Complete and balance the following redox reaction in acidic solution. Be sure to include the proper phases for all species within the reaction. As(s)→ H2AsO4(aq)+AsH3(s)

Predict which species will be oxidized and which will be reduced in a molten salt mixture that contains CdI2, NaOH, and AlCI3. Cd2+(aq)  +  2e  →  Cd(s)                                        Eored = – 0.40 V I2(s)  +  2e  →  2 I–(aq)                                            Eored = + 0.54 V Na+(aq)  +  1e  →  Na(s)                                         Eored = – 2.71 V Cl2(g)  +  2e  →  2 Cl–(aq)                                       Eored = + 1.36 V Al3+(aq)  +  3e  →  Al(s)                                          Eored = – 1.66 V O2(g)  +  2 H2O(l)  +  4e  →  4 OH–(aq)                  Eored = + 0.40 V     which is oxidized    which is reduced

Balance the following reaction in basic solution. Fill in the coefficients for the balanced overall equation. Al(s) + CrO (ag) → Al(OH)3(s) + Cr(OH), (aq) → 4 4. --v H0+ -- v Al + -v " →-v Al(OH), + -- v Cr(OH), + --v OH CrO, Cr(OH), + -- v OH 4 3.

The standard free energy change for a reaction can be calculated using the equation ΔG∘′=−nFΔE∘′ where n is the number of electrons transferred, F is Faraday's constant, 96.5 kJ·mol−1·V−1, and ΔE∘′ is the difference in reduction potential. For each of the given reactions, determine the number of electrons transferred (n) and calculate standard free energy (ΔG∘′) . Consider the half-reactions and overall reaction for reaction 1. half-reactions: fumarate^2− + 2H^+ ↽−−⇀ succinate^2− CoQH2 ↽−−⇀ CoQ + 2H^+   overall reaction: fumarate^2− + CoQH2↽−−⇀succinate^2− + CoQ ΔE∘′= −0.009 V   n=____ ΔG∘′= ____ (kJ⋅mol^−1) Consider the half-reactions and overall reaction for reaction 2. half-reactions: cytochrome (c1) (Fe^2+) ↽−−⇀ cytochrome (c1) (Fe^3+) cytochrome (c) (Fe^3+) ↽−−⇀ cytochrome (c) (Fe^2+)   overall reaction: cyt (c1) (Fe^2+)+cyt (c) (Fe^3+)↽−−⇀cyt (c1) (Fe^3+)+cyt (c) (Fe^2+) ΔE∘′=0.034 V n= ____ ΔG∘′=____(kJ⋅mol^−1)

Which reaction(s) can be identified as a redox reaction? CuO(s) + H₂SO4(aq) → CuSO4(aq) + H₂O(1) Cu(NO3)2(aq) + 2NaOH(aq) -> A →→ Cu(OH)₂(s) + 2NaNO3(aq) Cu(OH)2(s) CuO(s) + H₂O(g) CuSO4(aq) +Zn(s) → ZnSO4(aq) + Cu(s) Cu(s)+ 4HNO3(aq) - Cu(NO3)2(aq) + 2NO₂(aq) + 2H₂O(1)

What products are formed when an aqueous solution of potassium iodide, KI(aq), is electrolyzed?          (A) I2 at the anode; K at the cathode.                         (B) I2 at the anode; H2 at the cathode.            (C) O2 at the anode; H2 at the cathode.                       (D) O2 at the anode; K at the cathode.

Give detailed Solution

Complete and balance the following half-reaction in acidic solution. Be sure to include the proper phases for all species within the reaction. As(s) → H₂AsO4 (aq)

Complete and balance the following redox reaction in basic solution     NO3- (aq) + AsH3 (s) --> NH3 (g) + As (s)

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.