Posted by Sara on Wednesday, October 7, 2009 at 11:02pm.
Determine the percent yeild of:
KCl3(s)--> KCl(s)+ O2(g)
2.14g of KCl3 produces 0.67 of O2
I get 123% when the correct answer is 80%
KCl3: mm = 122.45, n =0.017
Theoretical yield: .017mol * 32g/mol
Pecent Yield: 0.67g/ 0.544g *100% = 123%
Chem - DrBob222, Wednesday, October 7, 2009 at 11:15pm
Thanks for showing your work. It helped me spot the error right off. You didn't balance the equation. Also note that I corrected the formula for KClO3 but you have the right moles so you must have used the correct molar mass.
2KClO3 ==> 2KCl + 3O2
moles KClO3 = 2.14/122.5 = 0.0175
moles oxygen = 0.0175 x (3 moles O2/2 moles KClO3) = 0.0175 x (3/2) = 0.0262.
grams O2 = moles O2 x molar mass = 0.0262 x 32 = 0.838 g O2 for theoretical yield.
Use that number with 0.67 and see if it's ok. I get 79.9% which rounds to 80% to two significant figures (which is all we are allowed with the 0.67).
Chem - MathMate, Wednesday, October 7, 2009 at 11:18pm
First, start with a balanced equation
2KClO3(s)--> 2KCl(s)+ 3O2(g)
2KClO3: mm=2(39+35.5+16*3)= 245
3O2: mm = 3(2*16) = 96
Chem-corr. - MathMate, Wednesday, October 7, 2009 at 11:20pm
80.% (to two significant figures)
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