Question

Elemental sulfur can be recovered from gaseous hydrogen sulfide through the reaction: 2 H2S (g) + SO2 (g) ® 3 S (s) + 2 H2O (l) What volume of H2S (in L, at 0.00°C and one atm) is required to produce 2.00 kg of sulfur by this process?

Answer 1

Molar mass of S = 32.07 g/mol

mass of S = 2.00 Kg = 2000 g

mol of S = (mass)/(molar mass)

= 2000/32.07

= 62.3636 mol

From balanced chemical reaction, we see that

when 3 mol of S reacts, 2 mol of H2S is required

mol of H2S required = (2/3)* moles of S

= (2/3)*62.3636

= 41.58 mol

we have:

P = 1.0 atm

n = 41.58 mol

T = 0.0 oC

= (0.0+273) K

= 273 K

we have below equation to be used:

P * V = n*R*T

1 atm * V = 41.58 mol* 0.0821 atm.L/mol.K * 273 K

V = 932 L

Answer: 932 L