How many grams of SO3 are produced when 20 g FeS2 reacts with 16g O2 according to the balanced equation?

4FeS2(s)+15 O2(g)>>>2Fe2O3+8SO3(g)

To determine the number of grams of SO3 produced, we need to use stoichiometry and the given balanced equation.

First, let's calculate the number of moles of FeS2 and O2:

Molar mass of FeS2 = 55.85 g/mol (Fe) + 32.07 g/mol (S) * 2 = 119.99 g/mol
Molar mass of O2 = 16.00 g/mol (O) * 2 = 32.00 g/mol

Number of moles of FeS2 = 20 g / 119.99 g/mol = 0.167 moles (approximately)
Number of moles of O2 = 16 g / 32.00 g/mol = 0.500 moles

According to the balanced equation, the stoichiometric ratio between FeS2 and SO3 is 4:8, meaning that for every 4 moles of FeS2, 8 moles of SO3 are produced.

Since we have 0.167 moles of FeS2, the number of moles of SO3 produced can be calculated as follows:

Number of moles of SO3 = (0.167 moles FeS2 / 4 moles FeS2) * 8 moles SO3
= 0.334 moles SO3

Finally, let's calculate the grams of SO3 produced:

Molar mass of SO3 = 32.07 g/mol (S) + 16.00 g/mol (O) * 3 = 80.07 g/mol

Grams of SO3 = 0.334 moles SO3 * 80.07 g/mol
= 26.79 grams

Therefore, approximately 26.79 grams of SO3 are produced when 20 grams of FeS2 reacts with 16 grams of O2.

To determine how many grams of SO3 are produced when 20 g of FeS2 reacts with 16 g of O2, you need to use stoichiometry.

Step 1: Calculate the number of moles of FeS2 and O2 using their molar masses.
- The molar mass of FeS2 is 119.98 g/mol.
- The molar mass of O2 is 32.00 g/mol.

Number of moles of FeS2 = mass / molar mass = 20 g / 119.98 g/mol = 0.167 mol
Number of moles of O2 = mass / molar mass = 16 g / 32.00 g/mol = 0.500 mol

Step 2: Use the balanced equation to determine the mole ratio between FeS2 and SO3.
From the balanced equation: 4 FeS2 : 8 SO3
- This means that for every 4 moles of FeS2, 8 moles of SO3 are produced.

Step 3: Use the mole ratio to calculate the number of moles of SO3 produced.
- Since the mole ratio is 4:8, we can say that 0.167 mol of FeS2 will produce (8/4) x 0.167 mol = 0.334 mol of SO3.

Step 4: Calculate the mass of SO3 produced.
Mass of SO3 = number of moles x molar mass = 0.334 mol x 80.06 g/mol = 26.72 g

Therefore, when 20 g of FeS2 reacts with 16 g of O2, 26.72 g of SO3 are produced according to the balanced equation.

Here is a worked example of a stoichiometry problem. Just follow the steps.

http://www.jiskha.com/science/chemistry/stoichiometry.html