The combustion of carbon disulfide in the presence of excess oxygen yields carbon dioxide and sulfur dioxide:

CS2(g)+3O2(g)--->CO2(g)+2SO2(g)

The combustion of 17.2 g of CS2 in the presence of excess oxygen yields __________ g of SO2.

Here is a solved example of a stoichiometry problem. Just follow the steps. Post your work if you get stuck.

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

25.26 g

To determine the mass of SO2 produced, we need to use stoichiometry and the given mass of CS2.

Step 1: Find the molar mass of CS2:
C = 12.01 g/mol
S = 32.07 g/mol
Molar mass of CS2 = (12.01 g/mol x 1) + (32.07 g/mol x 2) = 76.16 g/mol

Step 2: Convert the given mass of CS2 to moles:
Moles of CS2 = Given mass / Molar mass
Moles of CS2 = 17.2 g / 76.16 g/mol = 0.226 moles

Step 3: Use the balanced equation to determine the mole ratio between CS2 and SO2:
From the balanced equation: 1 mol CS2 produces 2 mol SO2

Step 4: Calculate the moles of SO2 produced:
Moles of SO2 = Moles of CS2 x (2 moles SO2 / 1 mol CS2)
Moles of SO2 = 0.226 moles x (2 mol SO2 / 1 mol CS2) = 0.452 moles

Step 5: Convert moles of SO2 to grams:
Molar mass of SO2 = (32.07 g/mol x 2) = 64.14 g/mol
Mass of SO2 = Moles of SO2 x Molar mass of SO2
Mass of SO2 = 0.452 moles x 64.14 g/mol = 29.00 g

Therefore, the combustion of 17.2 g of CS2 in the presence of excess oxygen yields approximately 29.00 grams of SO2.

To find the mass of SO2 produced, we need to use the given mass of CS2 and the balanced equation for the combustion reaction.

First, calculate the molar mass of CS2:
C = 12.01 g/mol
S = 32.07 g/mol
So, the molar mass of CS2 = (12.01 g/mol) + 2(32.07 g/mol) = 76.15 g/mol

Next, we need to determine the number of moles of CS2:
Moles of CS2 = mass of CS2 / molar mass of CS2
Moles of CS2 = 17.2 g / 76.15 g/mol ≈ 0.226 moles

According to the balanced equation, the stoichiometric ratio between CS2 and SO2 is 1:2.
So, the number of moles of SO2 produced will be twice the number of moles of CS2:
Moles of SO2 = 2 × Moles of CS2
Moles of SO2 = 2 × 0.226 ≈ 0.452 moles

Finally, calculate the mass of SO2:
Mass of SO2 = Moles of SO2 × molar mass of SO2

The molar mass of SO2 is:
S = 32.07 g/mol
O = 16.00 g/mol
Molar mass of SO2 = 32.07 g/mol + 2(16.00 g/mol) = 64.07 g/mol

Mass of SO2 = 0.452 moles × 64.07 g/mol ≈ 28.96 g

Therefore, the combustion of 17.2 g of CS2 in the presence of excess oxygen yields approximately 28.96 g of SO2.