Question

Check my answer? In the manufacturing process of sulfuric acid, sulfur dioxide is reacted with oxygen to produce sulfur trioxide. Using the equation, 2SO2 (g) + O2 arrow 2SO3 (g), if 128 g of sulfur dioxide is given the opportunity to react with an excess of oxygen, but only produces 144 g of sulfur trioxide, what is the percent yield of this reaction?

29.24%

58.48%

90.0%

100.0%

Answer 1

My answer is C

Answer 2

Im not sure about this one :/
can you try looking at this? :/
http://openstudy.com/study#/updates/53a99966e4b0ffdda15ea9ee
If we cant come up with anything ill tag someone else :)

Answer 3

Hmm, I think I have it correct, but if you could tag someone, that would be helpful :)

Answer 4

Ok :)
@misssunshinexxoxo @Compassionate @chmvijay

Answer 5

I think you have it right :/

Answer 6

Thank you I hope so!

Answer 7

:)

Answer 8

@Ciarán95

Answer 9

What do you think the answer is?

Answer 10

They put C

Answer 11

\(\color{blue}{\text{Originally Posted by}}\) @bruno102
My answer is C
\(\color{blue}{\text{End of Quote}}\)
.

Answer 12

e.e

Answer 13

I think you are correct, Bruno102.

Answer 14

Thank you!

Answer 15

Convert the 128g into moles

Answer 16

@iYuko my answer isn't correct?

Answer 17

You tell me.

Answer 18

Multiply that by 2 then convert it to a mass

Answer 19

Yes, I think so.

Answer 20

@iYuko what should I do after I convert it to a mass?

Answer 21

@iYuko

Answer 22

What you do is you convert mass into moles of SO2, since the ratio of SO2 to SO3 is 2:2 you actually don't need to multiply by 2, so you have the moles of SO3 currently, so you are able to multiply that by the molar mass of SO3 to get your theoretical yield. So you can take your experimental yield and divide by your theoretical yield and multiply by 100 to get your percent

Answer 23

And I got 90% when I did it

Answer 24

Thank you so much @taramgrant0543664

Answer 25

No problem!