Advertisements
Advertisements
प्रश्न
Reduction of metal oxide to metal becomes easier if the metal obtained is in liquid state. Why?
Advertisements
उत्तर
Entropy of a metal in the liquid state is higher than that of the same metal in the solid state (Sliquid > Ssolid). So, when the metal formed is in the liquid state and the metal oxide being reduced is in the solid state, the value of entropy change (ΔS) for the reduction reaction is more on the positive side. When the value of TΔS increases and that of ΔH remains the same, the value of ΔGr° for the reduction reaction becomes negative and thus reduction becomes easier.
APPEARS IN
संबंधित प्रश्न
Explain calcination with reactions.
What is the process in which concentrated ore is reduced to the corresponding metal by heating at high temperature with a reducing agent?
(a) Polling
(b) Pyrometallurgy
(c) Hydrometallurgy
(d) Calcination
Which one of the following oxidation state of Manganese is unstable?
(a) + 2
(b) + 4
(c) + 5
(d) + 7
Complete the given chemical equations
`F_2 + 2Cl^(-)`
What is the action of carbon on the following metal oxides:
Fe2O3 in the blast furnace
What is the action of carbon on the following metal oxides :
ZnO in the vertical retort furnace
An element X (molar mass = 60 g mol−1) has a density of 6.23 g cm−3. Identify the type of cubic unit cell, if the edge length of the unit cell is 4 ✕ 10−8 cm.
Which of the following reactions is an example of autoreduction?
At temperatures above 1073 K coke can be used to reduce \[\ce{FeO}\] to \[\ce{Fe}\]. How can you justify this reduction with Ellingham diagram?
Why are sulphide ores converted to oxide before reduction?
