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first and most important, balance the equation
Yep, @JFraser is right. Do you know how to balance, @firesquad ?
Balanced equation: 8Zn + S8 ---> 8ZnS
Yep, good. Percent yield = (actual/theoretical)*100
Actual is the amount of product given in the problem.
Theoretical is the amount of product found using stoichiometry from the amount of reactant given.
*from the amount of limiting reactant
I am stuck right here 4.88 g Zn x (1 mol Zn/ 65.38 g Zn) = 0.07464 mol Zn 5.03 g S8 x (1 mol S8/ 256.48 g S8) = 0.01961 mol S8
Ok, now use the molar ratios from the balanced reaction to convert to moles of ZnS
what do i do after
For both calculations.
would the ratio be 1: 8
For S8:ZnS, yes
But not for Zn:ZnS
0.07464 mol Zn * (1/1)= 0.07464 mol Zn 0.01961 mol S8 * (8/1) = 0.1569 mol S8 is that how to do it
Well, that looks good for everything but the units at the end.
What do I have to change for the units?
0.07464 mol ZnS 0.1569 mol ZnS
See why I did that?
Oh Ok, now I find the percent yield right?
Well, we need to first determine which value of product to go with.
This is the limiting reactant part. Do you know how to determine that?
The limiting reactant is S8
No, the limiting reactant is the reactant that produces less product.
Sorry, it is Zn
So, what is the mass of product using the limiting reactant?
Sorry for wait I had to do something. It is 0.07464 mol ZnS
No worries. That is the moles of product. What is the mass of product?
65.38 g Zn
Hm, that's not what I get. How did you do that?
I got it from the first formula
Hm, let me show you how I would do this step: 0.07464 mol ZnS(97.44 g/1 mol) = ? g ZnS
Ok I get it
:-) So, can you find the percent yield?
Wait 7.27 is the theoretical yield
so what is the actual yield?
The amount of product given in the problem.
Thank you so much
You're welcome! :-)