It was invented in 1859 by French physician Gaston Plante and still retains application today, more than 150 years later. There are two reactions that take place during discharge of the lead-acid storage battery. In one step, sulfuric acid decomposes to form sulfur trioxide and water: H₂SO4(1) SO3(9) + H₂O(1) ΔΗ=+113. In another step, lead, lead(IV) oxide, and sulfur trioxide react to form lead(II) sulfate: Pb(s) + PbO2(s) + 2 SO3(g) → 2 PbSO4(s) ΔH = -775 kJ Calculate the net change in enthalpy for the formation of one mole of lead(II) sulfate from lead, lead(IV) oxide, and sulfuric acid from these reactions. Round your answer to the nearest kJ.

Balance the equation and calculate the E∘cell of the given reaction Rb(s) + Hg2+(aq) ------> Rb+ (aq) + Hg(s)

Reaction 5a, where copper(II) sulfate reacts with solid zinc to form copper metal and zinc sulfate is best classified as Question options:   a decomposition reaction   an oxidation-reduction reaction   an acid-base reaction   a precipitation reaction

For the reaction below, determine the stoichiometric coefficient on water in the balanced redox reaction in acid solution. In compounds, the oxidation state of O is 2-. Assume X is a diatomic element and that M is a metal that can have multiple oxidation states. This question is not multiple choice, you will input the integer answer to this question.MO 4 3-(aq) + X 2+(aq) → X 3+(aq) + M 4+(aq)

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How many minutes does it take to plate 228.6 g of chromium onto a car part using 19.24 A of current? Cr²+ (aq) + 2 e¯ → Cr(s) Your Answer: Answer units

These two problems are connected and I don't know how to do these.

6. As we will discuss when we get to the chapter on electrochemistry, the AGO for a reaction can very easily be determined by incorporating the reaction into an electrochemical cell (battery). AGO is directly proportional to the potential (voltage) of the cell. Using this technique, it was found that the AG° = -1370.8 kJ for the following reaction. 2 CH₂OH(1) + 3 0₂(g) → 2 CO₂(g) + 4H₂O(1) 0. The standard entropy change (AST) for this reaction is ?163.6 J/K at 25.0 °C. A. B. C. What is the standard enthalpy of reaction, AHxn at 25.0 °C?. Please provider your answer below. ☐☐ → 0 0 0 If AHrxn and ASrxn do NOT change with temperature, what is the AGxn at 171.58 °C? Please provider your answer below. 0² 0₂ 010 H 0² 0₂ Above Please provider your answer below. °C, the reaction will become non-spontaneous? kJ kJ

+ 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

Complete and balance the following redox reaction in basic solution CIO3 (aq) + C204² (aq) → CIO2(g) + CO2(g) 14- 3- |2- O2+ 3+ 4+ 1 6. 7 8 9 0. O3 Os O, Do 12 14 7 9. (s) (1) (g) (aq) OH H2O ei H3O 4+ 2. +