In a zero-order reaction, the concentration of reactants decreases linearly with time.

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

Decreasing the volume increases the pressure, and according to Le Chatelier's principle, the equilibrium will shift towards the side with fewer moles of gas, which is the right side in this case.

Increasing the concentration of B will shift the equilibrium to the left to produce more A, 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).

Kp is expressed in terms of partial pressures, so for the reaction, Kp = (P_NH3)^2 / (P_N2)(P_H2)^3.

Kp is expressed in terms of the partial pressures of the gases involved in the reaction. For this reaction, Kp = (P_NH3)^2 / (P_N2)(P_H2)^3.

Decreasing the volume increases the pressure, and the equilibrium will shift towards the side with fewer moles of gas. Here, it shifts to the right, producing more C.

The equilibrium constant Kc is given by the expression Kc = [C]^3 / ([A]^2[B]), where the concentrations are raised to the power of their coefficients.

Boiling point elevation = i * Kb * m = 1 * 0.52 * 0.5 = 0.26 °C, so change = 0.52 °C.

Vapor pressure lowering = X_solute * P0 = (0.5 / (0.5 + 55.5)) * P0 ≈ 0.25 P0.

Vapor pressure lowering = (moles of solute / moles of solvent) * P0 = (0.5 / 55.5) * P0 ≈ 0.25 P0.

Molality (m) = moles of solute / kg of solvent. Assuming 1 L of water = 1 kg, molality = 0.5 moles / 1 kg = 0.5 m.

Freezing point depression (ΔTf) = i * Kf * m = 1 * 1.86 °C kg/mol * 1 mol/kg = 1.86 °C.

For the reverse reaction, Kc is the reciprocal of the forward reaction. Therefore, Kc (reverse) = 1/Kc (forward) = 1/10 = 0.1.

ΔTf = Kf * m; -5 = -1.86 * m; m = 5 / 1.86 = 2.68 m.

Freezing point depression = i * Kf * m = 2 * 1.86 °C kg/mol * 1 mol/kg = 3.72 °C. Thus, freezing point = 0 - 3.72 = -3.72 °C.

Using Raoult's Law: P_solution = X_solvent * P_solvent. X_solvent = P_solution / P_solvent = 80/100 = 0.8, thus X_solute = 1 - X_solvent = 0.2.

Relative lowering of vapor pressure = (P° - P) / P° = (100 - 80) / 100 = 0.2.

In a body-centered cubic (BCC) structure, there are 2 atoms per unit cell (1 from the center and 1 from the corners).

Activation energy is the minimum energy required to initiate a chemical reaction.

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

In a concentration cell, the electrodes are made of the same metal but have different concentrations of the electrolyte.

In a concentration cell, the two half-cells have the same electrodes but different concentrations of the electrolyte.

The arrangement of particles in a crystal lattice is primarily determined by intermolecular forces, which dictate how particles pack together.

Increasing the concentration of a reactant will shift the equilibrium position to the right, favoring the formation of products.

According to Le Chatelier's principle, increasing the concentration of products will shift the equilibrium to the left, favoring the formation of reactants.

According to Le Chatelier's principle, increasing the concentration of reactants will shift the equilibrium position to the right to produce more products.

For an exothermic reaction, increasing the temperature shifts the equilibrium to the left, favoring the reactants.

For an exothermic reaction, increasing the temperature shifts the equilibrium to the left, favoring the reactants.