What is the minimum mass of water necessary to produce 200. g of sulfuric acid in the following reaction?
2SO2 + O2 + 2H2O → 2H2SO4
How many moles of H2SO4 do you want? That's moles = g/molar mss 200/98 = 2.04
Then 2.04 mols H2SO4 x (2 mols H2O/2 molsH2SO4) = 2.04 x 2/2 = 2.04 moles H2O needed.
Then grams H2O = moles H2O x molar mass H2O = ?
To determine the minimum mass of water necessary to produce 200 g of sulfuric acid, we need to first calculate 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, and the molar mass of oxygen (O) is approximately 16 g/mol.
To calculate the molar mass of sulfuric acid (H2SO4), we add up the molar masses of its constituent elements:
2 moles of hydrogen (2 * 1 g/mol) = 2 g/mol
1 mole of sulfur (32 g/mol) = 32 g/mol
4 moles of oxygen (4 * 16 g/mol) = 64 g/mol
Adding these masses together, the molar mass of sulfuric acid (H2SO4) is:
2 g/mol + 32 g/mol + 64 g/mol = 98 g/mol
Given that the balanced chemical equation for the reaction states that 2 moles of sulfuric acid are produced for every 2 moles of water, we can use the stoichiometric ratio to calculate the mass of water required to produce 200 g of sulfuric acid.
1 mole of sulfuric acid (H2SO4) has a molar mass of 98 g/mol.
Therefore, 200 g of sulfuric acid is equal to:
200 g / (98 g/mol) = 2.04 mol of sulfuric acid
Since 2 moles of sulfuric acid are produced from 2 moles of water:
2.04 mol of sulfuric acid requires 2.04 mol of water.
Finally, to calculate the mass of water required, we multiply the molar mass of water by the number of moles required:
2.04 mol of water * 18 g/mol (molar mass of water) = 36.72 g of water
Therefore, the minimum mass of water necessary to produce 200 g of sulfuric acid is approximately 36.72 g.
To determine the minimum mass of water necessary to produce 200. g of sulfuric acid in the given reaction, we need to calculate the stoichiometric ratio between sulfuric acid and water.
Looking at the balanced equation:
2SO2 + O2 + 2H2O → 2H2SO4
We can see that for every 2 moles of sulfuric acid (H2SO4) produced, 2 moles of water (H2O) are also consumed.
First, we need to find the molar mass of sulfuric acid (H2SO4):
H2SO4: 2(1.01 g/mol) + 32.07 g/mol + 4(16.00 g/mol) = 98.09 g/mol
To calculate the moles of sulfuric acid required to produce 200. g:
Moles of H2SO4 = Mass of H2SO4 / Molar mass of H2SO4
Moles of H2SO4 = 200. g / 98.09 g/mol = 2.04 mol
Since the stoichiometric ratio between sulfuric acid and water is 1:1, we need an equal number of moles of water.
Moles of H2O required = Moles of H2SO4 = 2.04 mol
Finally, we can calculate the mass of water needed:
Mass of H2O = Moles of H2O × Molar mass of H2O
Mass of H2O = 2.04 mol × 18.02 g/mol = 36.85 g
Therefore, the minimum mass of water necessary to produce 200. g of sulfuric acid is approximately 36.85 grams.