Thermodynamic and Electrochemical Principles

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?

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?

If for the cell reaction,

$\text{Zn}+{\text{Cu}}^{2+}\rightleftharpoons \text{Cu}+{\text{Zn}}^{2+}$

entropy change, $\Delta {\text{S}}^{\circ }$is ${\text{96.5 J mol}}^{-1}{K}^{-1}$, then the temperature coefficient of the emf of a cell is

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