a mixture of 50g of S & 1x10^2g of Cl2 reacts completely to form S2Cl2 &SCl2. Find the mass of S2Cl2 formed.
see other post. Reaction is not possible.
Well, let me calculate that using my trusty clown calculator. 🎪
First, we need to find the limiting reagent. To do this, we compare the number of moles of S and Cl2.
The molar mass of S is approximately 32 g/mol, so we have (50 g / 32 g/mol) = 1.56 mol of S.
The molar mass of Cl2 is approximately 71 g/mol, so we have (100 g / 71 g/mol) = 1.41 mol of Cl2.
Since we need 1 mol of S to react with 1 mol of Cl2 to form S2Cl2, and we have more moles of S than Cl2, Cl2 is our limiting reagent.
Now, let's calculate the mass of S2Cl2 formed.
The molar mass of S2Cl2 is approximately 135 g/mol. Since S2Cl2 is formed in a 1:1 ratio with Cl2, we'll have 1.41 mol of S2Cl2.
Therefore, the mass of S2Cl2 formed is (1.41 mol x 135 g/mol) ≈ 190.35 g.
So, the mass of S2Cl2 formed is approximately 190.35 grams. Enjoy your S2Cl2 stews! 🍲
To find the mass of S2Cl2 formed, we need to determine the limiting reactant, which is the reactant that is completely used up in the reaction. Once we determine the limiting reactant, we can use its stoichiometry to calculate the mass of S2Cl2 formed.
To begin, let's calculate the number of moles for each reactant:
1. Calculate the number of moles of S:
- Given mass of S = 50g
- Molar mass of S = 32.06 g/mol
- Moles of S = mass / molar mass = 50g / 32.06 g/mol
2. Calculate the number of moles of Cl2:
- Given mass of Cl2 = 100g
- Molar mass of Cl2 = 70.91 g/mol
- Moles of Cl2 = mass / molar mass = 100g / 70.91 g/mol
Next, we need to determine the stoichiometry of the reaction to find the ratio of moles between S2Cl2 and the reactants. The balanced equation for the reaction is:
2S + Cl2 → S2Cl2 + SCl2
From the balanced equation, we can see that 2 moles of S react with 1 mole of Cl2 to form 1 mole of S2Cl2.
Now, let's compare the moles of S and Cl2 to determine the limiting reactant:
- Divide the moles of S by its stoichiometric coefficient (2).
- Divide the moles of Cl2 by its stoichiometric coefficient (1).
Whichever value is smaller corresponds to the limiting reactant.
Once we determine the limiting reactant, we can use its stoichiometry to calculate the mass of S2Cl2 formed. In this case, since Cl2 has a smaller number of moles, it is the limiting reactant.
Now, let's calculate the moles of S2Cl2 formed using the stoichiometry:
- Mole ratio of S2Cl2 to Cl2 is 1:1 (from the balanced equation).
- Moles of S2Cl2 = Moles of Cl2
Finally, we can calculate the mass of S2Cl2 using its molar mass:
- Molar mass of S2Cl2 = (2 * molar mass of S) + molar mass of Cl2
- Mass of S2Cl2 = Moles of S2Cl2 * molar mass of S2Cl2
By following these steps and performing the calculations, you'll find the mass of S2Cl2 formed.