## bruno102 one year ago 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%

1. bruno102

2. pooja195

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 :)

3. bruno102

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

4. pooja195

Ok :) @misssunshinexxoxo @Compassionate @chmvijay

5. pooja195

I think you have it right :/

6. bruno102

Thank you I hope so!

7. pooja195

:)

8. bruno102

@Ciarán95

9. Elsa213

What do you think the answer is?

10. pooja195

They put C

11. pooja195

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

12. Elsa213

e.e

13. Elsa213

I think you are correct, Bruno102.

14. bruno102

Thank you!

15. iYuko

Convert the 128g into moles

16. bruno102

17. iYuko

You tell me.

18. iYuko

Multiply that by 2 then convert it to a mass

19. bruno102

Yes, I think so.

20. bruno102

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

21. pooja195

@iYuko

22. taramgrant0543664

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

23. taramgrant0543664

And I got 90% when I did it

24. bruno102

Thank you so much @taramgrant0543664

25. taramgrant0543664

No problem!