Advertisements
Advertisements
Question
In the extraction of copper from its sulphide ore, the metal is formed by the reduction of \[\ce{Cu2O}\] with ______.
Options
\[\ce{FeS}\]
\[\ce{CO}\]
\[\ce{Cu2S}\]
\[\ce{SO2}\]
Solution
In the extraction of copper from its sulphide ore, the metal is formed by the reduction of \[\ce{Cu2O}\] with \[\ce{Cu2S}\].
Explanation:
In the extraction of copper from its sulphide ore, the metal is formed by the reduction of \[\ce{Cu2O}\] with \[\ce{Cu2S}\]. This reaction completes with the process of auto reduction.
Chemical reaction occurring in this reaction is as follows:
\[\ce{Cu2O + 1/2 Cu2S -> 3Cu + 1/2 SO2}\]
In this process, copper appears as blister copper.
APPEARS IN
RELATED QUESTIONS
The reaction,
Cr2O3 + 2Al → Al2O3 + 2Cr
(ΔGθ = -421kJ) is thermodynamically feasible as is apparent from the Gibbs energy value. Why does it not take place at room temperature?
Why is the extraction of copper from pyrites more difficult than that from its oxide ore through reduction?
Write down the reactions taking place in different zones in the blast furnace during the extraction of iron.
How will you convert the following:
Zinc blende to Zinc metal
For the reduction of \[\ce{FeO}\] at the temperature corresponding to point D, which of the following statements is correct?
Explain the following:
Silica is added to the sulphide ore of copper in the reverberatory furnace.
A cuprous ore among the following is:-
Heating of MgCl2 6H2O in absence of HCl gives ______.
Assertion: For the extraction of iron, haematite ore is used.
Reason: Haematite is a carbonate ore of iron.
\[\ce{Au + CN^- + H2O + O2 -> [Au(CN)2]^- + OH^-}\]
The number of CN− ions involved in the balanced equation is ______.
