Calculate the percent yield if 65.0g of CCl4 was obtained from the reaction CS2 + 3 Cl2 → CCl4 + S2Cl2
CS2 + 3 Cl2 → CCl4 + S2Cl2
%yield = (actual yield/theoretical yield)*100 = (65.0/theoretical yield)*100 = ? BUT you didn't tell me what you started with so I can't calculate a theoretical yield which then could be used to calculate % yield.
No way to know, since you don't say how much of what was used.
When you figure that out, note that you got 65/153.8 = 0.422 moles of CCl4
From the equation, figure how much you should have gotten, and then you can divide to find the % yield.
To calculate the percent yield, we need to compare the actual yield (the amount obtained in the reaction) to the theoretical yield (the amount that could have been obtained if the reaction had gone to completion).
First, we need to determine the balanced chemical equation for the reaction:
CS2 + 3 Cl2 → CCl4 + S2Cl2
From the equation, we can see that 1 mole of CS2 reacts to produce 1 mole of CCl4.
Next, we need to calculate the theoretical yield of CCl4 using stoichiometry.
1. Calculate the molar mass of CS2 (carbon disulfide):
C: 12.01 g/mol x 1 = 12.01 g/mol
S: 32.07 g/mol x 2 = 64.14 g/mol
Total molar mass of CS2 = 12.01 g/mol + 64.14 g/mol = 76.15 g/mol
2. Convert the given mass of CS2 to moles:
Moles of CS2 = Mass of CS2 / Molar mass of CS2
= 65.0 g / 76.15 g/mol
≈ 0.853 moles
3. According to the stoichiometry of the balanced equation, 1 mole of CS2 produces 1 mole of CCl4. Therefore, the theoretical yield of CCl4 is also 0.853 moles.
4. Convert the theoretical yield from moles to grams:
The molar mass of CCl4 (carbon tetrachloride) is 153.82 g/mol.
Theoretical yield of CCl4 = Moles of CCl4 x Molar mass of CCl4
= 0.853 moles x 153.82 g/mol
≈ 131.36 g
Now, we can calculate the percent yield using the formula:
Percent Yield = (Actual Yield / Theoretical Yield) x 100
Given that the actual yield is 65.0 g, and the theoretical yield is 131.36 g, we can substitute these values into the equation:
Percent Yield = (65.0 g / 131.36 g) x 100
≈ 49.52%
Therefore, the percent yield of CCl4 in this reaction is approximately 49.52%.
To calculate the percent yield, you need to compare the actual yield with the theoretical yield. The actual yield refers to the amount of the desired product that was actually obtained in the reaction, while the theoretical yield is the maximum amount of product that could be obtained based on the stoichiometry of the balanced equation.
In this case, the balanced equation is:
CS2 + 3 Cl2 → CCl4 + S2Cl2
From the equation, you can see that the stoichiometric ratio between CS2 and CCl4 is 1:1. This means that for every 1 mole of CS2, you should get 1 mole of CCl4.
To calculate the theoretical yield, you need to convert the mass of CS2 to moles. The molar mass of CS2 is 76.13 g/mol.
Moles of CS2 = Mass of CS2 / Molar mass of CS2
= 65.0 g / 76.13 g/mol
= 0.854 mol of CS2
Since the stoichiometric ratio between CS2 and CCl4 is 1:1, the theoretical yield of CCl4 is also 0.854 mol.
To convert the theoretical yield from moles to grams, you can multiply by the molar mass of CCl4. The molar mass of CCl4 is 153.82 g/mol.
Theoretical Yield of CCl4 = Theoretical Yield in moles * Molar mass of CCl4
= 0.854 mol * 153.82 g/mol
= 131.43 g
Now that we have calculated the theoretical yield, we can calculate the percent yield using the following formula:
Percent Yield = (Actual Yield / Theoretical Yield) * 100
Given that the actual yield is 65.0 g, and the theoretical yield is 131.43 g, we can substitute these values into the formula:
Percent Yield = (65.0 g / 131.43 g) * 100
= 49.48%
Therefore, the percent yield of CCl4 in this reaction is 49.48%.