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In the welding of railway tracks, a prop...

In the welding of railway tracks, a proper proportion of aluminium powder and iron (iii) oxide are made to react with each other at high temperature. Explain the type of reaction involved and also identify the reducing and the oxidizing agents.

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(i) Given the formula of iron (III) oxide.
(ii) Reaction between Al and iron (III) oxede.
(iii) Based on the above chemical reaction, predict the type of reactions.
(iv) Identification of oxidizing and reducing agents.
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Despite the fact that aluminium is a reactive metal, it is a stable in air as well as in water. This is due to the formation of thin layer of oxide on the surface of aluminium metal which makes it passive for further attack. The layer is so useful, that in industry, it is purposely deposited by an electrolytic process called anodising. Reaction of aluminium with oxygen is highly exothermic and is called thermite reaction. 2Al_((s)) +(3)/(2) O_(2(g)) rarr Al_(2)O_(3(s)) Delta_(f) H^(Ө) = -1670 kJmol^-1 This reaction finds application for welding of metal and in the metallurgical extraction of many metals from their oxides. The limitation is that to start the reaction, high temperature is required for which an ignition mixture is required. Which of the following metals cannot be extracted by using Al as a reducing agent ?

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Determining the directiom of spontaneity from electrode pot Na^(+)(aq.) + e^(-) rarr Na(s) E^(@) = -2.71 V entials : Predict from Table 3.1, whether Pb^(2+)(aq.) can oxidize Al(s) or Cu(s) under standard conditions. Calculate E^(ɵ) for each reaction at 25^(@)C . Strategy: To predict whether a redox reaction is spontaneous, remember that an oxidizing agent can oxidize any reducing agent that lies below it in the table but can't oxidize one that lies above it. Alternatively, write the expected reaction. Find the oxidizing agents in the equations, one is on the left side and the other on the right side. Locate these oxidizing agents in a table of electrode potentials (the oxidizing agent is on the left side of the reduction half-reaction). The stronger oxidizing agent is the one involved in the half-reaction with the more positive standard electrode potential.

Despite the fact that aluminium is a reactive metal, it is a stable in air as well as in water. This is due to the formation of thin layer of oxide on the surface of aluminium metal which makes it passive for further attack. The layer is so useful, that in industry, it is purposely deposited by an electrolytic process called anodising. Reaction of aluminium with oxygen is highly exothermic and is called thermite reaction. 2Al_((s)) +(3)/(2) O_(2(g)) rarr Al_(2)O_(3(s)) Delta_(f) H^(Ө) = -1670 kJmol^-1 This reaction finds application for welding of metal and in the metallurgical extraction of many metals from their oxides. The limitation is that to start the reaction, high temperature is required for which an ignition mixture is required. Thermite mixture used for welding is

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