Thermodynamic Principles of Metallurgy

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

Assertion $\mathrm{A}$ : The reduction of a metal oxide is easier if the metal formed is in liquid state than solid state.

Reason $\mathrm{R}$ : The value of ${\mathrm{\Delta G}}^{\mathrm{\Theta }}$ becomes more on negative side as entropy is higher in liquid state than solid state.

In the light of the above statements. Choose the most appropriate answer from the options given below

Given are two statements one is labelled as Assertion and other is labelled as Reason.

Assertion: Magnesium can reduce ${\mathrm{Al}}_2{\mathrm{O}}_3$ at a temperature below $1350 °\mathrm{C}$, while above $1350 °\mathrm{C}$ aluminium can reduce $\mathrm{MgO}$.

Reason: The melting and boiling points of magnesium are lower than those of aluminium.

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

According to the signs of ${∆}_{\mathrm{r}}{\mathrm{G}}^{°}$ for the following reactions: 

${\mathrm{PbO}}_2+\mathrm{Pb}\to 2\mathrm{PbO}, {∆}_{\mathrm{r}}\mathrm{G}°<0$

${\mathrm{SnO}}_2+\mathrm{Sn}\to 2\mathrm{SnO}, {∆}_{\mathrm{r}}\mathrm{G}°>0$

What is the more characteristic oxidation states for lead and tin?

In which of the following reactions, standard reaction entropy change $\left(\mathrm{\Delta S}°\right)$ is positive and standard Gibb's energy change $\left(\mathrm{\Delta G}°\right)$ decreases sharply with increasing temperature?

In the extraction of copper from its sulphide ore the metal is formed by reduction of ${\mathrm{Cu}}_2\mathrm{O}$ with

In which of the following reactions, standard reaction entropy change $\left(\mathrm{\Delta S}°\right)$ is positive and standard Gibb's energy change $\left(\mathrm{\Delta G}°\right)$ decreases sharply with increasing temperature?

Identify the reaction that does not take place in a blast furnace:

In view of the sign of${∆}_{\mathrm{r}}\mathrm{G}°$ for the following reactions :
${\mathrm{PbO}}_2+\mathrm{Pb}\to 2 \mathrm{PbO}; {∆}_{\mathrm{r}}\mathrm{G}°<0$
${\mathrm{SnO}}_2+\mathrm{Sn}\to 2\mathrm{SnO}; {∆}_{\mathrm{r}}\mathrm{G}°>0$ 
Which oxidation states are more characteristic for lead and tin ?

Heating ${\mathrm{Cu}}_{2}0$and ${\mathrm{Cu}}_2\mathrm{S}$ will give:

Calamine, malachite, magnetite and cryolite, respectively are:

Which of the following graph represents correctly the variation in thermodynamic functions during th formation of a binary solution showing positive deviators from ideal behavior?

In the extraction of copper from its sulphide ore the metal is formed by reduction of ${\mathrm{Cu}}_2\mathrm{O}$ with

The purest zinc is made by

The metal oxide reacts with a ______. The oxide is ______ to metal and reducing agent is ______. Net Gibb's energy change is ______.

The reaction ${\mathrm{Cr}}_2{\mathrm{O}}_3+2\mathrm{Al}\to {\mathrm{Al}}_2{\mathrm{O}}_3+2\mathrm{Cr}\left(∆\mathrm{G}°=-\mathrm{ }421\mathrm{ }\mathrm{kJ}\right)$ is thermodynamically feasible due to $-\mathrm{v}\mathrm{e}$ value of $∆G$ . Why does this reaction not take place at room temperature?

Which of the following statements is correct according to the basic concepts of thermodynamics which govern the feasibility of a metallurgical process?

Select the correct statement with respect to metallurgical extraction of a metal from its ore.