Elemental SS reacts with O2O2 to form SO3SO3 according to the
reaction
2S+3O2→2SO3
How many O2 molecules are needed to react with 3.16 g of S?
What is the theoretical yield of SO3 produced by 3.16 g
To determine how many O2 molecules are needed to react with 3.16 g of S, we first need to convert the mass of S into moles.
The molar mass of S is 32.06 g/mol.
Number of moles of S = mass of S / molar mass of S
Number of moles of S = 3.16 g / 32.06 g/mol = 0.0986 mol
According to the balanced equation, the ratio of moles of S to moles of O2 is 2:3. Therefore, the number of moles of O2 needed can be calculated as:
Number of moles of O2 = (2/3) * Number of moles of S
Number of moles of O2 = (2/3) * 0.0986 mol = 0.0657 mol
Now, we can convert the number of moles of O2 into molecules.
Avogadro's number tells us that 1 mole of any substance contains 6.022 x 10^23 molecules.
Number of O2 molecules = Number of moles of O2 * Avogadro's number
Number of O2 molecules = 0.0657 mol * 6.022 x 10^23 molecules/mol = 3.95 x 10^22 molecules
Therefore, 3.95 x 10^22 O2 molecules are needed to react with 3.16 g of S.
To find the theoretical yield of SO3 produced by 3.16 g of S, we need to use the stoichiometry of the balanced equation.
From the balanced equation, we can see that 2 moles of S react to form 2 moles of SO3.
Number of moles of SO3 produced = (2/2) * Number of moles of S
Number of moles of SO3 produced = (2/2) * 0.0986 mol = 0.0986 mol
The molar mass of SO3 is 80.06 g/mol.
Mass of SO3 produced = Number of moles of SO3 produced * molar mass of SO3
Mass of SO3 produced = 0.0986 mol * 80.06 g/mol = 7.889 g
Therefore, the theoretical yield of SO3 produced by 3.16 g of S is 7.889 g.
To find the number of O2 molecules needed to react with 3.16 g of S, we need to use the molar ratio from the balanced equation.
1. Calculate the molar mass of S:
The molar mass of S is 32.06 g/mol.
2. Convert the mass of S to moles:
To convert grams to moles, divide the given mass by the molar mass of S:
Moles of S = mass of S / molar mass of S = 3.16 g / 32.06 g/mol = 0.0987 mol
3. Use the mole ratio from the balanced equation:
From the balanced equation, we can see that 2 moles of S react with 3 moles of O2 to produce 2 moles of SO3.
Therefore, the mole ratio of S to O2 is 2:3, meaning that for every 2 moles of S, we need 3 moles of O2.
4. Calculate the moles of O2 required:
Moles of O2 = (moles of S) x (3 moles of O2 / 2 moles of S)
= 0.0987 mol x (3/2)
= 0.1481 mol
So, 0.1481 moles of O2 molecules are needed to react with 3.16 g of S.
To calculate the theoretical yield of SO3 produced by 3.16 g of S, we need to convert the moles of S to moles of SO3 using the molar ratio from the balanced equation.
5. Calculate the moles of SO3 produced:
From the balanced equation, we can see that 2 moles of S react to produce 2 moles of SO3.
Therefore, the mole ratio of S to SO3 is 2:2, meaning that for every 2 moles of S, we produce 2 moles of SO3.
Moles of SO3 = (moles of S) x (2 moles of SO3 / 2 moles of S)
= 0.0987 mol x (2/2)
= 0.0987 mol
So, the theoretical yield of SO3 produced by 3.16 g of S is 0.0987 mol.