In which condition(s) can I get this reaction:
Fe + H2SO4 = Fe2(SO4)3 + H2
You want to oxidize Fe directly from zero state to +3 state, and reduce the H+1 to zero.
So look at the REdox potentials.
http://chemwiki.ucdavis.edu/Analytical_Chemistry/Electrochemistry/Using_Redox_Potentials_to_Predict_the_Feasibility_of_Reactions
The reaction between iron (Fe) and sulfuric acid (H2SO4) will occur under specific conditions. In this case, it is a redox reaction where Fe is oxidized and H2SO4 is reduced. To determine the conditions under which the reaction occurs, we need to consider the reactivity of the elements and the availability of the reactants.
First, let's look at the reactivity of iron (Fe). Iron is a moderately reactive metal and can react with acids. However, it reacts slowly with cold dilute acids like sulfuric acid. To promote the reaction, we need to increase the temperature or concentration of the acid.
Secondly, we have sulfuric acid (H2SO4). It is a strong acid that can readily donate protons (H+ ions). When sulfuric acid dissociates, it forms H+ ions and sulfate ions (SO4^2-). These ions will take part in the reaction.
Given that Fe reacts slowly with cold dilute acids, we can increase the temperature or concentration of the acid to facilitate the reaction. By increasing the temperature, the particles have more kinetic energy, collide more frequently and with greater force, leading to a higher chance of successful collisions.
Similarly, increasing the concentration of sulfuric acid provides a greater number of H+ ions, which can react with iron more readily. Increasing the concentration also helps overcome the slower reaction rate of Fe.
Therefore, to ensure the reaction between Fe and H2SO4 takes place, you can increase the temperature or concentration of sulfuric acid. However, it is important to handle concentrated sulfuric acid with caution as it is highly corrosive and can cause severe burns.