The following reactions all occur in a blast furnace. Which...

The following reactions all occur in a blast furnace. Which of these are redox reactions? (a) $3 \mathrm{Fe}_{2} \mathrm{O}_{3}(s)+\mathrm{CO}(g) \longrightarrow 2 \mathrm{Fe}_{3} \mathrm{O}_{4}(s)+\mathrm{CO}_{2}(g)$ (b) $\mathrm{Fe}_{3} \mathrm{O}_{4}(s)+\mathrm{CO}(g) \longrightarrow 3 \mathrm{FeO}(s)+\mathrm{CO}_{2}(g)$ (c) $\mathrm{FeO}(s)+\mathrm{CO}(g) \longrightarrow \mathrm{Fe}(l)+\mathrm{CO}_{2}(g)$ (d) $\mathrm{C}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)$ (e) $\mathrm{C}(s)+\mathrm{CO}_{2}(g) \longrightarrow 2 \mathrm{CO}(g)$ (f) $\mathrm{CaCO}_{3}(s) \longrightarrow \mathrm{CaO}(s)+\mathrm{CO}_{2}(g)$ (g) $\mathrm{CaO}(s)+\mathrm{SiO}_{2}(s) \longrightarrow \mathrm{CaSiO}_{3}(l)$

The following reactions all occur in a blast furnace. Which of these are redox reactions?
(a) $3 \mathrm{Fe}_{2} \mathrm{O}_{3}(s)+\mathrm{CO}(g) \longrightarrow 2 \mathrm{Fe}_{3} \mathrm{O}_{4}(s)+\mathrm{CO}_{2}(g)$
(b) $\mathrm{Fe}_{3} \mathrm{O}_{4}(s)+\mathrm{CO}(g) \longrightarrow 3 \mathrm{FeO}(s)+\mathrm{CO}_{2}(g)$
(c) $\mathrm{FeO}(s)+\mathrm{CO}(g) \longrightarrow \mathrm{Fe}(l)+\mathrm{CO}_{2}(g)$
(d) $\mathrm{C}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)$
(e) $\mathrm{C}(s)+\mathrm{CO}_{2}(g) \longrightarrow 2 \mathrm{CO}(g)$
(f) $\mathrm{CaCO}_{3}(s) \longrightarrow \mathrm{CaO}(s)+\mathrm{CO}_{2}(g)$
(g) $\mathrm{CaO}(s)+\mathrm{SiO}_{2}(s) \longrightarrow \mathrm{CaSiO}_{3}(l)$

Key Concepts

Reduction Processes in Metallurgy

In processes such as those occurring in a blast furnace, reduction reactions are fundamental for extracting metals from their ores. These reactions involve a reducing agent that removes oxygen from metal oxides, converting them into their elemental or lower oxidation state forms.

Reaction Classification

Classifying reactions involves determining whether electron transfer occurs during the transformation of reactants to products. This classification distinguishes redox reactions from other types, such as decomposition or combination reactions, where no change in oxidation states is observed.

Oxidation States

The oxidation state is a number assigned to an element in a compound that indicates the degree of oxidation or electron loss. Tracking changes in oxidation states is a key method for identifying redox reactions, as any change signifies electron transfer.

Redox Reactions

A redox reaction involves the transfer of electrons between chemical species, leading to a change in the oxidation states of the elements involved. This concept is crucial since it helps determine which reactions in a series involve oxidation, reduction, or both.

Transcript

00:02 Okay, so a redox reaction happens when there's a change in the oxidation state of an element within the reaction.

00:09 So from this rule, we can take a look at each reaction formula individually and determine if they are redox reaction or not.

00:18 So from the question a, 3f .e .203 plus carbon monoxide will generate fe304.

00:31 Plus co2.

00:33 So here for the fe203, generally oxygen will have negative 2 oxidation state.

00:43 Thus, the fe here will have plus 3 oxidation state.

00:49 And the oxygen here also will have negative to oxidation state, and carbon here will have positive to oxidation state.

00:59 However, in fe 304, the oxygen same has negative 2 oxidation state.

01:10 However, the fe here, some of them will have positive 3 oxidation state, but some of them will have plus 2 oxidation state.

01:33 And for the carbon dioxide, again, oxygen have negative 2 oxidation state.

01:40 Carbon here has positive four oxidation state because there are two oxygen now in carbon dioxide.

01:48 So from here we can see that the oxidation state of carbon changes in the reaction and the oxidation state of the iron also changes within the reaction.

02:02 So because of that it is a redox reaction.

02:10 For b, as i have mentioned before, the iron here, some of them have the plus 2 oxidation state, some has plus 3 oxidation state.

02:26 And the carbon here is positive 2 oxidation state.

02:34 However, for feo, because of the molar ratio of iron and oxygen are 1 to 1.

02:41 So the iron here has positive 2 oxidation state, while the oxygen has negative to oxidation state.

02:49 And the carbon here again has positive 4 oxidation state as in carbon dioxide.

02:58 So again in this reaction, the oxidation state of iron changes from plus 3 to plus 2, and the carbon oxidation state also changes from plus 2 to plus 4.

03:13 So it is a redox reaction as well...

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