How do I figure this out?
In the reaction CS2 + 3O2 → CO2 + 2SO2, when 160 g of CS2 and 195 g of O2 are reacted, the theoretical yield of SO2 is 260 g.
To figure out the question, we can use stoichiometry.
1. First, we need to determine which reactant is limiting or limiting reagent. To do this, we calculate the number of moles for each reactant.
To find the number of moles, we divide the given mass of each reactant by their respective molar masses.
Molar mass of CS2 = 12.01 g/mol (C) + 32.07 g/mol (S) x 2 = 76.14 g/mol
Molar mass of O2 = 16.00 g/mol (O) x 2 = 32.00 g/mol
Number of moles of CS2 = 160 g / 76.14 g/mol = 2.10 mol
Number of moles of O2 = 195 g / 32.00 g/mol = 6.09 mol
2. Next, we need to determine the stoichiometric ratio between the reactant and product. From the balanced equation: CS2 + 3O2 → CO2 + 2SO2, we see that the ratio of CS2 to SO2 is 1:2.
3. Now, we can use the stoichiometry to find the theoretical yield of SO2. Since CS2 is the limiting reactant, we can calculate the theoretical yield of SO2 using the stoichiometric ratio.
Theoretical yield of SO2 = Number of moles of CS2 x (2 moles of SO2 / 1 mole of CS2) x Molar mass of SO2.
Number of moles of SO2 = 2.10 mol x (2 mol SO2 / 1 mol CS2) = 4.20 mol
Molar mass of SO2 = 32.07 g/mol (S) + 16.00 g/mol (O) x 2 = 64.07 g/mol
Theoretical yield of SO2 = 4.20 mol x 64.07 g/mol = 268.53 g (approximately 269 g)
Therefore, we find that the theoretical yield of SO2 is approximately 269 g, not 260 g as mentioned in the question.
To figure this out, you will need to use stoichiometry to determine the theoretical yield of SO2. Here's a step-by-step breakdown of the calculation:
1. Write down the balanced chemical equation for the reaction:
CS2 + 3O2 → CO2 + 2SO2
2. Determine the molar masses of the reactants and products involved:
Molar mass of CS2 = 12.01 g/mol (C) + 32.07 g/mol (S) × 2 = 76.14 g/mol
Molar mass of O2 = 16.00 g/mol (O) × 2 = 32.00 g/mol
Molar mass of CO2 = 12.01 g/mol (C) + 16.00 g/mol (O) × 2 = 44.01 g/mol
Molar mass of SO2 = 32.07 g/mol (S) + 16.00 g/mol (O) × 2 = 64.07 g/mol
3. Calculate the number of moles of CS2 and O2 used:
Number of moles of CS2 = 160 g / 76.14 g/mol = 2.10 mol
Number of moles of O2 = 195 g / 32.00 g/mol = 6.09 mol
4. Use the stoichiometric ratios from the balanced equation to determine the number of moles of SO2 produced:
According to the balanced equation, the ratio of CS2 to SO2 is 1:2. Therefore, for every 1 mol of CS2, 2 mol of SO2 is produced.
Number of moles of SO2 = 2.10 mol CS2 × (2 mol SO2 / 1 mol CS2) = 4.20 mol
5. Calculate the mass of SO2 produced using the molar mass of SO2:
Mass of SO2 = Number of moles of SO2 × Molar mass of SO2
Mass of SO2 = 4.20 mol × 64.07 g/mol = 269 g (rounded to the nearest whole number)
Comparing the calculated mass of SO2 (269 g) with the given theoretical yield (260 g), you can see that it is slightly higher.