SO3(g) can be produced by this two step process: 1.) 2FeS2 + 1 1/2 O2 =...

SO3(g) can be produced by this two step process:

1.) 2FeS2 + 1 1/2 O2 = Fe2O3 + 4SO2

2.) SO2 + 1/2 O2 = So3

How many grams of SO3 can be produced from the reaction of 45.0 g of FeS2 if there is no experimental error? How many grams would actually be measured if reaction 1 had 100% yield and reaction 2 had 83.4% yield?

Solutions

Expert Solution

2 FeS2 + 1 1/2 O2 -------------> Fe2O3 + 4 SO2

240 g 256.2 g

45.0 g ??

mass of SO2 produced = 45.0 x 256.2 / 240

= 48.1 g

SO2 + 1/2 O2 ------------> So3

64.06 g 80.06 g

48.06 g ??

mass of SO3 produced = 48.06 x 80.06 / 64.06

mass of SO3 produced = 60.1 g

% yield = actual / theoretical ) x 100

83.4 = Actual / 60.1 ) x 100

Actual yield = 50.1 g

queen_honey_blossom answered 1 year ago

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