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Chemistry
Chemical Reactions
Oxidation-Reduction Reactions
(Fes + H2o2→feo+ so2 ) it is a ph <7 the solustion of baleching
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4 FeS(s) + 7 O2(g) ==> 2 Fe2O3(s) + 4 SO2(g)
7.82 moles of FeS are required to produce 3.91 moles of Fe2O3 What is the maximum
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The problem here is "liters" of Fe2O3? and Liters of FeS? These are not gases, and something is
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75 grams of SO2? 4 FeS + 7 O2 → 2 Fe2O3 + 4 SO2
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You need to learn how to ask a question. Do you want to know how much FeS is needed to produce 75
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How many grams of O2 would be required to produce 75 grams of SO2
Reaction: 4 FeS + 7 O2 --> 2 Fe2O3 + 4 SO2
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how many moles of SO2 in 75g? It takes 7/4 that many moles of O2 convert that back to grams.
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Given the following standard reduction potentials,
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5.6g of iron metal Fe are heated strong and mixed with 8g of sulfur S to form 4.4g of iron(ll) sulfide FeS. a, identify the
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Choose the correct formula for:
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The correct formula is: Fe2O3 + CO -> Fe + CO2
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How many grams of Fe are in 6.6 g FeO. (Remember the percent Fe in FeO is the grams of Fe in 100 g of FeO)
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Determine percent Fe, then (%/100) x 6.5g = ?
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1. Al + Pb(NO3)2 ----> Al(NO3)3 + Pb
2. FeS + O2 ----> Fe2O3 + SO2 3. C3H8 + O2 ----> CO2 + H2O I need some help balancing these
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Trial and error. Here is how you go about the first one. Rule 1. You must balance ONLY by changing
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Can Fe2+ and Mn2+ be separated by precipitating FeS(s) and not MnS(s)? Assume [Fe2+]=[Mn2+]=[H2S]=0.10 M. Choose a [H3O+] that
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