Chemistry

Siderite – FeCO₃ (ore of iron)

Calamine – ZnCO₃ (ore of zinc)

Malachite – CuCO₃.Cu (OH)₂ (ore of copper)

Cryolite – Na₃AlF₆ (ore of aluminium)

It happens in reversible reactions when the rate of the forward reaction becomes equal to the rate of the backward reaction. Result in the same concentration of reactants and product.

If the conditions of equilibrium are changed, it shifts to oppose the change. For example, in Haber's process, high pressure favors NH? formation.

The equilibrium constant is the ratio of the concentrations of products to reactants, each raised to the power of their stoichiometric coefficients. For reversible reactions.

It is aldol condensation.

Number of sp² carbon = 8

CoCl₃.NH₃ + AgNO₃ $\stackrel{}{\to }AgC\mathcal{l}\downarrow \left(2mol\right)$  

$\left[Co{\left(N{H}_3\right)}_{5}C\mathcal{l}\right]C{\mathcal{l}}_2+AgN{O}_3\stackrel{}{\to }AgC\mathcal{l}\downarrow \left(2mol\right)$  

x = 5

$M{n}^{2+}\stackrel{}{\to }{t}_{2g^{111}}{e_g}^{11}$

(Number of unpaired electron = 5)

${\mu }_S=\sqrt[]{35}=5.91\cong 6$

$K=A.e^{-Ea/RT}=\left(6.5*10^2\right)e^{-26000K/T}$

$\frac{Ea}{8.314}=26000$

Ea = 216.164kJ/mol $\cong$ $$ 216

H₂ (g) + Cu²⁺ (aq) $\stackrel{}{\to }$  2H⁺ (aq) + Cu (s)

  $\therefore E_{cell}=E_{cell}^0-\frac{2.303RT}{nf}logQ$

0.31 = 0.34 - $\frac{0.06}{2}log\frac{\left[H^{+}\right]}{C{u}^{2+}}$  

  $\left[C{u}^{2+}\right]=10^{-7}\left(?\left[H^{+}\right]=10^{-3}\right)$

x = 7