When compared to $∆G°$ for the formation of $\mathrm{A}{\mathrm{l}}_2{\mathrm{O}}_3$, the $∆G°$ for the formation of $\mathrm{C}{\mathrm{r}}_2{\mathrm{O}}_3$ is

The point of intersection and sudden increase in the slope, in the diagram given below, respectively, indicates:

Given below are two statements.
Statement I: The choice of reducing agents for metals extraction can be made by using the Ellingham diagram, a plot of $\Delta \mathrm{G}$ vs temperature.
Statement II: The value of $\mathrm{\Delta S}$ increases from left to right in the Ellingham diagram.

In the light of the above statements, choose the most appropriate answer from the options given below:

From the Ellingham diagram given below, identify the correct statements
I) Below $673 \mathrm{K}$ CO can reduce FeO to Fe
II) Above $673 \mathrm{K}$ Coke can reduce FeO to Fe
III CO is the strong reducing agent for the reduction of ZnO to Zn above $1073 \mathrm{K}$ than coke
IV) Coke reducs ZnO to Zn readily at $1673 \mathrm{K}$

Given below are two statements: one is labelled as Assertion A and the other is labelled as Reason R

Assertion A: In the Ellingham diagram, a sharp change in slope of the line is observed from $\mathrm{Mg}\to \mathrm{MgO}$ at $~{1120}^{\mathrm{o}}\mathrm{C}$

Reason R: There is a large change of entropy associated with the change of state

In the light of the above statements, choose the correct answer from the options given below

An Ellingham diagram provides information about:

Given below are two statements :

Statement I : According to the Ellingham diagram, any metal oxide with higher $\mathrm{\Delta G}°$ is more stable than the one with lower $\mathrm{\Delta G}°$.

Statement II : The metal involved in the formation of oxide placed lower in the Ellingham diagram can reduce the oxide of a metal placed higher in the diagram.

In the light of the above statements, choose the most appropriate answer from the options given below

Given below are two statements: one is labelled as Assertion A and the other is labelled as Reason $\mathbf{R}$

Assertion A: In an Ellingham diagram, the oxidation of carbon to carbon monoxide shows a negative slope with respect to temperature.

Reason R: CO tends to get decomposed at higher temperature.

In the light of the above statements, choose the correct answer from the options given below

Gibbs energy vs $\mathrm{T}$ plot for the formation of oxides is given below.

For the given diagram, the correct statement is-

For a reaction $4 \mathrm{M}\left(\mathrm{s}\right)+{\mathrm{nO}}_2\left(\mathrm{g}\right)\to 2{\mathrm{M}}_2{\mathrm{O}}_{\mathrm{n}}\left(\mathrm{s}\right)$

The free energy change is plotted as a function of temperature. The temperature below which the oxide is stable could be inferred from the plot as the point at which :