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inna [77]
3 years ago
9

A sheet of steel 1.5 mm thick has nitrogen atmospheres on both sides at 1200°C and is permitted to achieve a steady-state diffus

ion condition. The diffusion coefficient for nitrogen in steel at this temperature is 6 × 10−11 m2/s, and the diffusion flux is found to be 1.2 × 10−7 kg/m2·s. Also, it is known that the concentration of nitrogen in the steel at the high-pressure surface is 4 kg/m3.
How far into the sheet from this high-pressure side will the concentration be 2.0 kg/m3?
Assume a linear concentration profile.
Chemistry
1 answer:
Svetradugi [14.3K]3 years ago
4 0

Answer:

1.2 × 10−7 kg/m2·s

Explanation:

Please mark me as brainiest

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A chemical engineer must calculate the maximum safe operating temperature of a high-pressure gas reaction vessel. The vessel is
Anuta_ua [19.1K]

The maximum safe operating temperature for this reaction is equal to 895°C.

<u>Given the following data:</u>

  • Width of cylinder = 22 cm.
  • Height, h = 26.4 cm.
  • Maximum safe pressure = 6.30mpa.
  • Mass = 0.537 kg.

<u>Scientific data:</u>

  • Ideal gas constant, R = 8.314 L-kPa/Kmol.
  • Molar mass of of dinitrogen monoxide (N_2F_2) gas = 66 g/mol.

Radius, r = \frac{width}{2} =\frac{22}{2} =11\;cm

<h3>How to calculate the maximum safe operating temperature.</h3>

First of all, we would determine the volume of the stainless-steel cylinder by using this formula:

V=\pi r^2 h\\\\V = 3.142 \times 11^2 \times 26.4\\\\

Volume, V = 10,036.81 cm^3.

In liters, we have:

Volume, V = 10.04 Liters.

Next, we would determine the number of moles of dinitrogen monoxide (N_2F_2) gas:

Number \;of \;moles = \frac {mass}{molar\;mass}\\\\Number \;of \;moles = \frac {537}{66}

Number of moles = 8.136 moles.

Now, we can solve for the maximum safe operating temperature by applying the ideal gas equation:

PV=nRT\\\\T=\frac{PV}{nR} \\\\T=\frac{6.30 \times 10^3 \times 10.04}{8.136 \times 8.314}\\\\T=\frac{60541.2}{67.6427}

T = 895.02 ≈ 895°C.

Read more on temperature here: brainly.com/question/24769208

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