Physical Chemistry Answers

Pure iron may be produced from the reactions of iron (III) oxide (F_e2 O₃) and carbon dioxide (CO) . The other proucts of the reactions is carbon dioxide ( CO₂) Fe₂O₃ + 2Fe + 3CO₂

a. How many grams of Fe₂ O₃ are needed to completely consume 1.5 molecules of CO?

b. How may moles of Fe can be obtained from 100grams of Fe₂O₃?

3. Sodium metal reacts with hydrogen to form sodium hydride (NaH). 2Na + H₂ to 2NaH

If 10grams of Na reacts with 8grams of H_2, How many grams of the products will be formed? Which reactant limiting?

Sulfuric acid ( H₂SO₄) is use in the production of phosphate fertilizer. The reaction is:

C_a3 (PO₄)₂+3H₂SO₄ to 3C_aSO₄ + 2H₃PO_4, How many grams of the two products are formed in 10.0 moles of H₂SO₄ is reacted with enough calcium phosphate [ C_a3 (PO₄)₂) ?

Distillation can be used to separate

What technology or research is involved with this career?

Gas is compressed slowly and

isothermally at 300K from 1 bar to 8bar. Calculate the

work done using the given state of equation. (B = -5.397 X 10-6 m3

/mol)

(note: volume at each stage should be near to the ideal gas volume)

PV

RT = 1 +

B

VGas is compressed slowly and isothermally at 300K from 1 bar to 8bar. Calculate the

work done using the given state of equation. (B = -5.397 X 10-6 m3

/mol)

(note: volume at each stage should be near to the ideal gas volume)

PV

RT = 1 +

B

V

7.23 × 1024 Al atoms

The bimolecular reaction of chlorine monoxide can result in the formation of three different combinations of products or product channels (the rate constant for each reaction is indicated): ClO(g) + ClO(g) → Cl2(g) + O2(g) k= 2.9 × 106 ClO(g) + ClO(g) → ClOO(g) + Cl(g) k= 7.0 × 106 ClO(g) + ClO(g) → OClO(g) + Cl(g) k= 2.1 × 106 By using 1.00 bar chlorine monoxide, what would be the partial pressure yield of chlorine atom? A) 0.38 bar B) 0.12 bar C) 0.58 bar D) 0.18 bar E) 0.70 bar 

A transparent microscope glass (2 x 5 cm) is covered with a TiO₂-film. The TiO₂-film is placed at the bottom of a Petri dish. The Petri dish is covered with a glass lid transparent to light at wavelengths above 320 nm. When using the lid, oxygen intrusion into the Petri dish can be neglected. The Petri dish is filled with 20 ml pure water (oxygen-free). The Petri dish with the photocatalyst at the bottom is illuminated with continuous light at 360 nm. The intensity of the incident light is 2 mW/cm². During the illumination the concentration of H₂O₂ is monitored as a function of time. The concentration reaches a constant level of 2.4 micromolar after 10 minutes. H₂O₂ is catalytically decomposed on TiO₂. The heterogeneous rate constant for the catalytic decomposition is 1.7 x 10^-5 m/s. In a separate experiment the light transmission of the TiO₂-film at 360 nm was determined to be 5.9 %. Calculate the quantum yield for photocatalytic formation of H₂O₂ under the present circumstances.