Question

Determine the volume of H₂S (at 375 K and 1.20 atm) needed to produce 55.0 g of S. Assume that there is excess SO₂ present.

Answer 1

The volume of H₂S gas needed to produce 55.0 g of sulfur is calculated using the balanced chemical equation, the molar mass of sulfur, and the ideal gas law. It is found to be 42.4 liters at the given conditions of 375 K and 1.20 atm.

Step-by-step explanation:

The student is asking to determine the volume of H₂S gas needed to produce 55.0 g of solid sulfur (S) when H₂S reacts with excess SO₂. We first need to balance the chemical equation:

H₂S + SO₂ → H₂O + S(solid) - becomes balanced with coefficients of 2, 2, 2, and 2 respectively:

2H₂S + 2SO₂ → 2H₂O + 2S(solid)

Next, we calculate the moles of sulfur produced using its molar mass (32.06 g/mol for S):

1. 
   
3. Number of moles of S = 55.0 g / 32.06 g/mol = 1.716 moles S
4. 
   
6. Since the molar ratio of H₂S to S in the balanced equation is 2:2, moles of H₂S needed = moles of S = 1.716 moles.

Finally, we use the ideal gas law (PV=nRT) to find the volume of H₂S gas under the given conditions (R = 0.0821 L is the ideal gas constant).

1. 
   
3. V = nRT/P = (1.716 moles) × (0.0821 L·atm/(mol·K)) × (375 K) / (1.20 atm)
4. 
   
6. V = 42.4 L (calculated by substituting the values into the ideal gas law equation).

The volume of H₂S gas needed at 375 K and 1.20 atm to produce 55.0 g of sulfur is 42.4 liters.