a) An iron sulfide contains 36.5% S by mass. The iron sulfide is heated in an atmosphere of pure oxygen, which produces SO2(g) and an iron oxide containing 27.6% O by mass.

Write a balanced equation for the reaction.

If 1.0 kg of the iron sulfide reacts with excess oxygen, what is the theoretical yield of the iron oxide?

b) In the manufacture of Portland cement, limestone (CaCO3(s)) is decomposed into lime (CaO(s)) and CO2(g), in a kiln. Use data from Appendix C in your textbook to calculate how much heat is required to decompose 2.70 × 103 kg of limestone. (Assume that the heats of reaction are temperature independent.)

In experiments concerned with the photoelectric effect, which of the following will increase the kinetic energy of an electron ejected from a metal surface? 1. increasing the wavelength of the light striking the surface 2. increasing the frequency of the light striking the surface 3. increasing the number of photons of light striking the surface A) 1 only B) 2 only C) 3 only D) 1 and 3 E) 1, 2, and 3

What is the product of 4-tert-butyl phenol reacted with p-bromobenzyl bromide when potassium hydroxide and ethanol is added with microwave heating.

Consider the titration of a 38.0mL sample of 0.170M  HBr with 0.205M KOH. Determine each of the following:

Part A: the initial pH

Part B: the volume of added base required to reach the equivalence point

Part C: the pH at 11.0mL of added base

Part D: the pH at the equivalence point

Part E: the pH after adding 5.0 mL of base beyond the equivalence point

The following information is to be used for the next two questions. Molar absorptivity data for the cobalt and nickel complexes with 2,3-quinoxalinedithiol are ε_Co = 36400 and ε_Ni = 5520 at 510 nm and ε_Co = 1240 and ε _Ni = 17500 at 656 nm. A 0.514-g sample was dissolved and diluted to 100.0 mL. A 25.0-mL aliquot was treated to eliminate interferences; after addition of 2,3-quinoxalinedithiol, the volume was adjusted to 50.0 mL. This solution had an absorbance of 1.246 at 510 nm and 0.367 at 656 nm in a 1.00-cm cell.

1. Calculate the concentration of cobalt (in ppm) in the initial solution prepared by dissolving the sample.

2. Calculate the concentration of nickel (in ppm) in the initial solution prepared by dissolving the sample.

I have some chemistry questions. please get all the answers correct ;)

a) Calculate the standard cell potential for the following cell

Zn (s) | Zn²⁺ (aq) (1M) || Co²⁺ (aq) (1M) | Co (s)

answer = __________V

b) The following cell was constructed and found to produce a voltage of 1.08 V.

Co (s) | Co²⁺ (aq) (1M) || Ag⁺ (aq) (1M) | Ag (s)

Calculate the standard reduction potential for Ag⁺ (aq) | Ag (s)

answer = _______V

c) Which of these species is the best oxidising agent?

Standard Reduction Potentials

Cu²⁺ | Cu    +0.34V

Ni²⁺ | Ni     �0.24V

Co²⁺ | Co    �0.28V

Fe²⁺ | Fe        �0.44V

Zn²⁺ | Zn    �0.76V

Mg²⁺ | Mg       �2.36V

Explain the difference between weak-field and strong-field metal complexes.

(around 200 words please)

Steam distillation. ANSWER IN DETAIL AND I WILL REWARD FIVE STARS TO FIRST PERSON TO ANSWER!!!!!!

A student steam distilled a mixtrue of toluene (bp 110.8 degrees Celsius) and water and noticed that distillate contained a larger volume of touleune than water. The student said to the professor, "I know there is something wrong with my experiment. I should have more water than toleune because water has a lowerboiling point. Should I redo the experiment?" The professor replied "do whatever you need to do" A classmate then said, "No, you dont need to redo it you DO have more water."

Explain in detail why the classmate is correct. Use calculations to support your explanation. Label all quantities used. Include all units.

Which cobalt complex was favored when the solution was taken off the heat plate and put in an ice bath? The solution contained deionzied water, ethanol, and cobalt II chloride. The solution went from blue to pink. If you could explain this using Le Chatelier's principle, thank you!

construct a flow diagram for Dehydration of Methylcyclohexanol via Gas Chromatography experiment.

Consider the reaction

CO(g)+NH3(g)⇌HCONH2(g),    Kc=0.760

If a reaction vessel initially contains only CO and NH3 at concentrations of 1.00 M and 2.00 M, respectively, what will the concentration of HCONH2 be at equilibrium?

What is the final pH when 9.77 g of phosphoric acid (98.00 g/mol) and 4.75 g of NaOH (40.00 g/mol) are added to 1 L of water. K_a1 = 1.1 x 10^-2 K_a2 = 7.5 x 10^-8 K_a3= 4.3 x 10^-13

In the first step of the Ostwald process for the synthesis of nitric acid, ammonia is converted to nitric oxide by the high-temperature reaction
4NH3(g)+5O2(g)→4NO(g)+6H2O(g)

Part A: How is the rate of consumption of O2 related to the rate of consumption of NH3?

Part B: How is the rate of formation of NO related to the rate of consumption of NH3?

Part C: How is the rates of formation of H2O related to the rate of consumption of NH3?

Determine the pH change when 0.069 mol KOH is added to 1.00 L of a buffer solution that is 0.326 M in HClO and 0.290 M in ClO^-.

pH after addition ? pH before addition = pH change =

A 50/50 blend of engine coolant and water (by volume) is usually used in an automobile\'s engine cooling system. If your car\'s cooling system holds 4.20 gallons, what is the boiling point of the solution? Make the following assumptions in your calculation: at normal filling conditions, the densities of engine coolant and water are 1.11 g/mL and 0.998 g/mL respectively. Assume that the engine coolant is pure ethylene glycol (HOCH2CH2OH), which is non-ionizing and non-volatile, and that the pressure remains constant at 1.00 atm. Also, you\'ll need to look up the boiling-point elevation constant for water.