Thermodynamic Principles of Metallurgy

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?

The choice of a reducing agent in a particular case depends on its thermodynamic factor. How do you agree with this statement?

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?

Cold diluted ${\mathrm{H}}_2{\mathrm{SO}}_4$ will completely dissolve:
$\left(\mathrm{i}\right)$ $\mathrm{Pb}$
$\left(\mathrm{ii}\right)$ ${\mathrm{Fe}}_3{\mathrm{O}}_4$
$\left(\mathrm{iii}\right)$ $\mathrm{Fe}$
$\left(\mathrm{iv}\right)$ $\mathrm{Cu}$
$\left(\mathrm{v}\right)$ $\mathrm{Mg}$
$\left(\mathrm{vi}\right)$ $\mathrm{MgO}$
$\left(\mathrm{vii}\right)$ ${\mathrm{CoCO}}_3$
$\left(\mathrm{viii}\right)$ ${\mathrm{CuCO}}_3$
$\left(\mathrm{ix}\right)$ ${\mathrm{SrCO}}_3$

Cold concentrated ${\mathrm{HNO}}_3$ will completely dissolve:
$\left(\mathrm{i}\right)$ $\mathrm{Pb}$
$\left(\mathrm{ii}\right)$ ${\mathrm{Pb}}_3{\mathrm{O}}_4$
$\left(\mathrm{iii}\right)$ $\mathrm{Fe}$
$\left(\mathrm{iv}\right)$ $\mathrm{Sn}$
$\left(\mathrm{v}\right)$ $\mathrm{Mg}$
$\left(\mathrm{vi}\right)$ $\mathrm{MgO}$
$\left(\mathrm{vii}\right)$$\mathrm{Hg}$
$\left(\mathrm{viii}\right)$ $\mathrm{Au}$
$\left(\mathrm{ix}\right)$ $\mathrm{Ag}$
$\left(\mathrm{x}\right)$ $\mathrm{Pt}$

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.