Write a balanced half-reaction describing the reduction of aqueous iron(III) cations to solid iron. 0 ローロ X 90

Write balanced half-reactions for the following redox reaction: 2 CO,(9)+12 H (aq)+12 C1¯(aq) → C,H;OH(1)+3 H,O(1)+6 Cl,(9) reduction: ローロ oxidation: U

Write the net ionic equation for the reaction between A^NO3(aq) and N22SO4(aq). Be sure to include states of matter in your answer.

Consider the following equation in aqueous solution: PO₃³⁻(aq) + SO₂(g) → PO₄³⁻(aq) + S²⁻(aq) The oxidation half-reaction is PO₃³⁻(aq) + H₂O(l) → PO₄³⁻(aq) + 2 H⁺(aq) + 2 e⁻ and the reduction half-reaction is SO₂ (g) + 4 H⁺(aq) + 6 e⁻ → S²⁻ (aq) + 2 H₂O(l). How many moles of electrons must be transferred in the overall reaction?

Balance the following redox reaction in the gas phase. Note that this reaction cannot be balanced with the half-reaction method and must be done by inspection. In the gas phase, H2 O (1) is used to balance oxygen atoms and H3 O+ and OH are not available for balancing purposes. ONLY integers should be used in your answer. NH3 (aq) + O2 (g) –→ NO2 (g) Enter your chemical notation here

Consider the reaction shown, which occurs in aqueous solutions: NO2^-1 + Al (s) --> NH3 + Al(OH)4^-1 Identify the species reduced: Identify the species oxidized: Identify the reducing agent: Identify the oxidizing agent: The balanced reduction half-reaction:  The balanced oxidation half-reaction: Overall balanced redox reaction:

What is the algebraic sum of the oxidation numbers of all the atoms in aluminium sulfate, Al2(SO4)3?

A. Balance the following redox reactions using the half-reaction method. B. Identify the oxidizing agent and the reducing agent. 1. Zn(s) + Fe²+ (aq) → Zn²+ (aq) + Fe (s) 2+ Zn(s) → Zn² +2e- oxidiation haut reaction (aq) 2+ 20+ Fe (an) → Fe (5) Reducation haut reaction (94) - Bris) Reducing agent (S) Fe 2+ oxidizing agent 2. (Balance this reaction In Acidic Solution):

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)

consider the reaction of Rubidium metal with water to form aqueous rubidium hydroxide and hydrogen gas 2Rb(s)+2H2O(l)->2RbOH(aq) assign the oxidation state for each reaction