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 work done by the gas during a reversible isothermal expansion is given by W = nRT ln(Vf/Vi).

Decreasing the volume increases the pressure, which shifts the equilibrium towards the side with fewer moles of gas.

In a zero-order reaction, the rate is independent of the concentration of the reactants, meaning it remains constant regardless of concentration.

In a zero-order reaction, the rate is constant and does not depend on the concentration of the reactants.

In a zero-order reaction, the rate is constant and the concentration of the reactant decreases linearly with time.

In a zero-order reaction, the rate is independent of the concentration of the reactant, thus it remains constant.

In a zero-order reaction, the rate is independent of the concentration of the reactant, thus it remains constant.

The anode is the site of oxidation where electrons are released.

In an endothermic reaction, the system absorbs heat, resulting in an increase in enthalpy (ΔH > 0).

In an endothermic reaction, heat is absorbed, resulting in a positive change in enthalpy (ΔH > 0).

Increasing the temperature of an exothermic reaction shifts the equilibrium to the left, favoring the reactants, as the system attempts to absorb the added heat.

In an exothermic reaction, the system releases heat, resulting in a decrease in enthalpy (ΔH < 0).

According to Boyle's Law, P1V1 = P2V2; if V doubles, P halves.

In an isothermal process, the temperature remains constant, which means the internal energy of an ideal gas does not change.

The salt bridge maintains charge balance by allowing ions to flow between the two half-cells, preventing charge buildup.

The cathode is the site of reduction in electrochemical cells.

Electrochemical sensors measure current as a response to the concentration of analytes, which is related to the electrochemical reaction occurring.

The Nernst equation relates the cell potential to the concentrations of the reactants and products, allowing for calculation of voltage under non-standard conditions.

Faradaic current refers to the current associated with redox reactions occurring at the electrode surface.

In electrolysis, reduction occurs at the cathode.

During electrolysis, ions in the electrolyte are oxidized or reduced at the electrodes, leading to chemical changes.

During electrolysis, hydrogen gas is produced at the cathode when water is electrolyzed.

In electrolysis, reduction occurs at the cathode as electrons are gained.

In electroplating, metal ions in the solution are reduced at the cathode, depositing metal onto the surface.

The anode is where the oxidation of the fuel occurs, releasing electrons that flow through an external circuit.

The wave function describes the probability distribution of a particle's position in quantum mechanics.