Iron is extracted using a blast furnace. Select the correct options regrarding this process:

Iron formed in the furnace melts below its melting point becuase of the presence of the impurities

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C O_{2}

formed by the combustion of C, reacts with excess coke in the furnace and produces CO

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F e_{2} O_{3}

is reduced by

A l

and produces molten iron

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Limestone get decomposed to CaO which combines with the impurity

S i O_{2}

from the ore

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Solution

The correct option is D Limestone get decomposed to CaO which combines with the impurity $S i O_{2}$ from the ore
a) Iron ore contains silica, phosphorous, aluminium etc as impurities. Thus, the melting point of iron in the furnace is lower than its melting point in its purest form.
b) $C + O_{2} \to C O_{2}$
This is a highly exothermic reaction and acts as a source of heat in the furnace. At high temperatures in the bottom of the furnace, carbon dioxide reacts with coal (C) to give carbon monoxide.
$C O_{2} + C \to 2 C O$
c) No such process follows inside a blast furnace.
d) $C a C O_{3} \to C a O + C O_{2}$
$C a O + S i O_{2} \to C a S i O_{3}$
The calcium silicate formed can be removed as slag.

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