Iron(III) oxide reacts with carbon monoxide according to the equation:

Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g)

A reaction mixture initially contains 22.10 g Fe2O3 and 14.00 g CO.

Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?

Express your answer to three significant figures.

Suppose that in an alternate universe, the possible values of l were the integer values from 0 to n(instead of 0 to n−1). Assuming no other differences from this universe, how many orbitals would exist in each of the following levels?

n = 4

DQ 11: Given that the solubility product of PbI₂ is expressed as K_sp = [Pb²⁺][I^–]², calculate the K_sp of PbI₂ from the concentration of Pb²⁺ found in Step 6 of the Data Analysis. (Hint: Think about the stoichiometry involved when PbI₂ was initially formed… how much I^– was left unreacted?) Is PbI₂ a soluble or insoluble salt? Explain.

3mL of 0.05M KI was used and 1mL of 0.05 Pb(NO3)2 was used to make the PbI2 solution/yellow precipitate

All work must be shown below for credit.

(2 pts) Show a properly balanced chemical equation:

Pb(NO₃)_2(aq)+ 2KI_(aq)--> PbI_2(s)+2KNO^-_3(aq)

(4 pts) Determine the limiting reagent:

(2 pts) Calculate the K_sp of PbI₂:

(2 pts) Is PbI₂ a soluble or insoluble salt? Explain:

Consider a 0.20 M NH4Cl aqueous solution. Rank the following species in the solution from highest to lowest concentration.

NH3, Cl-, H2O, NH4+, OH-, H3O+

Consider a 0.10 M aqueous solution of sodium nitrite, NaNO2. Rank the following species in the solution from highest to lowest concentration.  

OH-, HNO2, NO2-, H3O+, H2O, Na+

The acetate ion is the conjugate base of acetic acid. The Ka of acetic acid is 1.76×10–5. What is the pH of a 0.100 M solution of sodium acetate?

Consider the titration of 60.0 mL of 0.100 M NH3 Kb= 1.8 x 10^-5 with 0.150 M HCl. Calculate the pH after the following volumes of titrant have been added: 40.5 mL & 60.0 mL

Two 2.0-cm-diameter insulating spheres have a 7.00 cm space between them. One sphere is charged to + 70.0 nC , the other to - 79.0 nC . Part A What is the electric field strength at the midpoint between the two spheres? Express your answer with the appropriate units.

Although coal is no longer the favored energy source, U.S. coal mines still produced close to a billion short tons of coal. Detail 5 different forms of coal, including activated carbon, and chemical products and health hazards related to each different form. Describe DOT recommended response actions to incidents involving a release of coal and/or carbon.

Why is the mixture of .033 M of H₂SO₃ and .033 M of NaSO₃ not good buffers?

Phosphoric acid is a triprotic acid (Ka1 = 6.9× 10–3, Ka2 = 6.2× 10–8, and Ka3 = 4.8× 10–13). To find the pH of a buffer composed of H2PO4–(aq) and HPO42–(aq), which pKa value would you use in the Henderson-Hasselbalch equation?

Calculate the pH of a buffer solution obtained by dissolving 15.0 g of KH2PO4(s) and 33.0 g of Na2HPO4(s) in water and then diluting to 1.00 L.

For each of the following, what is AE, NE, Lewis structure, VSEPR sketch, VB sketch, geometry description, and bonding description? OF2 H3O+ PCL3 H2O2 CH2O N2 CO2 O3 NO3- NO2 PCl5 SiF6 2- SF4 I3- IF5 XEF4

What mass of ammonium chloride should be added to 2.45 L of a 0.165 M NH3 in order to obtain a buffer with a pH of 9.65?

Glycine, C2H5O2N, is important for biological energy. The combustion reaction of glycine is described by the following thermochemical equation. 4C2H5O2N(s) + 9O2(g) → 8CO2(g) + 10H2O(l) + 2N2(g) ΔH°rxn=-3857 kj/mol. What is the energy transfer in the oxidation of 17.00g of glycine?

(¶) Provide a component diagram sketch of a typical gas chromatography instrument setup and discuss the importance of each component.

(a) A commercial 737 jet transporting 143 passengers and 5 crew members from Kansas City to Baltimore burned 11,800 lbs. (about 1700 gallons) of Jet A fuel en route. Jet A fuel is kerosine based, consisting primarily of C_nH_2n+2 hydrocarbons, with n = 6 to 16, so the carbon: hydrogen ratio is close to 1:2. During this flight, how much CO₂ was released into the atmosphere? Assume the combustion of the fuel was complete, so all the fuel was burned to form CO₂ and H₂O. Give both the mass of CO₂ produced (in kg and lb) and the volume it would occupy at 298 K, 1 atm.

(b) How much CO₂ would be released into the atmosphere is those passengers and crew made the trip instead, in pairs, in hybrid cars at 40 miles per gallon. Assume the density of the gasoline is 0.75 kg/L and that carbon and hydrogen dominate the composition in a ration of 1:2. The road trip is 1082 miles.

Note: This is in the complete problem as written in the textbook, in a chapter about gas laws (both ideal and nonideal).

a. What ammonia levels are considered normal in an estuarine system? What types of toxic effects can it cause? At what concentration levels?

b. What effects do fluoride ions have on finfish? At what concentrations?