a mixture of 50g of S & 1x10^2g of Cl2 reacts completely to form S2Cl2 &SCl2. Find the mass of S2Cl2 formed.
To find the mass of S2Cl2 formed, we first need to calculate the number of moles of sulfur (S) and chlorine (Cl2) present in the mixture.
Given:
Mass of S = 50g
Mass of Cl2 = 1x10^2g
Step 1: Calculate the number of moles of S and Cl2 using their respective molar masses.
- The molar mass of S is 32.06 g/mol.
- The molar mass of Cl2 is 70.90 g/mol.
Number of moles of S = Mass of S / Molar mass of S
= 50g / 32.06 g/mol
≈ 1.56 moles
Number of moles of Cl2 = Mass of Cl2 / Molar mass of Cl2
= 1x10^2g / 70.90 g/mol
≈ 1.41 moles
Step 2: Determine the limiting reactant.
The limiting reactant is the reactant that will be completely consumed in the reaction, limiting the amount of product that can be formed. To find the limiting reactant, we compare the moles of S and Cl2 using the balanced chemical equation for the formation of S2Cl2 and SCl2.
The balanced chemical equation for the reaction is:
S + Cl2 → S2Cl2 + SCl2
From the equation, we can see that the stoichiometric ratio between S and Cl2 is 1:1. This means that for every mole of S, one mole of Cl2 is required.
Based on the moles calculated in Step 1, we can see that S has a higher number of moles (1.56 moles) compared to Cl2 (1.41 moles). Therefore, Cl2 is the limiting reactant.
Step 3: Determine the moles and mass of S2Cl2 formed.
Based on the balanced chemical equation, we know that for every mole of Cl2, one mole of S2Cl2 is formed.
Number of moles of S2Cl2 formed = Number of moles of Cl2
= 1.41 moles
Finally, we calculate the mass of S2Cl2 formed using its molar mass, which is 135.03 g/mol.
Mass of S2Cl2 formed = Number of moles of S2Cl2 formed × Molar mass of S2Cl2
≈ 1.41 moles × 135.03 g/mol
≈ 190.44 g
Therefore, the mass of S2Cl2 formed is approximately 190.44 grams.
To find the mass of S2Cl2 formed, we first need to determine the limiting reactant. The limiting reactant is the reactant that is completely consumed and determines the maximum amount of product that can be formed.
We can find the amount in moles of each reactant by dividing their respective masses by their molar masses.
The molar mass of S is 32 g/mol, and the molar mass of Cl2 is 71 g/mol.
Moles of S = mass of S / molar mass of S = 50 g / 32 g/mol = 1.5625 mol
Moles of Cl2 = mass of Cl2 / molar mass of Cl2 = 100 g / 71 g/mol = 1.4085 mol
The balanced chemical equation for the reaction is:
S + Cl2 → S2Cl2 + SCl2
From the equation, we can see that the ratio of S to S2Cl2 is 1:1.
Therefore, since we have 1.5625 moles of S, we will form the same amount (in moles) of S2Cl2.
Now, let's calculate the mass of S2Cl2 using the moles of S2Cl2 and its molar mass.
Molar mass of S2Cl2 = (32 g/mol x 2) + 35.5 g/mol = 99.5 g/mol
Mass of S2Cl2 = moles of S2Cl2 x molar mass of S2Cl2
= 1.5625 mol x 99.5 g/mol
= 155.46875 g
Therefore, the mass of S2Cl2 formed is approximately 155.47 g.
To balance the reaction, figure the moles in 50g S, and the moles in 100gCl2.
S: 50/32=1.56
Cl2: 100/71=1.41
so the mole ratio is 1.56/1.41=1.1 or 11 to 10.
At this point,
realizing that more moles of sulfur was consumed than Chlorine, it will not be possible to balance the equation, as the compound with the highest S:Cl2 ratio is S2Cl2, a 1:1 ratio.
Flawed problem.
S+Cl2 >> S2Cl2 + SCl2