Determine the amount of Precipitated sulfur (MW = 32.06 g/mol) that will be obtained from 15.5 g of lime (MW = 56.07 g/mol) a 28.06 g b 32.45 g c 23.63 g d 19.21 g

In the laboratory you are given the task of separating Ag* and Fe* ions in aqueous solution. For each reagent listed below indicate if it can be used to separate the ions. Type "Y" for or "N" for no. If the reagent CAN be used to separate the ions, give the formula of the precipitate. If it cannot, type "No" yes Y or N Reagent Formula of Precipitate if YES 1. HBr 2. K2SO4 3. КОН

Some chemical reactants are listed in the table below. Complete the table by filling in the oxidation state of the highlighted atom. oxidation state of species highlighted atom FeO(s) Cl2(9) SiO2(9) ОН (ад)

Consider the two-step process for the formation of tellurous acid described by the following equations:  ???2+ 2??−⟶ ???3 2− + ?2? ???3 2− + 2?+⟶ ?2???3 What mass of H2TeO3 is formed from 74.2 g of TeO2, assuming 100% yield?

The following solutions are needed to be prepared for the titration procedure:1. 20 mL of 2 M HCl2. 20 mL of 0.05 M KOHYou went through the titration process wherein 1.0867 grams of Fe(OH)n was mixed with the 20 mL of 2 M HCl that you initially prepared. This solution was diluted to 200 mL and was labeled as solution A. 20.0 mL aliquot of solution A was taken and titrated with 20.0 mL of 0.05 M KOH.Submit a detailed procedure of what you had done the above titration (include all the laboratory apparatus that you used).

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In the laboratory you are given the task of separating Ag" and Cu* ions in aqueous solution. For each reagent listed below indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the ions, give the formula of the precipitate. If it cannot, type "No" Y or N Reagent Formula of Precipitate if YES 1. Nal 2. NaOH 3.O K2S

Octane has a density of 0.703g/ml. Calculate the mass of CO2 produced by burning one gallon of octane. There are 3.79 liters to one gallon.

How many grams of this precipitate form? What is the concentration of Ni2+ that remains in solution?   What is the concentration of SO2−4SO42− that remains in solution?

A 1.00 g sample of KCl is dissolved in 38.0 mL of water. The resulting solution is then added to 56.0 mL of a 0.350 M CaCl2 (ag) solution. Assuming that the volumes are additive, calculate the concentrations of each ion present in the final solution. Concentration of K+ ions = M Concentration of Ca²+ ions = M Concentration of Cl- ions M %3D