How many grams of CS2(g) can be prepared by heating 12.9 moles of S2(g) with excess carbon in a 7.00 L reaction vessel held at 900 K until equilibrium is attained? Stoichiometry is 1 to 1
If stoichiometry is 1 to 1 then 12.9 mols CS2 can be formed. Convert to grams by g = mols x molar mass.
To find the number of grams of CS2(g) that can be prepared, we need to use stoichiometry and the molar mass of CS2.
1. Start by determining the molar mass of CS2, which can be calculated by adding the atomic masses of carbon (C) and sulfur (S) present in one molecule. The atomic mass of carbon is 12.01 g/mol, and the atomic mass of sulfur is 32.07 g/mol. Thus, the molar mass of CS2 is 12.01 + 2(32.07) = 76.15 g/mol.
2. Next, use the given amount of S2(g) in moles (12.9 moles) and the stoichiometry of the reaction (1 to 1) to determine the amount of CS2(g) formed. Since the stoichiometry is 1 to 1, the number of moles of CS2(g) formed will also be 12.9 moles.
3. To convert moles to grams, multiply the number of moles of CS2(g) by its molar mass. In this case, the mass of CS2(g) will be 12.9 moles × 76.15 g/mol = 984.435 g.
Therefore, by heating 12.9 moles of S2(g) with excess carbon, you can prepare 984.435 grams of CS2(g) in the given reaction vessel.