None A 0.02 cm BCC iron foil is used to separate a high hydrogen gas from a low hydrogen gas at420 °C. 511,498,741 H atoms/cm³ are in equilibrium on one side of the foil, and 11,730 Hatoms/cm³ are in equilibrium with the other side. Determine the flux of hydrogen throughthe foil in atoms/cm2/s. You will need to find the properties of hydrogen diffusing throughiron in the text book, Table 5-1.Report your answer to 3 significant figures, for example 1.23e5 or 3.45e8.Do not put any spaces in the number or CANVAS will interpret it as a two values. You canalso enter the answer using decimal notation, for example123400000.

To determine the flux of hydrogen through the iron foil, we need to use Fick's first law of…

Answered: A 0.02 cm BCC iron foil is used to…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter11: Solutions

Section: Chapter Questions

Problem 18P

See similar textbooks

Similar questions

How does hydraulic fracturing differ from previously used techniques for the recovery of natural gas from the earth?
Some Chem 16.1 students were tasked to perform the ideal gas experiment with some modifications. Instead of magnesium ribbon, the students were to use 0.029 g of aluminum foil. They prepared the eudiometer by adding 6M HCI and filling it with water to the brim. Once the setup was complete, they performed the experiment. Note that the aluminum was completely consumed in the reaction. From the experiment, it was found that the external pressure was 1.05 atm at 30.0 °C, and the volume of the air inside the eudiometer was 33.5 mL. The water level inside the eudiometer is 4.15 cm below the surface of the water level outside. Given these measurements and the following constants, answer the proceeding questions. At 30.0°C, Pvapor = 31.8 mmHg • R = 0.08206 L-atm/mol-K = 62.36 L-torr/mol-K • MWAI = 26.98 g/mol A. Find the value of the pressure of dry air (PDA) in torr. B. Give the balanced chemical reaction of the aluminum metal with the acid. C. Find the experimental mass (in grams) of…
The size of the ionic atmosphere, called the Debye radius, is 1/K, where K is given by e2 NA 1/2 VI E0 ɛkBT K = where e is the electronic charge, NA Avogadro's constant, ɛo the permittivity of vacuum (8.854×10-12 c²·n-1.m-2), ɛ the dielectric constant of the solvent, kB the Boltzmann constant, T the absolute temperature, and I the ionic strength. Calculate the Debye radius in a 0.036 m aqueous Na2S203 solution at 25°C. (Assume the density of the solution at 25°C is 1.0029 g•cm-3.) 4.0 4.208 Å
Before small batteries were available, carbide lamps were used for bicycle lights. Acetylene gas, C2H2, and solid calcium hydroxide were formed by the reaction of calcium carbide, CaC2, with water. The ignition of the acetylene gas provided the light. Currently, the same lamps are used by some cavers, and calcium carbide is used to produce acetylene for carbide cannons.(a) Outline the steps necessary to answer the following question: What volume of C2H2 at 1.005 atm and 12.2 °C is formed by the reaction of 15.48 g of CaC2 with water?(b) Answer the question.
A student experimentally determines the gas law constant, R, by reacting a small piece of magnesium with excess hydrochloric acid and then collecting the hydrogen gas over water in a eudiometer. Based L-atm on experimentally collected data, the student calculates R to equal 0.0832 mol·K L-atm Ideal gas law constant from literature: 0.08206 mol·K (a) Determine the percent error for the student's R-value. Percent error = % (b) For the statements below, identify the possible source(s) of error for this student's trial. The student notices a large air bubble in the eudiometer after collecting the hydrogen gas, but does not dislodge it. The student does not clean the zinc metal with sand paper. The student does not equilibrate the water levels within the eudiometer and the beaker at the end of the reaction. The water level in the eudiometer is 1-inch above the water level in the beaker. The student uses the barometric pressure for the lab to calculate R.
A chemical engineer must calculate the maximum safe operating temperature of a high-pressure gas reaction vessel. The vessel is a stainless-steel cylinder tha measures 52.0 cm wide and 62.4 cm high. The maximum safe pressure inside the vessel has been measured to be 7.00 MPa. For a certain reaction the vessel may contain up to 25.8 kg of sulfur hexafluoride gas. Calculate the maximum safe operating temperature the engineer should recommend for this reaction. Write your answer in degrees Celsius. Round your answer to 3 significant digits. temperature: C x10 X
0.0500 grams of zinc metal reacted in excess HCl(aq) in a gas tube and produced hydrogen gas that was collected over water at 25°C and aqueous zinc chloride. The barometric pressure in the room was 740 mm Hg. The vapor pressure of water at 25°C is 23.8 mm Hg. What is the theoretical yield (volume) of hydrogen gas that should be collected in this lab?
Canadian chemists have developed a modern variation ofthe 1899 Mond process for preparing extremely pure metallicnickel. A sample of impure nickel reacts with carbon monoxideat 50°C to form gaseous nickel carbonyl, Ni(CO)₄.(a) How many grams of nickel can be converted to the carbonylwith 3.55 m³ of CO at 100.7 kPa?(b) The carbonyl is then decomposed at 21 atm and 155°C to pure (>99.95%) nickel. How many grams of nickel are obtainedper cubic meter of the carbonyl?(c) The released carbon monoxide is cooled and collected forreuse by passing it through water at 35C. If the barometric pres-sure is 769 torr, what volume (in m³) of CO is formed per cubicmeter of carbonyl?
7. A technician is setting up a laboratory to standardise ~0.0200 mol dm–3 KMnO4. What mass of Mohr’s salt [FeSO4(NH4)2SO4·6H2O] would the technician be required to weigh out to produce a 5.00 L solution of Mohr’s salt such that 25.0 cm3 aliquots of the salt would require a titre of 20.0 cm3 to standardise the KMnO4 solution?
When hydrogen iodide gas is associated into hydrogen and iodine gases, at temperature of 698.8 K at 1.85 x 10^-2, assess and estimate the weight in grams of hydrogen iodide formed when the gas products formed are heated to 698.8 K in 3.01 liter veassel. Assuming 10.01 grams of iodide, and 0.202 gram of hydrogen were formed from the dissociation reaction, determine the partial pressure of the three components in the reaction: H2, I, and HI.
A 2.00 L reaction container at 25.0 °C contains CO2 (g) and O2 (g). The total pressure of the gases in the container was 656 torr and the mole fraction of CO2 is 0.245. A)Calculate the partial pressure of oxygen gas in the mixture. B)Calculate the mass of oxygen gas in the mixture (in g). C)Which gas will rise to the top of the container? Explain your answer.
If the molecular weight of air is 28.9,what is the density of air at atmosphericpressure and a temperature of 368.7 K?1 atm = 1.013 × 10^5 N/m2, the mass ofa proton is 1.67262 × 10 ^−27 kg , Avogadro’snumber is 6.02214 × 10 ^23 mol−1and k =1.38065 × 10^ −23 N · m/K .Answer in units of kg/m3.

SEE MORE QUESTIONS

Recommended textbooks for you

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

Introduction to General, Organic and Biochemistry

Chemistry

ISBN:

9781285869759

Author:

Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS