**Answer:**

We need 29.2 L of H2S

**Explanation:**

Step 1: Data given

Volume of H2S = TO BE DETERMINED

Temperature = 375 K

Pressure = 1.20 atm

Mass of S = 55.0 grams

Molar mass of S = 32.065 g/mol

Step 2: The balanced equation:

2H2S(g) + SO2(g) ⇒ 3 S(s) + 2 H2O(g)

Step 3: Calculate moles of S

Moles of S = Mass S / molar mass of S

Moles of S = 55.0 grams / 32.065 g/mol

Moles of S = 1.715 moles

Step 4: Calculate moles of H2S

For 2 moles of H2S we need 1 mol of SO2 to produce 3 moles of S and 2 moles of H2O

For 1.715 moles S we need, (2/3)*1.715 = 1.14 moles of H2S

Step 5: Calculate volume of H2S

p*V=n*R*T

⇒ p = the pressure of H2S = 1.20 atm

⇒ V = The volume of H2S = TO BE DETERMINED

⇒ n = the moles of H2S = 1.14 moles H2S

⇒ R = the gas constant = 0.08206 L*atm/K*mol

⇒ T = The temperature = 375 K

V= (n*R*T)/P

V = (1.14*0.08206*375)/1.20

V = 29.2 L

We need 29.2 L of H2S