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.

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

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 :

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 :

Mass S(Ar = 32 g/mol) :

= mol x Ar s

= 64.74 x 32

= 2071.68 g = 2.072 kg

answer: -

reaction:

na + cl ⇌ nacl

balanced chemical equation:

na + 2cl ⇌ nacl2

sodium + clorine goes to form sodium chloride (table salt).

the product is nacl2.

and the reactants are na and cl.

(note: if you don’t know what ⇌ means, read below: -

⇌(double head arrow) means reversible reaction).

water and alcohols have similar properties because water molecules contain hydroxyl groups that can form hydrogen bonds with other water molecules and with alcohol molecules, and likewise alcohol molecules can form hydrogen bonds with other alcohol molecules as well as with water.