Given the following chemical equation, if 162.0 grams of potassium reacts with excess oxygen gas and was found to produce 172 grams of potassium oxide, what is the percent yield for this reaction?
4 K(s) + O2(g) arrow 2K2O(s)

44%

75%

22%

88%

Question

Given the following chemical equation, if 162.0 grams of potassium reacts with excess oxygen gas and was found to produce 172 grams of potassium oxide, what is the percent yield for this reaction?
4 K(s) + O2(g) arrow 2K2O(s)
		
44%
		
75%
		
22%
		
88%

nvidiaintely · Answer

@Google @Kevin @ScribblePikachu

nvidiaintely · Answer

@Will.H Can someone help me with this?

natalief · Answer

can you provide the relative atomic mass of Potassium???

nvidiaintely · Answer

39.0983

scribblepikachu · Answer

i would say 88%

kevin · Answer

I'm sorry. I really don't know what is the 'percent yield' means.
I need to see how the other people solve this kind of question. So I can solve this too.

natalief · Answer

yes it is 88%

nvidiaintely · Answer

Thanks.
How did you get there @ScribblePikachu?

natalief · Answer

@Kevin Percentage yield is dividing the mass of the actual yield by the mass of theorectical yield and then x100%

scribblepikachu · Answer

188.4 gram of K2O should be formed for 100% yield 
then in this case  172 gram is formed 
188.4 gram = 100 % 
172 gram = 100*172 / 188.4 = 91.3 % but the closest to that is 88% so it should be 88% if not it would be lower than that meaning it would had been the exsact % of the other ones

nvidiaintely · Answer

T H A N K   Y O U !

scribblepikachu · Answer

np