If 49.6 mL of liquid CS2 and 12.8 g of gaseous Cl2 are reacted stoichiometrically according to the balanced equation, how many moles of liquid S2Cl2 are produced?
CS2(l) + 3Cl2(g) �¨ CCl4(l) + S2Cl2(l)
You need the density of CS2 to convert mL to grams, then to moles.
To find the number of moles of liquid S2Cl2 produced, we need to first determine the limiting reactant in the given reaction.
To do this, we compare the number of moles of each reactant to their respective stoichiometric coefficients in the balanced equation.
Let's calculate the number of moles of CS2 first:
- Given volume: 49.6 mL
- The molar mass of CS2 is approximately 76.14 g/mol
- We can convert the volume of CS2 to moles using the following equation:
Moles = Volume (L) x Concentration (mol/L)
Assuming the concentration of CS2 is 1 M (mol/L), we have:
- Volume = 49.6 mL = 0.0496 L
- Moles of CS2 = 0.0496 L x 1 mol/L = 0.0496 mol
Next, let's calculate the number of moles of Cl2:
- Given mass: 12.8 g
- The molar mass of Cl2 is approximately 70.90 g/mol
- Moles of Cl2 = Mass / Molar mass
- Moles of Cl2 = 12.8 g / 70.90 g/mol = 0.1804 mol
Based on the balanced equation, the stoichiometric ratio between CS2 and Cl2 is 1:3. This means that for every 1 mole of CS2, 3 moles of Cl2 are required.
By comparing the moles of CS2 (0.0496 mol) and Cl2 (0.1804 mol), we can see that we have an excess of Cl2. The CS2 is the limiting reactant since it determines the amount of product formed.
According to the balanced equation, the stoichiometric ratio between CS2 and S2Cl2 is 1:1. This means that for every 1 mole of CS2, 1 mole of S2Cl2 is produced.
Therefore, the number of moles of liquid S2Cl2 produced is 0.0496 mol.