Increasing the pressure by decreasing the volume shifts the equilibrium towards the side with fewer moles of gas, according to Le Chatelier's Principle.

Increasing the pressure will shift the equilibrium to the right, favoring the side with fewer moles of gas, according to Le Chatelier's Principle.

Increasing the pressure will shift the equilibrium position towards the side with fewer moles of gas, according to Le Chatelier's Principle.

Increasing the volume decreases the pressure, which shifts the equilibrium towards the side with more moles of gas.

At equilibrium, the concentrations of reactants and products remain constant over time.

According to Le Chatelier's principle, increasing temperature shifts the equilibrium position, which can affect the enthalpy change (ΔH) depending on the reaction.

For endothermic reactions, increasing temperature shifts the equilibrium and increases enthalpy.

At equilibrium, the rate of the forward reaction equals the rate of the reverse reaction.

A catalyst speeds up the rate of both the forward and reverse reactions equally, thus having no effect on the position of the equilibrium.

Decreasing the volume increases the pressure, and according to Le Chatelier's Principle, the equilibrium will shift to the side with fewer moles of gas to counteract the change.

Decreasing the volume increases the pressure, and according to Le Chatelier's Principle, the equilibrium will shift to the side with fewer moles of gas to counteract the change.

If the number of moles of gas is equal on both sides, increasing the pressure has no effect on the equilibrium position.

The rate of the overall reaction is determined by the slowest step, which in this case is A + B -> C, leading to the rate law Rate = k[A][B].

The rate-determining step is the slowest step in the mechanism and thus determines the overall reaction rate.

An intermediate is a species that is formed during the reaction and consumed in subsequent steps, not appearing in the overall reaction.

An intermediate is a species that is produced in one step of a reaction mechanism and consumed in a later step.

The rate-determining step is the slowest step in a reaction mechanism and thus controls the overall rate of the reaction.

Decreasing the temperature in an exothermic reaction (where heat is a product) shifts the equilibrium to the right, favoring the formation of products.

Decreasing the temperature in an endothermic reaction shifts the equilibrium to the left, favoring the formation of reactants as the system seeks to release heat.

Decreasing the temperature in an endothermic reaction shifts the equilibrium to the left, favoring the formation of reactants as the system seeks to release heat.

Increasing the temperature in an endothermic reaction shifts the equilibrium to the right, favoring the formation of products as the system absorbs the added heat.

A positive enthalpy change indicates that the reaction is endothermic, meaning it absorbs heat from the surroundings.

Using the Arrhenius equation and the temperature dependence of the rate constant, Ea can be estimated using the formula Ea = (R * ΔT * ln(2)) / (1/T1 - 1/T2). For a 10°C increase, Ea is approximately 80 kJ/mol.

The saturation concentration is the concentration at which the reaction rate is half of its maximum value.

The overall order is the sum of the exponents in the rate law: 2 (from [A]^2) + 1 (from [B]) = 3.

For a second order reaction, if [A] is doubled, the rate increases by a factor of (2^2) = 4, thus the rate quadruples.

For a first-order reaction, t = (ln([A]0/[A]) / k). Here, [A] = 0.25[A]0, so t = (ln(1/0.25) / 0.03) ≈ 46.2 s.

The change from +7 to +2 indicates a gain of 5 electrons (7 - 2 = 5).

The reducing agent donates electrons and is oxidized in the process.

The substance that is oxidized loses electrons during a redox reaction.