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Silver sulfide is formed by Ag and hydrogen sulfide not sulfur dioxide. You need reducing conditions where the latter can be reduced to
$$\ce{SO2 +reduction -> H2S}$$
Actually, sulfur dioxide chemisorbs on ultraclean silver surface, however heating can remove it. So this is reversible sorption, as suggested by Lassiter [1].
Just note that Auger ...
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Theoretical part
Chrome alum $\ce{KCr(SO4)2 * 12 H2O}$ is synthesized according to the following reaction (average oxidation numbers are shown above the elements undergoing redox reaction):
$$\ce{K2\overset{+6}{Cr}_2O7 + 3 \overset{-2}{C}_2H5OH + 4 H2SO4 →[15-40~°C] K2SO4 + \overset{+3}{Cr}_2(SO4)3 + 3 \overset{-1}{C}_2H4O + 7 H2O}$$
after joint ...
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I'm not familiar with selenium chemistry but am trying to help with the oxidation reaction of selenourea with hydrogen peroxide part. Here what I found on that reaction in literature (Ref.1):
Abstract: Reactions of biological oxidizing agents, such as hydroxyl radicals ($\ce{^•OH}$), singlet oxygen ($\ce{^1O2}$), hydrogen peroxide ($\ce{H2O2}$), and ...
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Given the problem as stated, you did the problem correctly. However I would have done it a bit differently to make it easier to check. I like to do the problems in steps. I also dislike carrying a lot of fractions in intermediate calculations since I get confused easily. (This is basically M. Farooq's answer with some explanation.)
Given
$$\ce{2FeS2 + 11/...
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Note the following relations from the equation you wrote:
1 mol $\ce{FeS2}$ = (11/4) mol $\ce{O2}$;
1 mol $\ce{FeS2}$ = (1/2) mol $\ce{Fe2O3}$;
1 mol $\ce{FeS2}$ = 2 mol $\ce{SO2}$.
You already determined that $\ce{FeS2}$ is the limiting reactant because we have 600/120 mol of iron sulfide and 800/32 mol of $\ce{O2}$;
This implies that 5 mol $\ce{FeS2}$ ...
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