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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%
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%

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pooja195
 one year ago
Best ResponseYou've already chosen the best response.0Im 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 :)

bruno102
 one year ago
Best ResponseYou've already chosen the best response.1Hmm, I think I have it correct, but if you could tag someone, that would be helpful :)

pooja195
 one year ago
Best ResponseYou've already chosen the best response.0Ok :) @misssunshinexxoxo @Compassionate @chmvijay

pooja195
 one year ago
Best ResponseYou've already chosen the best response.0I think you have it right :/

Elsa213
 one year ago
Best ResponseYou've already chosen the best response.0What do you think the answer is?

pooja195
 one year ago
Best ResponseYou've already chosen the best response.0\(\color{blue}{\text{Originally Posted by}}\) @bruno102 My answer is C \(\color{blue}{\text{End of Quote}}\) .

Elsa213
 one year ago
Best ResponseYou've already chosen the best response.0I think you are correct, Bruno102.

iYuko
 one year ago
Best ResponseYou've already chosen the best response.1Convert the 128g into moles

bruno102
 one year ago
Best ResponseYou've already chosen the best response.1@iYuko my answer isn't correct?

iYuko
 one year ago
Best ResponseYou've already chosen the best response.1Multiply that by 2 then convert it to a mass

bruno102
 one year ago
Best ResponseYou've already chosen the best response.1@iYuko what should I do after I convert it to a mass?

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.1What 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

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.1And I got 90% when I did it

bruno102
 one year ago
Best ResponseYou've already chosen the best response.1Thank you so much @taramgrant0543664
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