req K for this reaction would be than one. uestion uestion uestion Submit Answer Retry Entire Group Eelation... 2req 9 more group attempts remaining Calculat... 2req Calculat 2reg

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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please explaine why thoses are the answers, show work neatly!!!!!!!! please and thank you Reduction Potentials Half-reaction E° (V) -0.74 Cr3+ (aq) + 3e-- Cr (s) Fe2+ (aq) + 2e-Fe (s) -0.440 Fe3+ (aq) +-- Fe2+ (s) +0.771 Sn4+ (aq) + 2e- Sn2+ (aq) +0.154 9) The standard cell potential (Eºcell) for the voltaic cell based on the reaction below is 3Sn4+ (aq) + 2Cr (s)- 2Cr³+ (aq) + 3Sn2+ (aq) B) +2.53 C) +1.94 A) -0.59 0.74 +0.154 2Cr (s) + 3Fe2+ (aq) - 3Fe (s) + 2Cr³+ (aq) B) +0.83 C) +3.10 A) +2.80 0.894 v D) +0.89 = 06" -ntc²=-2011" 10) The standard cell potential (Eºcell) for the voltaic cell based on the reaction below is 0.74 +0.440 D) +0.30 E) -1.02 V. E) -0.16 V. 9) 10)
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction:2Ag+(aq) + Ni(s)2Ag(s) + Ni2+(aq)Answer: kJK for this reaction would be (greater/ less) than one.
Use standard reduction potentials to calculate the equilibrium constant for the reaction:Fe2+(aq) + 2Fe2+(aq)--->Fe(s) + 2Fe3+(aq)Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm.Equilibrium constant: ____G° for this reaction would be (greater/ less) than zero.
Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr2+]=0.805 M and [Sn2+]=0.0110 MCr(s)+Sn2+(aq)↽−−⇀ Cr2+(aq)+Sn(s)Use the standard reduction potentials (E) and natural log in the Nernet equation and show work so I can apply the info to other problems. Thank you.E for Cr 2+ = -0.805 E for Sn2+=-0.11
Given the half-reactions and their respective standard reduction potentials 1. Cu³+ + 2 e- + Cu+ E; = +1.28 V Cu²+ + e E; = +0.15 V E; = = +0.52 V 2. + Cu+ 3. Cu²+ + 2 e- → Cu(s) = +0.34 V 4. Cu* + e- Cu(s) E calculate the standard reduction potential for the reduction half-reaction of Cu(III) to Cu(II). Cu³+ + e Cu2+ E° = V
A river pollutant is found to have a concentration of 0.0031 % m/v. If the density of the river water is 1.183 g/ml, what is the concentration of the pollutant in ppm? Proper rounding of your answer is required.
6. Consider the following galvanic cell: Ag- shown: 1.00 M Ag 1.00 M Cd2+ A 15.0-mole sample of NH3 is added to the Ag compartment (assume 1.00 L of total solution after the addition). The silver ion reacts with ammonia to form complex ions as Ag+ (aq) + NH3(aq) AgNH3+ (aq) K₁ 2.1 x 10³ = AgNH3+ (aq) + NH3(aq) ⇒ Ag(NH3)2+(aq) K₂ = 8.2 x 10³ Calculate the cell potential after the addition of 15.0 moles of NH3.
For the cell diagram below, what is the equilibrium constant K for the reaction at 25 °C? * Pt(s) | [Fe(bpy),2*(aq), [Fe(bpy),]3"(aq) || S,0, (aq), So,2 (aq) | Pt(s) E° ([Fe(bpy),]3*/[Fe(bpy);]*) = +1.12 V E° (S,0, /SO,2) = +2.01 V O 8.54 x 1018 O 8.93 x 107 O 1.22 x 1030 O insufficient data
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction:Cu2+(aq) + Cr2+(aq) Cu+(aq) + Cr3+(aq)Answer: kJK for this reaction would be than one.
4. The possible galvanic corrosion between zinc and chromium is Cre) | Cr* (ag) || Zn²* (aq) | Zne) Note: Cr* (aq) + 2e → Cris) E° = - 0.910 V Oxidation Zn" (ag) + 2e → Zn(s) E° = - 0.763 V Reduction a) What is the chemical reaction that takes place? Spontaneous or non- spontaneous. b) What is the standard free energy change for that reaction?
ng and lea X + takeCovalentActivity.do?locator=assignment-take [Review Topics] [References] Use the References to access important values if needed for this question. Use the standard reduction potentials located in the 'Tables' linked above to calculate the standard free energy change in kJ for the reaction: Zn²+ (aq) + Co(s) → Zn(s) + Co²+ (aq) Answer: K for this reaction would be v than one. greater less Submit Answer Retry Entir 2 more group attempts remaining Previous Next Save and Exit Cengage Learning | Cengage Technical Support 10:28 PM A Rain.. 五 4/16/2022 ON F7 F10 F11 F12 Insert PrtSc Delete Home IDO 同回 * + Num Backspace
Consider the following reaction at 298K. Fe2+ (aq) + 2 Cu* (aq) - Fe (s) + 2 Cu2+ (aq) Which of the following statements are correct? Choose all that apply. Odelta G° <0 ☐ E° cell <0 On = 2 mol electrons OK<1 The reaction is product-favored.