For the reaction CS2+3Cl2=CCl4+S2Cl2, calculate the percent yield if 719 g of CCl4 are produced when 410 g of CS2 react w/ an excess of chlorine.
I have absolutely no clue on how to do this!! If I could get some help that would be great!!
the balanced equation indicates it takes 1 mole of CS2 to produce each mole of CCl4.
Moles CS2 should equal moles of CCl4
you have moles of CS2:
410grams/molemass=5.39 moles (check that).
so you should get mass of CCl4:
5.39(molmeassCCl4)=5.39*154=830g check that.
so your precent yield= what you got/what should have been
Oh, you're in a bit of a pickle, aren't you? Don't worry, I'll help you out with this chemistry conundrum. Percent yield is a measure of how efficiently a reaction produces the desired product. It's like trying to catch flies with a fly swatter – you want to catch as many as possible, but sometimes a few slip away.
To calculate the percent yield, you need to compare the actual yield (the amount of CCl4 you really got) to the theoretical yield (the amount of CCl4 you should have gotten if the reaction went perfectly according to the balanced equation).
First, we need to find the theoretical yield. From the balanced equation, we can see that the ratio between CS2 and CCl4 is 1:1. So, if 410 g of CS2 react, we would expect to produce 410 g of CCl4. Keep in mind that this is based on an ideal world – no spills, no errors, and absolutely no clumsy lab assistants.
Next, we look at the actual yield. You said that 719 g of CCl4 were produced. So, we take 719 g (actual yield) and divide it by 410 g (theoretical yield) and multiply by 100 to get the percent yield.
Percent yield = (actual yield / theoretical yield) x 100
Percent yield = (719 g / 410 g) x 100
Now, grab your calculator and divide 719 by 410, then multiply the result by 100. I promise, this math won't bite!
And there you have it – the percent yield of your reaction. I hope that helps, and remember, if at first you don't succeed, try, try again... or just blame the lab equipment.
To calculate the percent yield, we need to compare the actual yield (the amount of CCl4 actually produced) to the theoretical yield (the maximum amount of CCl4 that could be produced based on stoichiometry).
First, we 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. To find the limiting reactant, we can convert the mass of each reactant to moles using their respective molar masses.
Molar mass of CS2 = 76.14 g/mol
Molar mass of Cl2 = 70.906 g/mol
Moles of CS2 = 410 g / 76.14 g/mol ≈ 5.38 mol
Moles of Cl2 = excess (since it's in excess)
The balanced equation tells us that the ratio of CS2 to CCl4 is 1:1, so the theoretical yield of CCl4 is equal to the moles of CS2 used.
Theoretical yield of CCl4 = 5.38 mol
Now, we need to convert the theoretical yield to grams to compare with the actual yield.
The molar mass of CCl4 is 153.82 g/mol.
Theoretical yield of CCl4 = 5.38 mol × 153.82 g/mol ≈ 825.50 g
Now we can calculate the percent yield.
Percent yield = (actual yield / theoretical yield) × 100
= (719 g / 825.50 g) × 100
≈ 87.04%
Therefore, the percent yield of CCl4 is approximately 87.04%.
To calculate the percent yield of a reaction, you will need two pieces of information: the actual yield (in this case, the mass of CCl4 produced) and the theoretical yield (the maximum amount of CCl4 that could be produced based on stoichiometry).
1. Start by balancing the chemical equation:
CS2 + 3Cl2 → CCl4 + S2Cl2
2. Calculate the molar mass of CS2:
C = 12.01 g/mol
S = 32.07 g/mol
So, the molar mass of CS2 = (12.01 g/mol) + (2 × 32.07 g/mol) = 76.15 g/mol
3. Convert the mass of CS2 (410 g) to moles:
Moles of CS2 = Mass of CS2 / Molar mass of CS2
4. Use stoichiometry to determine the theoretical yield of CCl4:
From the balanced equation, the mole ratio between CS2 and CCl4 is 1:1. So, moles of CCl4 = moles of CS2.
5. Convert moles of CCl4 to grams:
Mass of CCl4 = Moles of CCl4 × Molar mass of CCl4
6. Finally, calculate the percent yield:
Percent Yield = (Actual yield / Theoretical yield) × 100
Given that 719 grams of CCl4 are produced, you now have all the necessary information to calculate the percent yield.