4. Calculate E' and E for each of the following redox reactions at 25.0°C.3Cu²"(aq) + Cr(s) → 3Cr*(aq) + Cr³*(aq)[Cu²*] = 4.50 M[Cu*] = 0.250 M[C**] = 0.125 MHalf ReactionE(V)Cu²"(aq) + e → Cu*(aq)Cr3*(aq) + 3e → Cr(s)+0.15-0.74

Given redox reaction 3Cu2+(aq) + Cr(s) -------> 3Cu+(aq) + Cr3+(aq) In this oxidation state of…

4. Calculate E and E for each of the following redox reactions at 25.0°C. 3Cu2"(aq) + Cr(s) → 3Cr*(aq) + Cr³*(aq) [Cu²*] = 4.50 M [Cu*] = 0.250 M [Cr**] = 0.125 M %3D Half Reaction E(V) Cu²"(aq) + e → Cu*(aq) Cr3*(aq) + 3e¯ → Cr(s) +0.15 -0.74

4. Calculate E and E for each of the following redox reactions at 25.0°C. 3Cu2"(aq) + Cr(s) → 3Cr(aq) + Cr³(aq) [Cu²] = 4.50 M [Cu] = 0.250 M [Cr**] = 0.125 M %3D Half Reaction E(V) Cu²"(aq) + e → Cu(aq) Cr3(aq) + 3e¯ → Cr(s) +0.15 -0.74

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...

See similar textbooks

Similar questions

Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG for the following redox reaction. Be sure your answer has the correct number of significant digits. NO(g) + H₂0 (1) + Cu (aq) → HNO₂ (aq) + H¨ (aq) + Cu (aq) 0.P X
+ 1.14 V TI Pt Cr3+ (1 M) Cr2 (1 M) T13+ (1 M) T13+ (aq) + 3e-→ TI (s) Cr2+ (aq) → Cr3+ (aq) + e- What happens to the thallium electrode as the redox reaction progresses? O it gains mass as thallium metal is plated onto the electrode O it loses mass as the thallium metal is consumed by the reaction O it spontaneously ignites and burns O the thallium electrode is inert and unaffected by the redox reaction O a thick layer of thallium salt develops on the clectrode DELL
Balance the following reaction in acidic solution. Fe?+ (ag) + MnO, (aq) → Fe+ (ag) + Mn²+(aq) Fill in the coefficients and substances for the balanced overall equation. Note: Do NOT leave any coeffient fields empty. If the coefficient is 1, choose "1" as opposed to leaving it blank. Fe2+ + MnO,¯ + 4 Fe3+ + Mn2+ +
Complete and balance the following redox reaction in basic solution. Be sure to include the proper phases for all species within the reaction. Cr:O,2 (aq) + Hg(1) → Hg² (aq) + Cr* (aq) 74- ]3- D2- O3+ 14+ 1 2 4 6. 7 8 9. D4 Os Os Do (s) (1) (g) (aq) + H H3O+ Cr H2O e OH- H+ Hg Reset • x H2O Delete 1L
Complete and balance the following redox reaction in acidic solution. Be sure to include the proper phases for all species within the reaction. MnO4 (aq) + S₂O3²¯(aq) → S4O6²¯(aq) + Mn²+ (aq) 1 1 + 04- e 2 Reset OH- ñ 4 3 4 ( ) 3 4 5 H+ 5 H3O+ 12 S 口。 (s) ²+ 7 H Mn 7 3+ ∞ 4+ • x H₂O 9 (1) (g) 口口。 O (aq) H₂O Delete
7. Please answer the following questions. (a) Given the following reduction potentials Cd (OH)2 (s) + 2e → Cd (s) + 2 OH (aq) Eºred = -0.76 V NIO(OH) (s) + H₂O (1) + e → Ni(OH)2 (aq) + OH (aq) Eºred = +0.49 V Calculate the standard emf of the nickel-cadmium (nicad) rechargeable battery. *hint: the reaction for the discharge of nicad battery is: Cd (s) + 2 NIO(OH) (s) + 2 H₂O (1)→ 2Ni(OH)2 (aq) + Cd(OH)2 (s) (b) A typical nicad voltaic cell generates an emf of +1.30 V. Why is there a difference between this value and the one you calculated in part (b)? (c) Calculate the equilibrium constant for the overall nicad reaction based on this typical emf value.
Answer the four questions below related to the spontaneous redox reaction that occurs whenCr(OH)3(s) reacts with NO3–(aq) to produce CrO42–(aq)and NO2–(aq) under basic conditions. Write the balanced net ionic equation, including states of matter, for the overall reaction.
In the balanced redox reaction: 2 Cu(s) + S(s) > Cu 2S(s); how many electrons are gained or lost by each copper atom?
The following skeletal oxidation-reduction reaction occurs under acidic conditions. Write the balanced OXIDATION half reaction. Mn2+ + Cr»Cr* + Mn
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: Cu²+ (aq) + 2Cu+ (aq) → Cu(s) + 2Cu²+ (aq) 2+ Cu²+ (aq) + 2e → Cu(s) Ee = 0.337 V red 0.153 V = 2+ Cu²+ (aq) +e → Cut (aq) E red AG° kJ K for this reaction would be than one.
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2H+ (aq) + Hg(1)→ H₂(g) + Hg²+ (aq) 2H+ (aq) + 2e¯ → H₂(g) Fº red 2+ Hg2 (aq) + 2e¯ → Hg(1) AGO = || kJ K for this reaction would be Eº red = 0.000 V = = 0.855 V than one.