Asked by Zufan Hagos
Calculate the percent yield if 65.0g of CCl4 was obtained from the reaction CS2 + 3 Cl2 → CCl4 + S2Cl2
Answers
Answered by
DrBob222
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.
%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.
Answered by
oobleck
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.
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.
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