Elemental sulfur can be converted to sulfur dioxide by combustion in air. Sulfur dioxide will react with water to form sulfurous acid (see balanced equation below).
SO2(g) + H2O(l) → H2SO3(l)
What mass of sulfur dioxide is needed to prepare 29.36 g of H2SO3(l)?
A. 0.4582 g
B. 29.36 g
C. 37.61 g
D. 22.91g
SO2(g) + H2O(l) → H2SO3(l)
mols H2SO3 needed = grams/molar mass = 29.36/82 = estimated 0.3
1 mol SO2 provides 1 mol H2SO3; therefore, approx 0.3 mol H2SO3 will need approx 0,3 mol SO2.
grams SO2 = mols SO2 x molar rmass SO2 = ? Remember my numbers are estimates.
To determine the mass of sulfur dioxide needed to prepare 29.36 g of H2SO3, we need to use stoichiometry.
First, let's find the molar mass of H2SO3:
H2SO3 = (2 * 1.01 g/mol) + (32.07 g/mol) + (16.00 g/mol * 3)
H2SO3 = 62.08 g/mol
Now, we need to use the balanced equation to establish the mole ratio between sulfur dioxide (SO2) and sulfurous acid (H2SO3):
1 mol SO2 : 1 mol H2SO3
Next, we can use the molar mass and mole ratio to calculate the number of moles of H2SO3:
moles H2SO3 = mass H2SO3 / molar mass H2SO3
moles H2SO3 = 29.36 g / 62.08 g/mol
moles H2SO3 ≈ 0.473 mol
Since the mole ratio is 1:1 between SO2 and H2SO3, the number of moles of SO2 is also approximately 0.473 mol.
Finally, we can calculate the mass of SO2 needed:
mass SO2 = moles SO2 * molar mass SO2
mass SO2 = 0.473 mol * 64.07 g/mol
mass SO2 ≈ 30.27 g
Therefore, the mass of sulfur dioxide needed to prepare 29.36 g of H2SO3 is approximately 30.27 g.
The closest option is:
C. 37.61 g
To calculate the mass of sulfur dioxide (SO2) needed to prepare a certain amount of sulfurous acid (H2SO3), we can use stoichiometry and the given balanced chemical equation.
The balanced equation tells us the molar ratio between SO2 and H2SO3. From the equation, we can see that 1 mole of SO2 reacts with 1 mole of H2SO3.
Step 1: Convert the mass of H2SO3 to moles.
Given that the mass of H2SO3 is 29.36 g, we need to convert this to moles. To do this, we need the molar mass of H2SO3, which is calculated by adding up the atomic masses of each element present in the compound.
H2SO3: (2 × 1.01 g/mol) + (32.07 g/mol) + (3 × 16.00 g/mol) = 82.09 g/mol
Now we can convert the mass of H2SO3 to moles:
Moles of H2SO3 = Mass of H2SO3 / Molar mass of H2SO3
= 29.36 g / 82.09 g/mol
≈ 0.357 mol
Step 2: Use the stoichiometry to find the mass of SO2.
Now that we have the moles of H2SO3, we can use the balanced equation to find the moles of SO2 needed. From the equation, we know that 1 mole of SO2 reacts with 1 mole of H2SO3.
Moles of SO2 = Moles of H2SO3
≈ 0.357 mol
Finally, we can convert the moles of SO2 to grams using the molar mass of SO2:
Mass of SO2 = Moles of SO2 × Molar mass of SO2
= 0.357 mol × (32.07 g/mol)
≈ 11.46 g
Therefore, the mass of sulfur dioxide needed to prepare 29.36 g of H2SO3 is approximately 11.46 g.
Since none of the given answer choices match the calculated value, it is possible that there is an error either in the given answer choices or in the calculation process.