The maximum safe operating temperature for this reaction is equal to 895°C.
<u>Given the following data:</u>
- Width of cylinder = 22 cm.
- Maximum safe pressure = 6.30mpa.
<u>Scientific data:</u>
- Ideal gas constant, R = 8.314 L-kPa/Kmol.
- Molar mass of of dinitrogen monoxide () gas = 66 g/mol.
Radius, r =
<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:
Volume, V = 10,036.81 .
In liters, we have:
Volume, V = 10.04 Liters.
Next, we would determine the number of moles of dinitrogen monoxide () gas:
Number of moles = 8.136 moles.
Now, we can solve for the maximum safe operating temperature by applying the ideal gas equation:
T = 895.02 ≈ 895°C.
Read more on temperature here: brainly.com/question/24769208
Steps:
Mw = w * R * T / p * V
T = 88 + 273 => 361 K
p = 975 mmHg in atm :
1 atm = 760 mmHg
975 mmg / 760 mmHg => 1.28 atm
Therefore:
= 0.827 * 0.0821 * 361 / 1.28 * 0.270
= 24.51 / 0.3456
molar mass = 70.92 g/mol
The balanced equation for the formation of ammonia is as follows
N₂ + 3H₂ --> 2NH₃
stoichiometry of H₂ to NH₃ is 3:2
Avagadros law states that at volume of gas is proportional to number of moles of gas at contant pressure and temperature
therefore molar ratio is equivalent to volume ratio
hence, volume ratio of H₂ to NH₃ is 3:2
if 2 L of NH₃ requires 3 L of H₂
then 3.0 L of NH₃ requires - 3/2 x 3.0 L = 4.5 L of H₂
volume of H₂ required is
<span>C.4.5L</span>