Problem :
If the percent yield of the following equation is 55%,
how many moles of H2SO4 are produced when 44.8 L
of SO3 are combined with excess water?
| SO3(g) + H2O(l)→H2SO4(aq) |
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The equation is balanced, so convert to moles.
 = 2 moles SO3(g) |
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Now calculate the theoretical yield. How many moles of
H2SO4(aq) should we get?
 = 2 moles H2SO4(aq) |
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Now solve algebraically for the actual yield.
| 55% = 0.55 = Actual Yield/(2 moles H2SO4(aq)) | | |
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| 2 moles H2SO4(aq)×0.55 = 1.1 moles H2SO4(aq) | | |
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