Removing SO2 will shift the equilibrium to the left to produce more SO2, 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, which is the right side (2 moles of SO3).

Increasing the pressure will shift the equilibrium towards the side with fewer moles of gas, which is the right side in this case (2 moles of SO3).

Increasing the concentration of a reactant shifts the equilibrium position to the right, favoring the formation of products (SO3).

Removing SO3 will shift the equilibrium to the right to produce more SO3, according to Le Chatelier's principle.

From the stoichiometry, 3 moles of A produce 4 moles of C. Therefore, 6 moles of A will produce (6 moles A) x (4 moles C / 3 moles A) = 8 moles of C.

According to the stoichiometry, 2 moles of NH3 require 1 mole of N2. Therefore, 6 moles of NH3 will require 3 moles of N2.

Hydrogen (H) is oxidized as it goes from an oxidation state of 0 to +1 in NH3.

According to the stoichiometry, 4 moles of Al produce 2 moles of Al2O3. Therefore, 12 moles of Al will produce (12/4) x 2 = 6 moles of Al2O3.

8 g of Fe = 0.143 moles. 4 moles of Fe produce 2 moles of Fe2O3, so 0.0715 moles of Fe2O3 = 0.0715 * 160 g = 11.44 g.

From the balanced equation, 3 moles of O2 react with 4 moles of Fe. Therefore, 6 moles of O2 will require (4/3) * 6 = 8 moles of Fe.

From the balanced equation, 4 moles of Fe produce 2 moles of Fe2O3. Therefore, 12 moles of Fe will produce (12/4) x 2 = 6 moles of Fe2O3.

From the stoichiometry, 4 moles of Fe produce 2 moles of Fe2O3. Therefore, 12 moles of Fe will produce (12/4) x 2 = 6 moles of Fe2O3.

In Fe2O3, iron has an oxidation state of +3.

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

Removing H2 will shift the equilibrium to the left to produce more H2, according to Le Chatelier's principle.

Removing H2 will shift the equilibrium to the left to produce more H2, thus favoring the reactants.

Removing H2 will shift the equilibrium to the left to produce more H2, according to Le Chatelier's principle.

Decreasing the volume increases the pressure, which shifts the equilibrium to the side with fewer moles of gas, favoring the production of CH3OH.

Decreasing the volume increases the pressure, and the equilibrium will shift towards the side with fewer moles of gas, which is the left side in this case.

Decreasing the volume increases the pressure, and the equilibrium will shift to the side with fewer moles of gas, which is the left side in this case.

If the reaction is exothermic, increasing the temperature will shift the equilibrium to the left, favoring the reactants.

In CO2, the oxidation state of carbon is +4.

'a' accounts for the attractive forces between molecules, while 'b' accounts for the volume occupied by the gas molecules.

The first law of thermodynamics states that energy cannot be created or destroyed, only transformed from one form to another.

The first law of thermodynamics states that energy cannot be created or destroyed, only transformed from one form to another.

Enthalpy is defined as H = U + PV, where U is internal energy, P is pressure, and V is volume.

A phase change of π occurs when a wave reflects off a denser medium.

Using Heron's formula, s = (7 + 24 + 25)/2 = 28. Area = √[s(s-a)(s-b)(s-c)] = √[28(28-7)(28-24)(28-25)] = √[28*21*4*3] = 84.

Using the Law of Cosines: BC² = AB² + AC² - 2 * AB * AC * cos(A) = 10² + 6² - 2 * 10 * 6 * (√3/2) = 100 + 36 - 60√3. BC = √(100 + 36 - 60√3) ≈ 7 cm.