If 0.500 g of sulfur dioxide from pollutants reacts with excess water and oxygen found in the air, what mass of sulfuric acid can be produced?
2H2O(l)+O2(g)+2SO2(g)= 2H2SO4(aq)
To find the mass of sulfuric acid produced, we need to start by calculating the number of moles of sulfur dioxide (SO2) present.
The molar mass of sulfur dioxide (SO2) is calculated as follows:
S: 1 atom x 32.07 g/mol = 32.07 g/mol
O: 2 atoms x 16.00 g/mol = 32.00 g/mol
Adding these values together, we get the molar mass of SO2:
32.07 g/mol + 32.00 g/mol = 64.07 g/mol
Now, we can calculate the moles of SO2 using the given mass:
moles of SO2 = mass of SO2 / molar mass of SO2
moles of SO2 = 0.500 g / 64.07 g/mol
Let's calculate this value:
moles of SO2 = 0.500 g / 64.07 g/mol ≈ 0.0078 mol
According to the balanced equation, every 2 moles of SO2 will produce 2 moles of H2SO4 (sulfuric acid).
So, the moles of H2SO4 produced will be equal to the moles of SO2 produced.
moles of H2SO4 = moles of SO2 ≈ 0.0078 mol
Now, we need to convert moles back into mass to find the mass of H2SO4 produced.
mass of H2SO4 = moles of H2SO4 x molar mass of H2SO4
The molar mass of H2SO4 is calculated as follows:
H: 2 atoms x 1.01 g/mol = 2.02 g/mol
S: 1 atom x 32.07 g/mol = 32.07 g/mol
O: 4 atoms x 16.00 g/mol = 64.00 g/mol
Adding these values together, we get the molar mass of H2SO4:
2.02 g/mol + 32.07 g/mol + 64.00 g/mol = 98.09 g/mol
Let's calculate the mass of H2SO4 now:
mass of H2SO4 = moles of H2SO4 x molar mass of H2SO4
mass of H2SO4 = 0.0078 mol x 98.09 g/mol ≈ 0.764 g
Therefore, approximately 0.764 g of sulfuric acid can be produced.
To determine the mass of sulfuric acid that can be produced, we need to calculate the molar mass of sulfuric acid and use it to convert the given mass of sulfur dioxide to the mass of sulfuric acid.
First, let's find the molar mass of sulfuric acid (H2SO4):
- The molar mass of hydrogen (H) is approximately 1 g/mol.
- The molar mass of sulfur (S) is approximately 32 g/mol.
- The molar mass of oxygen (O) is approximately 16 g/mol.
Since there are two hydrogen atoms, one sulfur atom, and four oxygen atoms in each molecule of sulfuric acid, the molar mass is calculated as follows:
(2 * 1g/mol) + (1 * 32g/mol) + (4 * 16g/mol) = 98 g/mol.
Next, we can use the balanced chemical equation to determine the mole ratio between sulfur dioxide and sulfuric acid. The equation shows that for every 2 moles of sulfur dioxide, 2 moles of sulfuric acid are produced.
Given that we have 0.500 g of sulfur dioxide, we need to convert this mass to moles using the molar mass of sulfur dioxide. The molar mass of sulfur dioxide (SO2) is approximately 64 g/mol.
0.500 g / 64 g/mol = 0.00781 mol.
Since the mole ratio between sulfur dioxide and sulfuric acid is 2:2, we can conclude that 0.00781 mol of sulfur dioxide will produce an equal number of moles of sulfuric acid.
Finally, we can convert the number of moles of sulfuric acid to the mass of sulfuric acid using its molar mass:
0.00781 mol * 98 g/mol = 0.765 g.
Therefore, approximately 0.765 g of sulfuric acid can be produced from the given 0.500 g of sulfur dioxide.