Lead in the water pipe surface have two oxidation states (as PbO and PbO₂). PbO can transform into dissolved species in the drinking water, so that a strong oxidizing agent (free chlorine, Cl₂) is used to prevent this process by further oxidizing PbO into the non-soluble species, PbO₂. Balance the net chemical reaction below. Show your process. PbO + Cl₂ + H₂O PbO₂ + H+ + CI

novel process for obtaining magnesium from sea water involves several reactions. Write a balanced chemical equation for each step of the process. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.)   In the third step, calcium hydroxide (mixed with seawater) reacts with dissolved magnesium chloride to yield solid magnesium hydroxide and aqueous calcium chloride.     In the fourth step, solid magnesium hydroxide is added to an aqueous hydrochloric acid solution, producing dissolved magnesium chloride and liquid water.       magnesium chloride is melted and this liquid is electrolyzed to yield liquid magnesium metal and diatomic chlorine gas.

1) The question screenshot has been attached down below answer ques 8 a, b step-by-step.

Balance the following reaction in acidic solution. Cr2O, (ag) + HNO,(aq) → Cr* (aq) + NO, (aq) 3 Fill in the coefficients for the balanced overall equation. HNO, + -- v H* + -v Cr.O,* → -- ♥ NO, +- Cr3+ + Cr,O, - H.O --V

Classify each of these reactions. Ba(CIO,),(s) → BaCl,(s) + 3 O,(g) 2 NaCl(aq) + K,S(aq) → Na, S(aq) + 2 KCI(aq) acid-base neutralization acid-base neutralization O precipitation O precipitation redox redox none of the above none of the above CaO(s) + CO,(g) –→ CaCO;(s) KOH(aq) + AgNO,(aq) → KNO, (aq) + AgOH(s) acid-base neutralization acid-base neutralization O precipitation O precipitation redox redox none of the above none of the above Ba(OH), (aq) + 2 HNO, (aq) → Ba(NO,),(aq) + 2 H,O(1) acid-base neutralization precipitation redox none of the above

Write the equation for the dissolving of iron(II) hydroxide in water. Be sure to specify the state of each reactant and product. +

Enter a molecular equation for the reaction of dilute sulfuric acid with iron. (Assume that sulfuric acid acts as a diprotic acid and that an iron(II) compound is formed.) Express your answer as a balanced chemical equation. Identify all of the phases in your answer.   Enter a molecular equation for the reaction of hydrobromic acid with magnesium. Express your answer as a balanced chemical equation. Identify all of the phases in your answer.   Enter a molecular equation for the reaction of acetic acid, CH3COOHCH3COOH, with zinc. Express your answer as a balanced chemical equation. Identify all of the phases in your answer.

Consider the following redox reaction: 3Ag+ (aq) + Al(s) → 3Ag (s) + A1³+ (aq) If this reaction starts with 2.50 g of Al and the enough amount of Ag+, how much of electric charge could be generated? 4.28 x 104 C 8.94 × 10³ C 2.68 × 104 C 6.25 × 10³ C O 1.67 x 104 C

Balance the following reaction in basic solution. Ag(s) + Zn (aq) 21 Ag,O(aq) + Zn(s) Fill in the coefficients for the balanced overall equation. Ag + Zn2- OH vZn + Ag, 0 + H,O

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