2H2O(l) � O2(g) � 2SO2(g) → 2H2SO4(aq)
If 50.0 g of sulfur dioxide from pollutants reacts with
water and oxygen found in the air, how many grams of
sulfuric acid can be produced? How many grams of
oxygen are used in the process?
mols SO2 = grams/molar mass = ?
Using the coefficients in the balanced equation, convert mols SO2 to mols H2SO4.
Now convert mols H2SO4 to grams. g = mols x molar mass = ?
You find the g O2 by the same process. Using the coefficients, convert mols SO2 to mols O2 then convert that to grams O2.
Post your work if you get stuck.
To find out how many grams of sulfuric acid can be produced, we need to consider the balanced equation and the given quantity of sulfur dioxide.
The balanced equation is:
2H2O(l) + O2(g) + 2SO2(g) → 2H2SO4(aq)
According to the equation, 2 moles of sulfur dioxide (SO2) react to produce 2 moles of sulfuric acid (H2SO4). The molar mass of sulfur dioxide is 64.06 g/mol, and the molar mass of sulfuric acid is 98.09 g/mol.
Given that we have 50.0 g of sulfur dioxide, we can calculate the amount of sulfuric acid produced:
50.0 g SO2 * (1 mol SO2 / 64.06 g SO2) * (2 mol H2SO4 / 2 mol SO2) * (98.09 g H2SO4 / 1 mol H2SO4) = X g H2SO4
Simplifying the equation, we get:
X = 77.10 g H2SO4
Therefore, 77.10 grams of sulfuric acid can be produced.
Now, let's determine how many grams of oxygen are used in the process. Using the balanced equation:
2H2O(l) + O2(g) + 2SO2(g) → 2H2SO4(aq)
We can see that 1 mole of oxygen (O2) is needed to produce 2 moles of sulfuric acid (H2SO4).
Using the given amount of sulfur dioxide (50.0 g SO2), we can calculate the amount of oxygen used:
50.0 g SO2 * (1 mol SO2 / 64.06 g SO2) * (1 mol O2 / 2 mol SO2) * (32.00 g O2 / 1 mol O2) = Y g O2
Simplifying the equation, we get:
Y = 25.0 g O2
Therefore, 25.0 grams of oxygen are used in the process.
To find the grams of sulfuric acid produced and the grams of oxygen used in the process, we need to use stoichiometry.
1. Determine the molar mass of the given substances:
- Molar mass of SO2 (sulfur dioxide) = 32.07 g/mol
- Molar mass of H2SO4 (sulfuric acid) = 98.09 g/mol
- Molar mass of O2 (oxygen) = 32.00 g/mol
2. Convert the mass of SO2 to moles using its molar mass:
- Moles of SO2 = mass of SO2 (given) / molar mass of SO2
3. Set up the stoichiometric ratio between SO2, H2SO4, and O2 from the balanced chemical equation:
- According to the balanced equation, for every 2 moles of SO2, 2 moles of H2SO4 and 1 mole of O2 are produced.
4. Calculate the moles of H2SO4 and O2 produced:
- Moles of H2SO4 = Moles of SO2 (calculated in step 2) * (2 moles of H2SO4 / 2 moles of SO2)
- Moles of O2 = Moles of SO2 (calculated in step 2) * (1 mole of O2 / 2 moles of SO2)
5. Convert the moles of H2SO4 and O2 to grams using their respective molar masses:
- Mass of H2SO4 = Moles of H2SO4 * Molar mass of H2SO4
- Mass of O2 = Moles of O2 * Molar mass of O2
By following the steps above, we can now calculate the grams of sulfuric acid produced and the grams of oxygen used in the process.