In [Fe(CN)6]3-, the CN- ligand has a charge of -1 and there are six CN- ligands. Therefore, the total negative charge is -6. To balance the -6 charge with the overall -3 charge of the complex, the oxidation state of iron must be +3.

Zinc (Zn) is oxidized to Zn2+, so its oxidation state is +2.

Iron (Fe) is oxidized as it loses electrons to form FeCl3.

Fe2O3 is reduced to Fe, as it gains electrons during the reaction.

Magnesium is oxidized as it loses electrons and its oxidation state increases from 0 to +2.

According to Le Chatelier's principle, decreasing the volume increases the pressure, and the equilibrium will shift towards the side with fewer moles of gas. In this case, the right side has 2 moles of SO3 compared to 3 moles on the left, so the equilibrium shifts to the right.

According to Le Chatelier's principle, increasing the volume of the container decreases the pressure. The equilibrium will shift towards the side with more moles of gas, which is the left side (2 moles of SO2 + 1 mole of O2).

N2 is reduced to NH3 as it gains electrons.

Iron (Fe) is oxidized as it loses electrons to form Fe2O3.

For an exothermic reaction, increasing the temperature shifts the equilibrium to the left (towards the reactants) to absorb the added heat, according to Le Chatelier's principle.

For an exothermic reaction, increasing the temperature shifts the equilibrium to the left, favoring the reactants, as the system tries to absorb the added heat.

Increasing the pressure shifts the equilibrium towards the side with fewer moles of gas, which in this case is the right side (2 moles of NH3).

Copper (Cu) is reduced as it gains electrons from zinc.

Increasing the pressure shifts the equilibrium towards the side with fewer moles of gas. In this case, it shifts to the right, producing more SO3.

Cu is oxidized to Cu2+ as it loses electrons in the reaction.

Zn is oxidized to Zn2+ as it loses electrons.

In C2O4^2-, the oxidation state of carbon is +3.

Adsorption is widely used in water purification processes to remove impurities.

Gas particles have the highest energy compared to solids and liquids, allowing them to move freely and occupy more space.

Particles in a solid have the least amount of energy compared to liquids, gases, and plasma.

In gases, particles move freely and are far apart compared to solids and liquids.

The Arrhenius equation relates the rate constant (k) to temperature (T) and activation energy (Ea).

The half-life of a first-order reaction is independent of the initial concentration and is directly proportional to the rate constant.

For a first-order reaction, the half-life is constant and is given by the formula t1/2 = 0.693/k.

The half-life of a first-order reaction is given by the formula t1/2 = 0.693/k, which shows that it is independent of the initial concentration.

The half-life of a first-order reaction is given by the formula t1/2 = 0.693/k, where k is the rate constant.

In the Langmuir isotherm, the maximum coverage of adsorbate on the adsorbent is referred to as a monolayer.

The Langmuir isotherm assumes that adsorption occurs at specific sites, leading to a monolayer coverage of the adsorbate.

The rate constant of a reaction is affected by the nature of the reactants, temperature, and the presence of catalysts.

Enthalpy refers to the heat content of a system at constant pressure, defined as internal energy plus pressure times volume.