When the molecular reaction between sodium silicate and copper(II) nitrite is balanced correctly the stoichiometric coefficient for sodium nitrite is _____.
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When the molecular reaction between sodium silicate and copper(II) nitrite is balanced correctly the
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- Silver tarnish is the result of the oxide on the silver surface reacting with hydrogen sulfide (H2S) in air. This leaves a black film of silver sulfide (Ag2S). Polishing the tarnished silver will restore the shine but at the expense of some of the silver metal. An alternative process is to allow aluminum to reduce the silver in the presence of a solution of sodium bicarbonate (baking sodium) electrolyte. 2. Assume that Aluminum and Silver Sulfide are the starting substances (reactants) in the reaction: A) Write a balanced chemical equation describing the ”re-creation” of silver, using the information in the case study. B) State the names of the products that are produced from this reaction. C) What type of reaction(s) is/are being represented by the chemical reaction you wrote in part (a)? D) Is the reaction in part (a) an oxidation-reduction (redox) reaction? E) If this is a redox reaction, then identify the following: What is undergoing oxidation (what is being oxidized)?…a student carries out this chemical reaction in a beaker Zn+CuCl2 -> Cu+ZnCl2 after the reaction has come to completion, what should the student expect to find in the beaker ?Write the chemical equation that describes the dissolution of alum in water and describe how many moles of aluminum and sulfate ions are produced when 1 mole of alum dissolves in sufficient water?
- Ultra-pure Si is required to produce semi-conductors. The first step in this process is combining silicon dioxide with carbon and chlorine. Choose the answer that represents the sum of all the coefficients when this equation is balanced using the smallest whole number coefficients. SiO2 + C + Cl2→ CO + SICI4 O a. 6 b. 7 О с. 16 d. 8 О е.5 ОООО СSilver tarnish is the result of the oxide on the silver surface reacting with hydrogen sulfide (H2S) in air. This leaves a black film of silver sulfide (Ag2S).Polishing the tarnished silver will restore the shine but at the expense of some of the silver metal. An alternative process is to allow aluminumto reduce the silver in the presence of a solution of sodium bicarbonate (baking sodium) electrolyte. 1. Assume that Aluminumand Silver Sulfideare the starting substances (reactants) in the reaction: a.Write a balanced chemical equation describing the ”re-creation” of silver, using the information in the case study. b.State the names of the products that are produced from this reaction. c.What type of reaction(s) is/are being represented by the chemical reaction you wrote in part (a)? d.Is the reaction in part (a) an oxidation-reduction (redox) reaction? e.If this is a redox reaction, then identify the following: What is undergoing oxidation (what is being oxidized)?…You are a budding inventor who has just manufactured their own toy rocket from scratch. As your dream is to manufacture the most realistic toy ever, you wish to create even the rocket fuel. You don’t know how long you will need to store the fuel components for, so you will leave the Ammonium perchlorate in solution form until required. This ammonium perchlorate solution is made by combining 100 mL 1.2 mol Perchloric acid (HClO4) and 100 mL 2.0 mol of Ammonia (NH3). You need to know whether this solution is acidic or basic to ensure you store it safely and properly. What is the pH of the solution you created? Full solution please
- Balance the following reaction in acidic solution. 3+ Cr20 (aq) + HNO2(aq) → Cr" (ag) + NO, (ag) 7. Fill in the coefficients for the balanced overall equation. v HNO. ΗΝΟ, Η v H* + --♥ Cr,O.² → -- v NO + -- v Cr³+ Cr3+ + HOCalculate the no. of amperes necessary to deposit 84.5 g of nickel from a solution of NiCl 3 in 45.0 min.Qu The amount of calcium carbonate with MM:100.1 g/mol in the ore dolomite can be determined by gravimetry. The dolomite sample is dissolved in acid and the calcium ions (Ca2*) present are precipitated as calcium oxalate (CaC204) with MM: 128.1 g/mol. The calcium oxalate is filtered, dried and strongly heated to form calcium oxide (Cao) with Formula Mass (FM) = 56.1 g mol". In one analysis the mass of dolomite used was 3.72 %3D g. The mass of calcium oxide formed was found to be 1.24 g. Questions: 1. What is the chemical formula of the analyte in this problem? 2. What is precipitating agent? 3. Give the molecular formula of the precipitate measured in this problem. g. 4. What is the mass(g) of the analyte? Show your answer in correct no. of SF. 5. What is the % w/w of the analyte in the sample? Give the answer in correct answer of SF. 026.9 033.3 056 060.1 02.23
- Must show workThe oxidation number of Mn in MnO₂ isPLEASE ANSWER WITH SOLUTIONS! THANK YOUUU! A sample of iron ore weighing 0.2792 g was dissolved in dilute acid solution, and all the Fe(II) was converted to Fe(III) ions, The solution required 23.30 ml of 0.0194 M KMnO4 for titration. Fill in the table below and calculate the % by mass of iron in the ore. 1. Balance the equation: Fe+2 + MnO4- ⟶ Fe+3 + MnO2 Name of Analyte Mass of analyte Name of the titrant Volume of Titrant Millequivalents of the Titrant Mass of pure analyte % Fe in analyte
