How could you distinguish sodium chloride (table salt) from sodium iodide (a poison)? ° 1. Use AgNO3(aq) solution: forming Agl(s) (white), turns purple in light; or forming AgCl(s) (yellow). 2. Use concentrated H2SO4(1) on solid: iodide ion forms HI(g), a pungent gas; chloride ion forms dark solid and purple vapors appear. 1. Use AgNO3(aq) solution: forming AgCl(s) (white), turns purple in light; or forming Agl(s) (yellow). 2. Use concentrated H2SO4(1) on solid: iodide ion forms HI(g), a pungent gas; chloride ion forms dark solid and purple vapors appear. 1. Use AgNO3(aq) solution: forming AgCl(s) (white), turns purple in light; or forming Agl(s) (yellow). 2. Use concentrated H2SO4(1) on solid: chloride ion forms HCl(g), a pungent gas; iodide ion forms dark solid and purple vapors appear. 1. Use AgNO3(aq) solution: forming Agl(s) (white), turns purple in light; or forming AgCl(s) (yellow). 2. Use concentrated H2SO4(1) on solid: chloride ion forms HCI, a pungent gas; iodide ion forms dark solid and purple vapors appear.

What is Hrxn for reaction of iron(III) oxide and carbon monoxide to give iron metal and carbon dioxide gas? Use the following reactions: 4Fe(s)+3O2(g)2Fe2O3(s)H=1648.4kJ4CO(g)+O2(g)2CO3(g)H=565.98kJ

According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?

Three reactions very important to the semiconductor industry are The reduction of silicon dioxide to crude silicon, SiO2(s) + 2 C(s) → Si(s) + 2 CO(g) ΔrH° = 689.9 kJ/mol The formation of silicon tetrachloride from crude silicon, Si(s) + 2 Cl2(g) → SiCl4(g) ΔrH° = −657.01 kJ/mol The reduction of silicon tetrachloride to pure silicon with magnesium, SiCl4(g) + 2 Mg(s) → 2 MgCl2(s) + Si(s) ΔrH° = −625.6 kJ/mol Calculate the overall enthalpy change when 1.00 mol sand, SiO2, changes into very pure silicon by this series of reactions.

Equal amounts of two acids - HCl and CH3CO OH (acetic acid) - are placed in aqueous solution. When equilibrium is achieved, the HCI solution has a much greater conductivity than the acetic acid solution. Which reactions is more product-favored at equilibrium? Explain your answer in terms of your understanding of electrolytes.

B. 3CO+Fe,O,→ 2Fe + 3CO, Not balanced SO, + 2NaOH → Na SO+ 2H O balunred Evaluate a Chemical Equation The photo shows that when a clear colorless solution of lead nitrate Is added to a clear, colorless solution of sodium iodide, a yelloW solid, lead iodide, forms. lead nitrate + sodium jodide > lead jodide + sodium nitrate (solution) Pb(NO,), (solution) NaNO, (solution) (solid) Nal -> Pbl, 26. Explain how the equation shown is not currently a balanced equation. Include conservation of matter in your explanation. A student proposed that the balanced chemical equation for t Pb(NO,), + 2Nal > Pbl, + 2NaNO, Determine whether this is a correctly balanced equation and for your concluusion

Given this: 1. Aluminum metal reacts with water to produce hydrogen gas and aluminum hydroxide, which is a white, insoluble salt. It may appear grey if the aluminum foil contains black impurities. 2. Aluminum hydroxide reacts with potassium hydroxide to produce soluble potassium ions and aluminate ions Al(OH)4 -  3. Aluminate ions combine with sulfuric acid to produce aluminum hydroxide again, soluble (SO4)2- ions, and water. It should look like a white precipitate at this point. 4. As more sulfuric acid is added, aluminum hydroxide further reacts to produce soluble Al3+ and (SO4)2- ions and water. 5. Alum KAl(SO4)2·12H2O crystallizes out when water is cooled enough to cause the soluble ions (of which alum is made) to coalesce and precipitate out of the solution. Write five balanced equations which correspond to the four intermediate reaction steps and the final crystallization step in the synthesis of Alum from aluminum. Note: Use only those products from one equation that actually…

Given the following exothermic reaction : Fe3+(aq)+SCN-(aq) <-> FeSCN2+(a1), what will cause the formation of additional FeSCN2+(aq)? Adding heat or Adding Fe(No3)3(aq)? both?

Sodium hydrogen carbonate (NaHCO3), also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid (HCl), which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl (aq)+ NaHCO3 (aq) → NaCl (aq) + H2O (l) + CO2 (g) The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 50.mL of a 0.054 M HCl solution. What mass of NaHCO3 would he need to ingest to neutralize this much HCl? Be sure your answer has the correct number of significant digits.

Sodium hydrogen carbonate (NaHCO3), also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid (HCI), which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl(aq) + NaHCO3(aq) → NaCl(aq) + H2O(l) + CO₂(9) The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 50. mL of a 0.035 M HCl solution. What mass of NaHCO3 would he need to ingest to neutralize this much HCI? Be sure your answer has the correct number of significant digits.