28.6 grams of SO2 react in the following synthesis: SO2+O2->SO3 How many grams of SO3 could be produced
First, balance the equation:
2SO2 + O2 -> 2SO3
equal moles of SO2 and SO3
So, how many moles of SO2 in 28.6 grams?
To find out how many grams of SO3 could be produced, we need to use stoichiometry. Stoichiometry involves calculating the quantities of reactants and products in a chemical reaction.
1. Begin by writing the balanced chemical equation:
2 SO2 + O2 → 2 SO3
2. Determine the molar mass of each substance:
- Molar mass of SO2 = 32.06 g/mol
- Molar mass of O2 = 31.9988 g/mol
- Molar mass of SO3 = 80.06 g/mol
3. Convert the given mass of SO2 to moles:
- Moles of SO2 = mass (g) / molar mass (g/mol)
- Moles of SO2 = 28.6 g / 32.06 g/mol
- Moles of SO2 = 0.892 mol SO2
4. Use the stoichiometry of the balanced equation to determine the moles of SO3 produced:
- From the balanced equation, we see that 2 moles of SO2 react to produce 2 moles of SO3.
- Therefore, 0.892 mol SO2 will produce (0.892 mol SO3 / 2 mol SO2) * 2 mol SO3 = 0.892 mol SO3
5. Convert moles of SO3 to grams:
- Mass of SO3 = moles of SO3 * molar mass of SO3
- Mass of SO3 = 0.892 mol * 80.06 g/mol
- Mass of SO3 = 71.43 g
Therefore, 28.6 grams of SO2 would produce approximately 71.43 grams of SO3.