The discussion revolves around the calculation of the volume of KCl produced in the reaction 2KClO3 -----> 2KCl + 3O2. Participants are trying to reconcile differing interpretations of the problem statement and the associated calculations.
Participants do not reach a consensus on the correct interpretation of the problem or the calculation of the volume, indicating multiple competing views remain.
The discussion highlights potential limitations in the problem statement, including missing assumptions and the ambiguity regarding whether the question pertains to moles of solid KCl or gaseous products.
So is it incorrect statement? Because it is asked in my test. Do you think there is another way of thinking about the question? If this is wrong should I inform it to my teacher so they can cancel the question.Chestermiller said:What is the exact and complete problem statement?
I don't know. Maybe those are supposed to be both the numbers of moles in the balanced chemical equation and the actual numbers of moles involved. How did you get 44.8?Aafia said:So is it incorrect statement? Because it is asked in my test. Do you think there is another way of thinking about the question? If this is wrong should I inform it to my teacher so they can cancel the question.
one mole of any gas occupy volume of 22.4dm³ (molar volume) and from equation there are two moles of potassium chloride so volume will be 2×22.4dm³= 44.8dm³. I think they are asking about 2 moles of solid KCl. Is that right?Chestermiller said:I don't know. Maybe those are supposed to be both the numbers of moles in the balanced chemical equation and the actual numbers of moles involved. How did you get 44.8?
That would be my guess.Aafia said:one mole of any gas occupy volume of 22.4dm³ (molar volume) and from equation there are two moles of potassium chloride so volume will be 2×22.4dm³= 44.8dm³. I think they are asking about 2 moles of solid KCl. Is that right?