Answered

Westonci.ca makes finding answers easy, with a community of experts ready to provide you with the information you seek. Connect with a community of experts ready to provide precise solutions to your questions on our user-friendly Q&A platform. Experience the ease of finding precise answers to your questions from a knowledgeable community of experts.

One of the steps to sweeten sour gas using the Claus process is reacting
hydrogen sulfide gas with sulfur dioxide gas to produce water vapour and sulfur.
16 H2S(g) + 8 SO2(g) → 16 H2O(g) + 3 Sg(s)
8.56 kL of hydrogen sulfide at 175 kPa and 250 °C reacts with excess sulfur
dioxide. Calculate the mass, in kg, of sulfur produced.

Sagot :

ardni313

The mass, in kg, of Sulfur produced : 2.072 kg

Further explanation

Given

V = 8.56 kL = 8560 L

P = 175 kPa = 1,73 atm

T = 250 + 273 = 523 K

Required

mass of Sulfur produced

Solution

mol of H₂S :

[tex]\tt n=\dfrac{PV}{RT}\\\\n=\dfrac{1.73\times 8560}{0.082\times 523}\\\\n=345.3[/tex]

mol of Sulfur based on mol  H₂S as a limiting reactant( excess Sulfur  dioxide)

From equation, mol ratio  H₂S : S = 16 : 3, so mol S :

[tex]\tt \dfrac{3}{16}\times 345.3=64.74[/tex]

Mass S(Ar = 32 g/mol) :

= mol x Ar s

= 64.74 x 32

= 2071.68 g = 2.072 kg

We hope you found this helpful. Feel free to come back anytime for more accurate answers and updated information. Thank you for visiting. Our goal is to provide the most accurate answers for all your informational needs. Come back soon. Thank you for using Westonci.ca. Come back for more in-depth answers to all your queries.