Given the data: 1. Mass of test tube + MNO² = 21.5403g                       21.5403g 2. Mass of the test tube + MnO² + KClO³ + KCl             22.5518g 3. Constant mass of test tube + reaction product          22.3514g  a. Mass of O2 released:  Answers by an expert of bartleyby:  1) 0.078 moles 2) 0.2004g  b. Moles of O2 released: 1) 0.00243 moles 2) 0.0063 mol c. Moles of KClO3 required by the moles 1) 0.00163 moles d. Mass of KClO3 required:  1) 0.5116g g KClO3  d. Mass KClO3 & KCl mixture: 1) 1.0115g

I'm very confused. I didnt knew that 3 subtopics could be answered, so I uploaded one subtopic at the time. After gerting teh answers back, I uploaded the entire question and got the answer for the first 3 subtopics ( I'll call this A). However, a few of the single questions previously uploaded were answered and they are different from A. I'll upload the entire document again and please answer subtopics c, . If possible please confirm the write answer!

Given the data:

1. Mass of test tube + MNO² = 21.5403g                       21.5403g

2. Mass of the test tube + MnO² + KClO³ + KCl             22.5518g

3. Constant mass of test tube + reaction product          22.3514g 

a. Mass of O2 released: 

Answers by an expert of bartleyby: 

1) 0.078 moles

2) 0.2004g 

b. Moles of O2 released:

1) 0.00243 moles

2) 0.0063 mol

c. Moles of KClO3 required by the moles

1) 0.00163 moles

d. Mass of KClO3 required: 

1) 0.5116g g KClO3 

d. Mass KClO3 & KCl mixture:

1) 1.0115g

e. Percent composition of KClO3 & KCl mixture 

1) 50.56%

f. If there were 0.5011g KClO3 in the original mixture, what is the true percent of KClO3?