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In Ellingham diagrams plots of DeltaG (o...

In Ellingham diagrams plots of `Delta`G (oxide formation) show positive slopes except for the formation of CO(g) from coke. Why?

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To understand why the Ellingham diagrams show positive slopes for most oxide formations except for the formation of carbon monoxide (CO) from coke (solid carbon), we can break down the explanation into the following steps: ### Step-by-Step Solution: 1. **Understanding Ellingham Diagrams**: - Ellingham diagrams are graphical representations that plot the Gibbs free energy change (ΔG) for the formation of oxides as a function of temperature. They are used in metallurgy to assess the stability of metal oxides and predict the conditions under which reduction reactions can occur. 2. **Formation of Carbon Monoxide**: ...
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In Ellingham diagrams plots of Delta_(f)G (oxide formation) show positive slope except for the formation of CO(g) from coke. Why ?

In Ellingham diagrams plots of Delta_(f)G (oxide formation) show positive slope except for the formation of CO(g) from coke. Why ?

Ellingham diagrams are plots of DeltaG_(1)^(@) Vs T for the formation of

In Ellingham diagrams of Delta_(1)G oxide formation Vs T , which of the following graphs has negative slope ?

The choice of reducing agent for metal oxide is decided by thermodynamic principles of metallurgy. Delta G must be negative. Ellingham diagram is a plot of Delta_(f)G^(0) vs T for the formation of oxides of various elements. All the plots slope upwards when temperature increases. Each plot is a straight line except when some change in phase takes place. A metal will reduce the oxide of other metals which lie above it in this diagram. At a temperature below 1623 K. Al cannot reduce

The value of Delta H for the combustion of C(s) is - 94.4 Kcal. The heat of formation of CO_(2)(g) is :-

For a sponaneous reaction, the free energy change must be negative, Delta G=Delta H-T Delta S, Delta H is the enthalpy change during the reaction. T is the absolute temperature, and Delta S is the change in entropy during the reaction. Consider a reaction such as the formation of an oxide M+O_(2) to MO Dioxygen is used up in the course of this reaction. Gases have a more random structure (less ordered) than liquid or solids. Consequently gases have a higher entropy than liquids and solids. In this reaction S (entropy or randomness) decreases, hence Delta S is negative. Thus, if the temperature is raised then T Delta S becomes more negative,Since, TDelta S is substracted in the equation, then Delta G becomes less negative. Thus, the free energy change increases with the increase in temperature. The free energy changes that occur when one mole of common reactant (in this case dioxygen) is used may be plotted graphically aginst temperature for a number of reactions of metals to their oxides. The following plot is called an Ellingham diagram for metal oxide. Understanding of Ellingham diagram is extremely important for the efficient extraction of metals. As per the Ellingham diagram of oxides which of the following conclusion is true ?

For a sponaneous reaction, the free energy change must be negative, Delta G=Delta H-T Delta S, Delta H is the enthalpy change during the reaction. T is the absolute temperature, and Delta S is the change in entropy during the reaction. Consider a reaction such as the formation of an oxide M+O_(2) to MO Dioxygen is used up in the course of this reaction. Gases have a more random structure (less ordered) than liquid or solids. Consequently gases have a higher entropy than liquids and solids. In this reaction S (entropy or randomness) decreases, hence Delta S is negative. Thus, if the temperature is raised then T Delta S becomes more negative,Since, TDelta S is substracted in the equation, then Delta G becomes less negative. Thus, the free energy change increases with the increase in temperature. The free energy changes that occur when one mole of common reactant (in this case dioxygen) is used may be plotted graphically aginst temperature for a number of reactions of metals to their oxides. The following plot is called an Ellingham diagram for metal oxide. Understanding of Ellingham diagram is extremely important for the efficient extraction of metals. Which of the following elements can be prepared by heating the oxide above 400^(@)C ?

Which of the following reaction can be used to define the heat of formation of CO_(2)(g) ?

The plot of Delta G versus temperature for the formation of oxides of elements is called

AAKASH INSTITUTE ENGLISH-GENERAL PRINCIPLES AND PROCESSES OF ISOLATION OF ELEMENTS-Assignment (Section-D) Assertion-Reason Type Question
  1. In Ellingham diagrams plots of DeltaG (oxide formation) show positive ...

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  2. A: Cuprite is concentrated by froth floatation process R: Cuprite is ...

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  3. A: Bauxite is purified by leaching process R: Aluminium oxide reacts ...

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  4. A: A: Calamine and Dolomite are the carbonate ores. R: Calamine is Z...

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  5. A: Roasting process is involved in the metallurgy of Cu from Malachite...

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  6. A: Metallurgy of Ag from Argentite is known as hydro-metallurgy R: Ar...

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  7. In the manufacture of iron from hematite, limestone is added to act as...

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  8. A: Ultrapure metals are obtained by zone refining. R: Van arkel metho...

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  9. The purest form of iron is

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  10. A: Magnesium oxide is used for the lining in steel making furnace . R...

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  11. A: Aluminium metal is used as a reducing agent for the extraction of m...

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  12. STATEMENT-1 : Zinc and not copper is used in the recovery of silver fr...

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  13. A: Hydrometallurgy is used for extraction of Ag and Au. R: Hydrometal...

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  14. A: Pure silver is obtained by electrolysis of AgNO3 solution R: In el...

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  15. In blast furnace iron oxide is reduced by

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  16. A:In Hall process Aluminium is purified. B:Al2O3(aq)is used in Hall pr...

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