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11 Οκτ 2015 · You could replace $\ce{H2SO4}$ with $\ce{HCl}$ and get the same reaction. In the second equation, the same oxidation of $\ce{Fe}$ to $\ce{Fe^2+}$ by $\ce{H+}$ also occurs. However, on top of that, some of the $\ce{SO4^2-}$ ions are reduced to $\ce{SO2}$, and some of the $\ce{Fe^2+}$ is further oxidised to $\ce{Fe^3+}$. Clearly, in the dilute ...
24 Σεπ 2019 · Can concentrated (18 M) $\ce{H2SO4}$ oxidize $\ce{Fe^2+}$ to $\ce{Fe^3+}?$ Or does it actually block the oxidation? I read in some forum somewhere that in order to prevent $\ce{Fe^2+}$ from being oxidized, one should acidify the solution. I don't know if that's the reason why we added $\ce{H2SO4}$ in our $\ce{Fe^2+}$ solution. But then again ...
14 Ιουν 2021 · 1. It is commonly taught in chemistry textbooks that metals such as Fe, Al, Cr F e, A l, C r is "passivated" in cold concentrated HX2SOX4 H X 2 S O X 4 and HNOX3 H N O X 3 due to them forming oxide films on the surface that prevents the bulk metal from reacting further. However, all those metals can dissolve in dilute solutions of the ...
22 Μαΐ 2024 · The chemical equation provided is: Fe + H2SO4 -> H2 + FeSO4. This equation represents the reaction of iron (Fe) with sulfuric acid (H2SO4) to produce hydrogen gas (H2) and iron(II) sulfate (FeSO4).
4 Νοε 2016 · My working so far is: There must be the same number of of FeSX2 F e S X 2. as Fe(OH)X3 F e (O H) X 3. There must be twice as many HX2SOX4 H X 2 S O X 4. as FeSX2 F e S X 2. If there is one mole of FeSX2 F e S X 2. for example, there must be 1 mole of Fe(OH)X3 F e (O H) X 3. and two moles of HX2SOX4 H X 2 S O X 4.
3 Απρ 2021 · The reduction of water is also unfavored, but is driven forward by the consumption of OH $^-$ ions by precipitation by Fe $^+$$^3$, which also keeps the Fe $^+$$^3$ low. LeChatelier predicted as much: by increasing the acidity, you reduce the availability of electrons from OH $^-$ , and O $_2$ is more able to take electrons from Fe $^+$$^2$ .
11 Σεπ 2015 · $$\ce{KMnO4 + FeSO4 + H2SO4 -> K2SO4 + MnSO4 + Fe2(SO4)3 + H2O}$$ I found out that manganese is reduced as the oxidation number goes from $+7$ to $+2$ and iron gets oxidized as the oxidation number goes from $+2$ to $+3$ .
22 Μαρ 2024 · FeClX2 +HX2SOX4 FeSOX4 +HCl F e C l X 2 + H X 2 S O X 4 F e S O X 4 + H C l. I dissolved the FeCl2 crystal in water, added equivalent amount of H2SO4 to react with all Fe (No excess) and increased the temperature to 40 C and 90 C (separate experiments). But the yield at 40 C is 70% and at 90 C is less than 30%.
17 Ιουλ 2020 · a) After the dissolution of a $\pu{0.4 g}$ portion of rust, the total concentration of iron(III) in a $\pu{100 mL}$ portion of solution is $\displaystyle\frac{\pu{0.4 g}}{\pu{107 g mol-1}\times\pu{0.1 L}} = \pu{0.037 M}.$ As there are no competing reactions (sulfate ion does not form stable complexes with iron), it is easy to find the minimal ...
8 Αυγ 2015 · The sulphate ions will be solvated by hydrogen bonding with the water and the iron ions will form the hexaaquairon(III) complex, $\ce{[Fe(H2O)6]^{3+}}$. As @Mithoron mentioned, the $\ce{Fe^{3+}}$ ions cannot easily be further oxidised so no additional reaction takes place.
