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For the reaction represented by the equation: SO3 + H2O → H2SO4, how many grams of sulfur trioxide are required to produce 14.4 mol of sulfuric acid in an excess of water?

Accepted Answer

Here's how to solve this stoichiometry problem:
1. Balanced Equation: The equation is already balanced: SO3 + H2O → H2SO4
2. Mole Ratio: From the balanced equation, 1 mole of SO3 produces 1 mole of H2SO4.
3. Moles of SO3: Since we need to produce 14.4 mol of H2SO4, we need 14.4 mol of SO3.
4. Grams of SO3:
- Molar mass of SO3 = 32.07 g/mol (S) + 3
16.00 g/mol (O) = 80.07 g/mol
- Mass of SO3 = 14.4 mol
80.07 g/mol = 1152.8 g
Therefore, 1152.8 grams of sulfur trioxide are required to produce 14.4 mol of sulfuric acid in an excess of water.

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