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.
2 H2S(g) + SO2(g) �¨ 3 S(s) + 2 H2O(g)
To determine the volume of H2S required, we need to use the ideal gas law equation:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in liters)
n = moles of gas
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin)
First, we need to calculate the number of moles of S produced. This can be done using the molar mass of S:
1 mole of S = 32.06 grams
55.0 g of S / (32.06 g/mol) = 1.7158 mol of S
According to the balanced equation, 2 moles of H2S produce 3 moles of S. Therefore, the moles of H2S required can be calculated as follows:
(1.7158 mol S) * (2 mol H2S / 3 mol S) = 1.1439 mol H2S
Now, we can calculate the volume of H2S using the ideal gas law equation. Rearranging the equation to solve for V:
V = nRT / P
V = (1.1439 mol) * (0.0821 L·atm/(mol·K)) * (375 K) / (1.20 atm)
V ≈ 27.026 L
Therefore, approximately 27.026 liters of H2S are needed to produce 55.0 g of S at 375 K and 1.20 atm.
To determine the volume of H2S needed to produce 55.0 g of S, we need to use the stoichiometry of the balanced equation.
The balanced equation is:
2 H2S(g) + SO2(g) → 3 S(s) + 2 H2O(g)
From the stoichiometry of the balanced equation, we see that 2 moles of H2S are needed to produce 3 moles of S.
To find the moles of S produced, we need to convert the given mass of S (55.0 g) to moles.
The molecular weight of S is 32.06 g/mol. Using the formula: moles = mass / molecular weight, we find:
moles of S = 55.0 g / 32.06 g/mol ≈ 1.715 moles of S
Since 2 moles of H2S are needed to produce 3 moles of S, we can set up a proportion to find the moles of H2S needed:
2 moles H2S / 3 moles S = x moles H2S / 1.715 moles S
Solving for x gives:
x ≈ (2 moles H2S / 3 moles S) * 1.715 moles S
x ≈ 1.143 moles H2S
Now we need to determine the volume of H2S at the given conditions of 375 K and 1.20 atm.
To do this, we can use the ideal gas law, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin.
Rearranging the ideal gas law equation to solve for V, we get:
V = (nRT) / P
Plugging in the values, we have:
V = (1.143 moles H2S * 0.0821 L·atm/mol·K * 375 K) / 1.20 atm
Calculating this gives the volume of H2S needed to produce 55.0 g of S at the given conditions.