How many grams of carbon disulfide,CS2 will form if 0.450 mol of carbon is consumed in a 3C+2SO2=CS2 +2CO2 reaction

Here is a worked example of a stoichiometry problem. Just follow the steps. http://www.jiskha.com/science/chemistry/stoichiometry.html

0.15g CS2

To find the number of grams of carbon disulfide (CS2) formed in the reaction, we need to use the given information and follow a few steps.

Step 1: Write the balanced equation for the reaction:
3C + 2SO2 -> CS2 + 2CO2

This equation tells us that three moles of carbon react with two moles of sulfur dioxide to produce one mole of carbon disulfide and two moles of carbon dioxide.

Step 2: Calculate the molar mass of CS2:
Carbon (C) has a molar mass of 12.01 g/mol, and sulfur (S) has a molar mass of 32.07 g/mol. Since carbon disulfide has two sulfur atoms, we multiply the molar mass of sulfur by 2.
Molar mass of CS2 = (12.01 g/mol) + (2 × 32.07 g/mol) = 12.01 g/mol + 64.14 g/mol = 76.15 g/mol

Step 3: Determine the number of moles of CS2 produced:
We are given that 0.450 mol of carbon is consumed in the reaction. According to the balanced equation, one mole of carbon produces one mole of CS2.
Since 0.450 mol of carbon is consumed, the same number (0.450 mol) of moles of CS2 will be produced.

Step 4: Calculate the mass of CS2 produced:
To find the mass of CS2, we use the equation:
Mass = Number of moles × Molar mass

Mass of CS2 = 0.450 mol × 76.15 g/mol
Mass of CS2 = 34.27 g

Therefore, 0.450 mol of carbon will produce 34.27 grams of carbon disulfide (CS2) in the given reaction.